Buku Latihan Kimia f4 2015

8/10/2019 Buku Latihan Kimia f4 2015

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K : Kimia

I : Itu

M : Mudah

I : In Sya Allah / Pasti

A : A+


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Atomic Structure

HAND OUT 1

1. From the above diagram, define diffusion

2. What is the relationship between

A) diffusion and space between particles

. B) diffusion and temperature of particles

C) diffusion and mass of gas particles

..

3. Explain the following observation:

A) Diffusion in gas is faster than diffusion in liquid


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1. Positivelycharged or negativelycharged particles

2. A group of two or more atoms which are chemically

bonded together

3. The smallest particle of an element that can participate ina chemical reaction

4. Made up of tiny and discreet particles

5. Anything that occupies space and mass

6. A process when particles of a substance move in betweenthe particles of another substance

7. A substance that consists of only one type of atom

8 A b t e th t t i t e ele e t th t e

ION MELTING

POINT

MATTERDIFFUSION COMPOUND


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KINETIC THEORY OF MATTER SOLID, LIQUID

OR GAS?

1. The particles are packed closely together in orderly manner

2. Can be compressed easily

3. Particles only vibrate and rotate about their fixed positions

4. Cannot be compressed

5. Particles are far apart from each other and in random motion

6. There are weak force between particles

7 Has fixed volume and shape

8 Does not have a fixed volume and shape

9 Has a fixed volume but no fixed shape

10 Takes the shape of the container

11 Particles are held together by strong forces but weaker than in a

solid

12 P ti l ib t t t d th h t


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HANDOUT 4


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WE LEARN THAT THERE ARE 3 STATES OF MATTER. BUT DO YOU KNOW

THAT ACTUALLY THERE ARE 5 STATES OF MATTER?

Look at the diagram on the right

PLASMA AND BOSE- EINSTEIN CONDENSATE ARE THE 4TH

AND THE 5TH

STATES OF MATTER

PLASMA

Plasmas are a lot like gases, but the atoms are different because they are made up of free

electrons and ions of the element. Northern Lights or ball lightning, are types of plasmas.

FINDING A PLASMA

Inside the long tube of fluorescent light bulb is a gas. Electricity flows through the tube

when the light is turned on. The electricity acts as that special energy and charges up the

gas. This charging and exciting of the atoms creates glowing plasma inside the bulb.

Another example of plasma is a neon sign. The electricity charges the gas, possibly neon,

d t l i id f th t b Th l l i l l d di h t


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HANDOUT 6

The following graph shows the HEATING CURVEof a substance

Using the kinetic theory of matter, explain what happens when the solid is heated

Fill in the blanks with right words in the sentences below.

more energy overcome the temperature gains energy

li d d i h i li id


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SUMMARY

HANDOUT 7

1. Fill in the table below ( Note that the order of discovery is not arranged according to the correct sequence)

Students are requested

1) to draw the atomic models suggested by each scientist 2) To rearrange the ideas according to the correct order of discovery

Scientists Ideas/discovery Draw atomic model Arrangement of

discovery

Democritus All matter is composed of atoms. Atoms cannot be split

into smaller portions There is empty space between atoms Atoms are completely solid Atoms are homogenous (same all the way) , with no

internal structure Atoms are different in their sizes , shapes and weights

J.J. Thomson Discover electrons through cathode rays experiment Electrons are embedded in clouds of positive charges

Describe atoms as a sphere of positive charges whichcontains tiny negative particlesRemember, no protons in the Thomson model

Remember, he did not say that electrons are revolving around

nucleus!


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John

Dalton

All atoms of a given element are identical in size, mass,and other properties.

Atoms of different elements differ in size, mass, and otherproperties.

Atoms cannot be subdivided, created, or destroyed. Atoms of different elements can combine in simple,

whole-number ratios to form compounds. In chemical reactions, atoms are combined, separated, or

rearranged

Atom is tiny impenetrable ball

known as the discoverer of the neutron. He found neutrons the same mass as the proton.

Explain the flaw in Rutherford model of atom Awarded the Nobel Prize in physics in 1935

Werner

Heisenberg

Heisenberg pointed out that it is impossible to know boththe exact position and the exact momentum of an

electron at the same time. This concept, called the Heisenberg Uncertainty

principle, effectively destroys the idea of electrons

traveling around in neat orbits.


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In 1913, Niels Bohr proposed improvement toRutherford atomic model.

Bohr added the idea of fixed orbits, or energy levels forthe electron traveling around the nucleus.

Electrons traveling in neat orbits

Lord Ernest

Rutherford

discovering that most of the atom is made up of "emptyspace."

Electrons move at high speed around nucleus "the greater part of the mass of the atom was

concentrated in a minute nucleus."

Discovered protons

. calculated mass of atom from his model is less thanmass of real atom

Famous for his gold foil experiment.

Note 1 - Answers to worksheet 1

scientists year Ideas/discovery model

1. Democritus BC460-371BC

All matter is composed of atoms. Atoms cannot be splitinto smaller portions There is empty space between atoms Atoms are completely solid Atoms are homogenous (same all the way) , with no

internal structure

Atoms are different in their sizes , shapes and weights


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John

Dalton

1766-1844

All atoms of a given element are identical in size, mass,and other properties.

Atoms of different elements differ in size, mass, and otherproperties.

Atoms cannot be subdivided, created, or destroyed. Atoms of different elements can combine in simple,

whole-number ratios to form compounds. In chemical reactions, atoms are combined, separated, or

rearranged

Atom is tiny impenetrable ball

J.J. Thomson

1856-1940

Discover electrons through cathode rays experiment Electrons are embedded in clouds of positive charges

Describe atoms as a sphere of positive charges whichcontains tiny negative particles

Remember, no protons in the Thomson model

Remember, he did not say that electrons are revolving around

nucleus!

Lord Ernest

Rutherford

1871-1937 discovering that most of the atom is made up of "emptyspace."

Electrons move at high speed around nucleus

"the greater part of the mass of the atom wasconcentrated in a minute nucleus."

Discovered protons

. calculated mass of atom from his model is less thanmass of real atom

Famous for his gold foil experiment.

Negative

electron

Positive

sphere
http://images.google.com/imgres?imgurl=http://www.hcc.mnscu.edu/programs/dept/chem/abomb/Gold_Foil_Exp.jpg&imgrefurl=http://www.hcc.mnscu.edu/programs/dept/chem/abomb/page_id_13691.html&h=325&w=493&sz=36&hl=en&start=4&tbnid=W0WEbH0_KxyKCM:&tbnh=86&tbnw=130&prev=/images?q=Rutherford+gold+foil&svnum=10&hl=en&rls=ITVA,ITVA:2006-48,ITVA:en&sa=Nhttp://images.google.com/imgres?imgurl=http://www.hcc.mnscu.edu/programs/dept/chem/abomb/Gold_Foil_Exp.jpg&imgrefurl=http://www.hcc.mnscu.edu/programs/dept/chem/abomb/page_id_13691.html&h=325&w=493&sz=36&hl=en&start=4&tbnid=W0WEbH0_KxyKCM:&tbnh=86&tbnw=130&prev=/images?q=Rutherford+gold+foil&svnum=10&hl=en&rls=ITVA,ITVA:2006-48,ITVA:en&sa=Nhttp://images.google.com/imgres?imgurl=http://www.hcc.mnscu.edu/programs/dept/chem/abomb/Gold_Foil_Exp.jpg&imgrefurl=http://www.hcc.mnscu.edu/programs/dept/chem/abomb/page_id_13691.html&h=325&w=493&sz=36&hl=en&start=4&tbnid=W0WEbH0_KxyKCM:&tbnh=86&tbnw=130&prev=/images?q=Rutherford+gold+foil&svnum=10&hl=en&rls=ITVA,ITVA:2006-48,ITVA:en&sa=N


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scientists year discovery Model

Niels Bohr

1913-1963

In 1913, Niels Bohr proposed improvement toRutherford atomic model.

Bohr added the idea of fixed orbits, or energy levels forthe electron traveling around the nucleus.

Electrons traveling in neat orbits

James

Chadwick

1891-1974

known as the discoverer of the neutron. He found neutrons the same mass as the proton. Explain the flaw in Rutherford model of atom

Awarded the Nobel Prize in physics in 1935

Werner

Heisenberg

1901-1976 Heisenberg pointed out that it is impossible to know boththe exact position and the exact momentum of anelectron at the same time.

This concept, called the Heisenberg Uncertaintyprinciple, effectively destroys the idea of electrons

traveling around in neat orbits.

The Charge-Cloud Model


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HANDOUT 8 ( MATCHING DISCOVERIES AND NAME OF SCIENTISTS)

Match the following ideas with the names of scientists in the box above

1. Atoms are of different size, shape and weight .2. Atom is a small indivisible matter like a tiny ball ..3. Discovered electrons 4. Proposed that atom is a sphere of positive charges that that contains tiny negative particles like plum pudding model

.

5. Discovered protons 6. Most of an atom consists of an empty space ..7. Positive charge only concentrated in a small , central region .8. Proposed that protons are small central nucleus with electrons revolve around

9. Famous for gold foil experiment .10.Calculated that mass of atom is less than mass of real atom 11.Proposed that electrons moved in shells around nucleus ..12.Proposed electrons traveling in fixed orbits ..13.Proved the existence of neutrons ..

14.Calculated that mass of proton is about the same as mass of neutron 15.Proposed charge cloud model of atom ..16.Impossible to know exact positions of electrons in atom 17.

Democritus John Dalton Werner Heisenberg

James Chadwick Niels Bohr Lord Ernest Rutherford

J.J. Thomson


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HANDOUT 9 ( MATCHING ATOMIC MODELS AND NAME OF SCIENTISTS)

Below are atomic model of atoms . Write down names of the scientists who proposed the ideas of the models.

ATOMIC MODELS SCIENTISTS

1

2

3

4


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5

6

7


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HANDOUT 10

1. Fill in the table below

SYMBOL RELATIVE

ELECTRIC CHARGE

RELATIVE

MASS

PROTON p +1 1

NEUTRON 1

ELECTRON 1/1840


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2. Fill in the blanks with appropriate words to describe properties of subatomic particles of an atom. Use words in the box to help you

1. ..................................................is the number of protons in the nucleus of an atom2. ....................................................is the number of protons and neutrons in the nucleus of an atom3. An is the smallest particle of an element that remain identical to all other particles.4. The atoms of one .are different from those of all other element.5. are made when atoms of different elements are combined together.6. ..are used to describe the types of atoms and their numbers in an element or compound.7. Protons and neutrons are composed of smaller particles called ..8. While an atom is tiny, the nucleus is ten thousand times smaller than the atom and the quarks and electrons are at least ten thousand times

smaller than the nucleus.

9. ..are particles that are smaller than the atom.10.Atoms of a particular element must have the same number of protons but can have different numbers of 11.When two atoms have the same number of protons but different number of neutrons, they are called .

QUARKS SPIN AND ROTATE ELEMENT COMPOUNDS

CHEMICALLY

CHEMICAL FORMULA GAIN OR LOSE SUBATOMIC PARTICLES

ATOM

NEUTRONS AN ISOTOPE PROTONS AND NEUTRONS


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12. Element's or isotope's mass numberor nucleon number tells how many ..in itsatoms.

13. Electrons around the outside of the nucleus.

14. As the electrons circle the nucleus they travel at certain energy levels but can "jump" between different energy levels if they

energy.

If an electron weighed the same as a 1 cent ,

a proton would weigh the same as a gallon of milk.

HANDOUT 11

Write symbols for elements below

ELEMENT SYMBOL ELEMENT SYMBOL

Hydrogen Sodium

Helium Magnesium

Calcium Aluminium Al

Potassium K Silicon

If this were the proton in a

hydrogen atom, it would take a

screen 1 mile across to display

the electron's orbit.


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Argon Phosphorous

Chlorine Neon

Sulphur

S

Fluorine F

Lithium Oxygen

Beryllium Zinc

Boron Iron

Carbon

C

Silver

Nitrogen Gold Au

Lead Nitrogen

Note 1What is the function of electron to an atom?

Answer:

Absorbs or give out energy. Also valence electron able to form bond with other atoms so to make compounds

What is the function of proton to an atom?

Answer:

The number ofprotons in an atomdefines what element the atomis. Also provides an attractive force for orbiting electrons.

What is the function of neutron to an atom?Answer:

neutrons hold the nucleus together.

Neutrons in an atom'snucleus decide the isotopes of an atom


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Worksheet 1.1:

Question:1. Helium-6 and Helium-7 are isotopes. The nucleon number of helium-6 is 6 and Helium-7 is 7. Given the proton number for each isotope

is 2, answer the following question.

(a)What is meaning of the term isotopes?

____________________________________________________________________(b)Write the symbol for helium-6 and helium-7 , showing proton number and nucleon number.

(c)Compare the number of electrons, protons and neutrons in one atom of helium-6 and one atom of helium-7______________________________________________________________________________________________________________

______________________________________________________________________________________________________________

(d)What are the similarities and difference between isotopes helium-6 and helium-7.

Answer the following questions.

Atoms of the same element can have different numbers of neutrons; the different possible versions of each element are called isotopes.

For example,


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Fill in the table below

Isotopes No. of protons No. of electrons No of neutrons

8

10

6

17


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9. inhibit budding in potatoes

10.pest control in agriculture

Worksheet 1 (complete the table below)Element Proton

number

Nucleon

number

Number

of

neutrons

Number

of

protons

Number

of

electrons

Draw the BOHR S

ATOMIC MODEL

Electron

arrangement

Number of

valence electrons

Hydrogen 1 1 1

Helium 2 4

Lithium 3 7

Beryllium 4 9


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Boron 5 11

Carbon 6 12 2.4 4

Nitrogen 7 7

Oxygen 8 8


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Fluorine 9 10

Neon 10 10

Sodium 11 12

Magnesium 12 12

Aluminium 13 27


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Silicon 14 28

Phosphorus 15 31

Sulphur 16 32

Chlorine 17 18

Argon 18 22


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Potassium 19 20

Calcium 20 20

STATE THE MEANINGS OF THESE TERMS

A. VALENCE ELECTRONS

Are the number of in the occupied shell of an ..


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LO 3.3 ANALYSING THE RELATIONSHIP BETWEEN THE NUMBER OF MOLES OF A SUBSTANCE WITH ITS MASS

Activity 1 : Relate molar mass of a substance to its NAconstant and RAM / RMM / RFM

No

NameRAM/RMM/RFM

No of particles

(atom/molecule/ion)

Molar mass

(g/mol)

Mass of

1 mole

(g)

1. Potassium, K(39)

6.02 x 1023 (39g/mol) 39g

2. Oxygen, O2 (32)6.02 x 1023

3. Water, H2O (18)6.02 x 1023

4. Zinc, Zn 6.02 x 1023(65g/mol)

5. Magnesium

oxide, MgO 6.02 x 1023

(40g/mol)

6. Sodium

chloride, NaCl(58.5)

6.02 x 1023

7. Nitrogen

dioxide, NO2 (46)

6.02 x 1023

8. Aluminium

sulphate,

Al2(SO4)3 (342)

6.02 x 1023

(342g/mol)

9. Sulphur

dioxide, SO26.02 x 1023

(64g/mol0

10. Copper(II)nitrate, Cu(NO3)2

6.02 x 1023


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(188)

11. Methane,CH4 (16)

6.02 x 1023

12. Iron(III)

chloride, FeCl3

(162.5)

6.02 x 1023

13. Carbon, C 6.02 x 1023(12g/mol)

14. Nitric acid,

HNO3 (63)

6.02 x 1023

Activity 2 : Solving numerical problems to convert the number of moles of a given substance to its mass and vice versa

1. The molar mass of a substance ,

= the mass of _________________ mole of the substance.= the mass of (NA) number of particles

= the mass of ____________________ particles

x Molar mass

Molar mass

2. Calculating the Mass from a number of Moles

Number of moles = . mass of the substance .

Number of moles Mass in g


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mass of 1 mole of the substance/molar mass

Therefore :

Example 1 : What is the mass of 2 moles of carbon ?

Mass = 2 x 12= 24g

Example 2 : What is the mass of 2 moles of H2O ?

Mass = 2 x [ 2(1) + 16 ]

= 36g

3. Calculate the masses of these substances.

a) 2 moles of aluminium atomsMass =

b) 10 moles of iodine atomsMass =

c) 3 moles of lithium atomsMass =

d) 0.5 moles of oxygen gas (O2)Mass =

e) 0.1 moles of sodiumMass =

f) 2 moles of chlorine molecules (Cl2)Mass =

Mass of substance = Number of moles x Molar mass


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g) 1 mole of carbon dioxide ( CO2)Mass =

h) 3 moles of nitric acid, ( HNO3)Mass =

i) 2 moles of calcium carbonate (CaCO3)Mass =

j) 0.25 moles of calcium chloride (CaCl2)Mass =

k) 0.25 moles of sodium hydroxide (NaOH)Mass =

l) 0.25 moles of sodium carbonate (Na2CO3)Mass =

m)0.5 moles of potassium manganate (VII) (KMnO4)Mass = n) 0.25 moles of hydrated magnesium sulphate (MgSO4.7H2O)Mass =

4. Calculate the Number of Moles from a given Mass

Example : How many moles are there in 88g of CO2

Number of moles = 88 = 2 moles

44

a) 2g of helium atomsNumber of moles = b) 6g of carbon atomsNumber of moles =

c) 16g of helium atoms d) 4g of sulphur atoms


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Number of moles = Number of moles =

e) 4g of oxygen molecules (O2)Number of moles =

f) 213g of chlorine molecules (Cl2)Number of moles =

g) 0.56g of nitrogen molecules (N2)Number of moles =

h) 254g of iodine molecules (I2)Number of moles =

i) 88g of carbon dioxide (CO2)Number of moles =

j) 3.1g of sulphur dioxide (SO2)Number of moles =

k) 560g of potassium hydroxide (KOH)Number of moles =

l) 392g of sulphuric acid (H2SO4)Number of moles =

m)170g of ammonia (NH3)Number of moles =

n) 120g of magnesium oxide (MgO)Number of moles =

o) 4g of sodium hydroxide (NaOH)Number of moles =

p) 73g of hydrogen choride (HCl)Number of moles =


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q) 15.8g of potassium manganate (VII) KMnO4Number of moles =

r) 8g of ammonium nitrate (NH4NO3)Number of moles =

s) 0.78g of aluminium hydroxide Al(OH)3Number of moles =

t) 0.92g of ethanol (C2H5OH)Number of moles =

5. Complete the following table.

Element/compoundChemical

formulaeMolar mass Calculate

Copper Cu RAM= 64 (a)Mass of 1 mol = g

(b) Mass of 2 mol = . g

(c)Mass of mol = .g

(d)Mass of 3.01x1023 Cu atoms

=

Sodium hydroxide NaOH RFM= 40 (a) Mass of 3 mol of sodium hydroxide

=


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(b) Number of moles of sodium hydroxide in

20 g =

Zinc nitrate Zn(NO3)2 RFM = a) Number of moles in 37.8 g of zinc nitrate :

LO 3.4 ANALYSING THE RELATIONSHIP BETWEEN THE NUMBER OF MOLES OF A GAS WITH ITS VOLUME

Activity 1 : Calculate the volume of gases at STP or room conditions from the number of moles and vice versa,

1. The molar volumeof a gas is defined as the

.

2. One mole of any gas always has the under the same temperature and pressure.

3. The molar volume of any gas is

24 dm3at or

22.4 dm3at .Example :

1 mol of oxygen gas, 1 mol of ammonia gas, 1 mol helium gas and 1 mol sulphur dioxide gas occupies the same volume of 24 dm3at room

condition.


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x 22.4 / 24 dm3

22.4/24 dm3

4. Calculate the volume of gasin the following numbers of moles at STP

Example : Find the volume of 1 mole of CO2gas

Volume = number of moles x 22.4 dm3

= 1 x 22.4 dm3

= 22.4 dm3

a) 3 moles of oxygenVolume =

b) 2 moles of CH4Volume =

c) 0.3 moles of ArgonVolume =

d) 0.2 moles of SO3Volume =

e) 0.1 moles of N2Volume = f) 1.5 mol of N2Volume =

Number of moles of gas Volume of gas


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5. Complete the diagram below .

Activity 2 : Solve numerical problems involving number of particles, number of moles, mass of substances and volume of gases at STP or room

conditions.

Solve these numerical problems

1. What is the volume of 0.3 mole of sulphur dioxide gas at STP? [Molar volume: 22.4 dm3mol-1at STP]

(Ans: 6.72 dm3)

2. Find the number of moles of oxygen gas contained in a sample of 120 cm3of the gas at room conditions. [Molar volume: 24 dm3mol-1at

room conditions]

(Ans: 0.005 mol)

Volume of gas (dm )

Number of molesMass in gram No of particles


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3. Calculate the number of water molecules in 90 g of water, H2O. [Relative atomic mass: H, 1; O, 16. Avogadro constant,NA: 6.02 x 1023

mol-1]

(Ans; 3.01x 1024molecules)4. What is the volume of 24 g methane, CH4 at STP? [Relative atomic mass: H, 1; C, 12. Molar volume: 22.4 dm3mol-1at STP]

(Ans: 33.6 dm3)

5. How many aluminium ions are there in 20.4 g of aluminium oxide, Al2O3? [Relative atomic mass: O, 16; Al, 27. Avogadro constant,NA:

6.02 x 1023mol-

(2 x 0.2 x 6.02 x1023)


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6. Calculate the number of hydrogen molecules contained in 6 dm3of hydrogen gas at room conditions. [Molar volume: 24 dm3mol-1at

room conditions Avogadro constant,NA: 6.02 x 1023mol-1]

(Ans: 1.505x1023 molecules)

7. Find the volume of nitrogen in cm3at STP that consists of 2.408 x 1023nitrogen molecules. [Molar volume: 22.4 dm3mol-1at STP.

Avogadro constant,NA: 6.02 x 1023mol-1]

(Ans: 8.96 dm3)


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SOLVING NUMERICAL PROBLEMS INVOLVING EMPIRICAL FORMULA1. 24g of element X combines with 32 g of sulphur to form a compound. Determine the empirical formula of the compound? [RAM: X; 6,

S; 32 ]

2. 1.72g of M oxide contains 0.8g oxygen. Determine the empirical formula of M oxide. [RAM : M; 46, O; 16 ]

3. A sample of carbon disulfide, CS2, contains 16g of sulphur. Determine the mass of carbon in the sample. [RAM: S; 32, C; 12 ]


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4. 11g of element A combines with 6.4g of element B to form a compound AB2, Calculate the relative atomic mass of element A. [RAM :

B; 16 ]

5. An oxide of sulphur contains 40% sulphur. Calculate its empirical formula. [RAM: S; 32, O; 16 ]

6. Element M combines with fluorine to form MFx. Determine the value of x if 2.28g of fluorine combines with 3.8g of element M.[RAM :

M; 190, F; 19 ]


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EXERCISE 1 : EMPIRICAL FORMULA AND MOLECULAR FORMULA

a) Write the empirical formula of the following compounds in the table below.

Molecular Formula Empirical Formula

C2H4

C4H8

C6H12O6

H2SO4

MgO

b) A compound has empirical formula of C4H9and relative molecular mass is 114. Determine the molecular formula of the compound.[

RAM: C; 12, O; 16]


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c) A compound has the empirical formula CH and relative molecular mass is 78. Determine its molecular formula. [RAM : C; 12, H; 1 ]

DETERMINATION OF EMPIRICAL FORMULA OF METAL OXIDE

1. The empirical formula of an oxide of metal X is determined using the set-up shown in the diagram 1. A result of the experiment is as

follows. [ RAM: X; 24, O; 16]

Diagram 1

Mass of combustion tube = 24.56 g

Mass of combustion tube + metal X = 25.16 g

Mass of combustion tube + oxide of X = 25.56 g

a. Why must metal X used in powdered form?

................................................................................................................................................

b. Suggest a method to prepare oxygen................................................................................................................................................


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c. How do you determine that all metal X has completely reacted with oxygen?

............................................................................................................................................................................................................................

............................................................................................................................................................................................................................

d. i. Determine the empirical formula for the oxide of metal X.

ii. Write the chemical equation for the above reaction

................................................................................................................................................

CHEMICAL FORMULA OF COMPOUNDS

Write the formula for the ionic compounds listed below.

sodium chloride ammonium sulphate calcium carbonate

zinc sulphate lead (II) oxide lead (II) bromide

Magnesium sulphate sulphuric acid calcium nitrate

sodium hydride silver nitrate magnesium hydroxide


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iron (II) nitrate Lead(II) nitrate zinc sulphide.

Potassium sulphate Copper(II) sulphate barium hydroxide

aluminium oxide calcium carbonate copper (II) chloride

NAMING OF CHEMICAL COMPOUNDS USING IUPAC NOMENCLATURE

Name the compounds below.

H2 S FeCl2

Cu2 O K2 Cr2 O7

NH4NO3 Al2(OH)3

NaBr BaCO3

PbI2 CaSO4

MgH2 Fe (OH)3


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ZnSO4 CuCO3

Li2 SO4 Ag2 CrO4

SnO (NH4)2SO4

CH3 COOH Na2 CO3

ACTIVITY 1: NUMERICAL PROBLEMS INVOLVING CHEMICAL EQUATION

NO. QUESTION ANSWER

1 2 Li + 2 H2O 2 LiOH + H

2

Lithium atom has 0.5 mol, find the number of mole for :

a) water

b) lithium hydroxidec) hydrogen gas

a)

b)

c)

a)0.5 mol , b)0.5mol , c)0.25 mol


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2 Zn + 2 HCl ZnCl2 + H2a) How many moles of hydrochloric acid are needed to

react with 0.2 mol of zinc ?

b) How many moles of hydrogen gas are produced from

0.6 mol of HCl?

a)

b)

a)0.4 mol , b) 0.3 mol

3 2 H2O2 2 H2O + O2When 0.02 mol of H2O2decomposes, calculate

a) the mass of water formed[Ar H = 1 , O =16]b) the volume of O2gas evolved at s.t.p

[1 mol of gas occupied 22.4 dm3at s.t.p]

a)

b)

a)0.36 g , b) 0.224 dm3

4 2 Mg + O2 2 MgO

Calculate the mass of magnesium oxide which is formedwhen 1.2 g of magnesium is burn in oxygen .

[Ar O = 16 , Mg = 24 ]

Ans : 1.0 g


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WORKSHEET 1 -IONIC BOND

ANSWER ALL QUESTIONS.

Exercise 1 : Write the half equation for the:

a) Formation of cation from a metal atom b) Formation of anion from a non metal atomi) Li : _____________________ F :_______________________

ii) Na:_____________________ Cl:_______________________

iii) K : _____________________ Br:______________________

iv) Mg:_____________________ I : _______________________

v) Ba:_____________________ N:_______________________

i) Pb:______________________

Exercise 2: Formation of ionic compound, sodium chloride

1. Electron arrangement of sodium atom is _____________________________2. A sodium atom _________________ one valence electron to achieve the ________

Electron arrangement which is 2.8.

3. A sodium ion, _____________ is formed.

4. Half equation : ____________________________________

5. Electron arrangement of chlorine atom is _______________________

6. A chlorine atom _____________ one electron from sodium atom to achieve

_______________________________________ which is 2.8.8.

7. A chloride ion, ___________ is formed.

8. Half equation : _____________________________________9. The sodium ion, Na+ and chloride ion, Cl-are attracted to each other by a strong

________________________________________

10. Forming an ________________ bond.

11.Electron arrangement diagram :


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Exercise 3: Explain the formation of ionic bond in magnesium chloride.(Proton no: Mg;12, Cl; 17)

Covalent BondsActivity 1 : Formation of covalent bonds

Fill in the blanks with the correct words.

1 Covalent bonds are formed when .. atoms .. electrons to achieve . electron

arrangements .2 Types of covalent bonds:-

(i)

(ii)

(iii)

3 A single bond is formed when of electrons is shared between two atoms.

A double bond is formed when ..of electrons is shared between two atoms.

A triple bond is formed when .of electrons is shared between two atoms.4 Formation of hydrogen molecules,H2:-

A hydrogen atom has valence electron, with an electron arrangement of... It needs .. more electron to achieve the .. electron arrangement

..hydrogen atoms one electron each for

Shared-paired electrons forms a .. bond in the hydrogen molecule,H2

Single bond holds the two hydrogen atoms together because the shared-pair of electrons is attracted to the of


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both atoms

5 Complete the diagram below.

(a)

(b) A covalent bond can be illustrated by using.

Activity 2 : Formation of covalent bonds

1 Formation of oxygen molecules, O2:

An oxygen atom has valence electron, with an electron arrangement of..

It needs .more electrons to achieve the .. electron arrangement

....oxygen atoms sharepairs of electrons forming a..bond2

(a)

Draw the electron arrangement for the formation of oxygen molecule.

[Proton number : O, 8 ;]


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(b) Illustrate the formation of oxygen molecule using the Lewis structure.

3 Formation of a nitrogen molecule,N2:

A nitrogen atom has valence electron, with an electron arrangement ....

It needs more electrons to achieve the .. electron arrangement

..nitrogen atoms sharepairs of electrons forming a covalent bond

4 Draw the electron arrangement for the formation of nitrogen molecule.

[Proton number : N, 7]

(b) Illustrate the formation for nitrogen molecule using the Lewis structure.


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Appendix 1Complete the following table for the electrolysis of 0.5 mol dm-3sodium nitrate, NaNO3solution using carbon electrode.

Set up of apparatus

Ions present in electrolyte

Electrode Anode Cathode

Ion that are attracted toanode and cathode

Ion discharged (accept ordonate electron)

______ ions because ________ ion because

Half equation

Name of the products

Observations

Confirmatory test (methodand observation)


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Changes in electrolyte

Appendix 2

Complete the following table for the electrolysis of 0.5 moldm-3copper (II) nitrate, Cu(NO3)2 solution using carbon electrode.

Set up of apparatus


Electrode Anode Cathode

Ion that are attracted to

anode and cathode

Ion discharged (accept ordonate electron)


Half equation

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Observations

Confirmatory test (method

and observation)


Appendix 3Complete the following table for the electrolysis of 0.5 moldm-3sodium sulphate, Na2SO4solution using carbon electrode.

Set up of apparatus

Ions present in electrolyteElectrode Anode Cathode


anode and cathode

Ion discharged (accept or ______ ions because ________ ion because

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donate electron)

Half equation


Observations

Confirmatory test (method

and observation)


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Appendix 4EXERCISES

1 Diagram 1 shows the electrolysis of copper (II) sulphate solution using carbon electrodes.

Diagram 1

(a) Determine the cathode and the anode electrodes.

(b) (i) State all the ions present in the dilute copper (II) sulphate solution.

(ii) Name the ions which move to electrodes K and L.

Electrode K :

Electrode L : .

(c) (i) What is observed at electrode L in the cell?

(ii) Write down the half equation for the reaction at electrode L.

..

(d) (i) Name the product at electrode K in the cell.

(ii) Explain your answer.

...

(iii) Write down the half equation for the reaction at electrode K.

.

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Appendix 1

Complete the following table for the electrolysis of 0.001moldm-3hydrochloric acid and 1 moldm-3hydrochloric acid using carbon electrode.

Set up of apparatus

Electrolyte 0.001 moldm-

hydrochloric acid 1 moldm-

hydrochloric acid



anode

Ion discharged (accept ordonate electron) at anode


Half equation at the anode

Name of the products atanode

Observations at anode

Confirmatory test at theanode (method and

observation)


cathode

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Ion discharged (accept or

donate electron) at cathode


Half equation at cathode

Name of the products at

cathode

Observations at cathode

Confirmatory test at

cathode (method and

observation)

Appendix 2

Complete the following table for the electrolysis of 0.001 moldm-3

sodium chloride solution and 2.0 moldm-3

sodium chloride solution using carbonelectrode.

Set up of apparatus

Electrolyte 0.001 moldm- sodium chloride solution 2.0 moldm- sodium chloride solution



anode

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donate electron) at anode




anode


Confirmatory test at the

anode (method and

observation)


cathode

Ion discharged (accept ordonate electron) at cathode




cathode


Confirmatory test at

cathode (method and

observation)

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Appendix 3Complete the following table for the electrolysis of 1 moldm-3copper (II) sulphate solution with carbon electrode and copper electrode.

Set up of apparatus

Electrode Carbon Copper



anode


donate electron) at anode




anode


Confirmatory test at theanode (method andobservation)


cathode

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donate electron) at cathode




cathode


Changes in the intensity of

blue solution and the

reason.

Appendix 41 Diagram 1 shows the apparatus set up to investigate the electrolysis of 1.0 mol dm-3 sodium chloride solution using carbon electrodes.

Diagram 1

(a) State all ions present in sodium chloride solution.

..............................................................................................................................

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(b) (i) State the ion that will be discharged at electrode X.

.........................................................................................................................

(ii) Explain your answer in b(i).

........................................................................................................................

(c) (i) Name the product formed at electrode Y.

.........................................................................................................................

(ii) Write the half equation for the reaction at electrode Y..........................................................................................................................

(iii) 0.1 mol of gas is released at electrode Y.

Calculate the volume of gas released.

[Molar volume of gas = 24 dm3 mol-1 at room temperature and pressure]

(d) The experiment is repeated using 0.0001 mol dm-3 sodium chloride solution as the electrolyte.

(i) Name the gas produced at electrode X.

.......................................................................................................................

(ii) Write the half equation for the reaction in d(i).......................................................................................................................

(iii) Describe a chemical test to confirm the presence of gas named in d(i).

................................................................................................................................................................................................

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2. The Diagram 2 shows the apparatus set-up for the electrolysis of silver nitrate solution using silver electrodes X and Y.

Diagram 2

Based on Diagram 2, answer the following questions.

(a) (i) What is meant by cation?

..........

(ii) List the ions present in silver nitrate solution..................................................................................................................

(iii) Name the ions attracted toanode : ................................................................................. ............

cathode : ................................................................................................(b) (i) Name the product formed at the silver electrode X.

..........

(ii) Write the half equation for the reaction that take place at silver electrode X.

......

(c) (i) The electrolysis is repeated by replacing both silver electrodes with carbon electrodes. What can be observed at anode andcathode?

At anode: .......

At cathode: ..........

(ii) Write the half equation

Silver

electrode X Silver

electrode Y

Silver nitrate

solution

Bulb

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At anode: ......

At cathode..............

Topic : ElectrochemistrySub topic : 6.6 Construct the electrochemical series using voltaic cell

Diagram 1 shows a chemical cell. /Rajah 1menunjukkan satu sel kimia.

Diagram /Rajah1

(a) (i) State the name of apparatus A.Nyatakan nama bagi radas A.

..

[1 mark]

(ii) What is the function of apparatus in (a) (i).

Apakah fungsi radas dalam (a) (i).

..

[1 mark]

(b) (i) State one observation at the zinc plate.

Nyatakan satu pemerhatian pada kepingan zink.

.. [1 mark]

(ii) Write the half equation for the reaction that occurs at the zinc plate.

Tuliskan setengah persamaan bagi tindak balas yang berlaku pada kepingan zink.

..................................................................................................................

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[1 mark]

(c) What is the type of reaction occur at copper plate.

Apakah jenis tindak balas yang berlaku pada kepingan kuprum.

[1 mark]

(d) Draw the flow of electron in Diagram 1.

Lukiskan arah pengaliran elektron pada Rajah1.[1 mark]

(e) The copper plate in the chemical cell above is replaced by magnesium metal and copper(II) sulphate solution is replaced bymagnesium sulphate solution.

Kepingan kuprum dalam sel kimia di atas ditukar dengan logam magnesium dan larutan kuprum(II)sulfat ditukar dengan

larutan magnesium sulfat.

(i) What will happen to the direction of electron flow?Apakah yang akan berlaku kepada arah pengaliran elektron?

..

[1 mark](ii) Give a reason for your answer.

Berikan satu sebab untuk jawapan anda.

..

[1 mark]

(f) Another experiment is carried out by replacing zinc plate with metal P and Q.

Table 1 shows the results.

Satu eksperimen lain dijalankan dengan menggantikan kepingan zink dengan logam P danQ.Jadual 3.2menunjukkan keputusan

yang telah diperolehi.

Pair of metal Voltage / V Negative terminal

P and Cu 2.0 P

Q and Cu 0.5 Q

Table /Jadual1(i) Arrange metals P, Q and Cu in ascending order of electropositivity.

Susunkan logam P, Q dan Cumengikut tertib menaik keelektropositifan.

..................................................................................................................

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[1 mark]

(ii) Predict the voltage for chemical cell using pair of metal P and Q.Ramalkan voltan bagi sel kimia yang menggunakan pasangan logam P dan Q.

..................................................................................................................

[1 mark]

Topic : ElectrochemistrySub topic : 6.6 Construc electrohcemical Series : Predict the ability of a metal to displace another metal from its salt solution

An experiment is carried out to determine the relative position of three metals, silver,L and M, in the electrochemical series. Diagram 8.2 shows

the results of theexperiment.

experiment

I II III

Observation Grey deposit

Colourless solution

Grey deposit

Light blue solution

No change

Diagram 8.2

(i) Based on the results, arrange the three metals in order of increasing electropositivity. Explain your answer.[6 marks]

(ii) If M is copper, name the product formed in experiment II. [2 marks]

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EXAMPLE OF ESSAY QUESTION.

A student is given a piece of impure silver plate. Design an experiment to

produce a sample of very pure silver metal in the laboratory.

Your answer should consist of the following:

Chemicals required Procedures of the experiment

Diagram showing the set-up of apparatus

Chemical equation involved in the reaction

Observation 10 marks

C: CONCENTRATIONS OF ACIDS AND ALKALIS

Learning Outcomes

You should be able to:

State the meaning of concentration State the meaning of molarity

State the relationship between the number of moles with molarity and volume of asolution

Describe the methods for preparing standard solutions

Describe the preparation of a solution with a specified concentration using dilutionmethod

Relate pH values with the molarity of acids and alkalis

Solve numerical involving molarity of acids and alkalis

Activity 1 : Concentration of acids and alkalis

Fill in the blanks with the correct answers.

1

2

The concentration of a solution refers to the quantity of solute in 1dm of solution

Concentration can be defined in two ways :-

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(a) Concentration in g dm- =

(b) Concentration in mol dm- =

(Concentration in mol dm-3is also known as molarityor molar concentration (M ) )

2 The two units of concentration can be inter-converted:

Work thi s out.

3 5.0 g of copper(II) sulphate is dissolved in water to form 500 cm solution. Calculate the concentration of copper(II) sulphate solution

in g dm-3?

[Answer: 10.0 g dm-3]

4 What is the mass of sodium carbonate required to dissolve in water to prepare 200 cm solution that contains 50 g dm- ?

[Answer: 10 g]

(Refer to page 123 -124 - F4 Chemistry textbook )

Concentration in................... Concentration in............................

X Molar mass

Molar mass

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5 4.0 g of sodium carbonate powder, Na2CO3 , is dissolved in water and made up to 250 cm . What is the molarity of the sodium

carbonate solution?

[Relative atomic mass: C, 12; O, 16; Na, 23]

[Answer: 0.15 moldm-3]

Activity 2

The number of moles of solute, nin a given volume of solution V and the molarity of M can be calculated by using the formula :

n = Number of moles of solute

M = Molarity of solution (mol dm- )

V = Volume of solution (dm )

If the volume is in cm convert the volume of solution from cm to dm

5 Calculate the number of moles of ammonia in 150 cm of 2 mol dm- aqueous ammonia.

[Answer: 0.3 mol]

n = MV

n = M x V

1000n= MV

1000or

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6 A student pipetted 20.0 cm of potassium hydroxide , KOH solution into a conical flask. The concentration of the alkali was 1.5 mol

dm-3. Calculate the number of moles of potassium , KOH in the flask.

[Answer: 0.03 mol dm-3]

7 Calculate the number of moles of hydrogen ions present in 200 cm of 0.5 mol dm- sulphuric acid, H2SO4.

[Answer: 0.2 mol of H+ions]

Activity 12 : Preparation of Standard solutions

1 What is a standard solution?

2 Preparation of standard solutions by Weighing method (mass of solute) :-

Step 1: Calculate the mass of solute needed .

mass = n X molar mass

= MV X molar mass

1000

Example: To prepare 100 cm3of 2.0 mol dm-3sodium hydroxide solution.

Calculate the mass of NaOH needed. [Relative atomic mass: Na, 23 ; O, 16 ; H, 1]

mass = n X molar mass

n = MV

1000

n = mass

molar mass

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= MV X molar mass

1000= 2.0 X 100 X 40 = 8 g

1000

Try this:

(a) To prepare 250 cm3of 1.0 mol dm-3sodium carbonate solution. Calculate the mass of Na2CO3needed. [Relative atomic

mass: Na, 23 ; O, 16 ; C, 12]

[Answer : 26.50g]

(b) 0.25 mol dm- solution of sodium hydroxide was prepared by dissolving xg of sodium hydroxide in 750 cm of water. What is

the value ofx? [Relative atomic mass: Na, 23 ; O, 16 ; H, 1]

[Answer : 7.5 g]

(Refer to page 126 - F4 Chemistry textbook )

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Step 2 :Match the descriptions / procedures with the correct diagram below.

Wash and rinse the weighing bottleor small beaker and filter funnel to

ensure no solute remains in any of

the apparatus used.

Transfer the dissolved solute into asuitable volumetric flask.

(a)

Add water slowly by using adropper to bring the level of the

solution to the calibration mark.

The volumetric flask is closedtightly and inverted several times to

get a uniform or homogenous

solution.

(b)

Calculate the mass of soluteneeded.

Weigh out the exact mass of soluteneeded in a weighing bottle.

Dissolved the solute in a smallamount of distilled water.

(c)

Add more water carefully to thevolumetric flask and swirl gently.

Shake well to ensure thoroughmixing.

(d)

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Handout : Preparation of Standard solutions by Dilution method

1 Dilution method

Step 1: Calculate the volume of stock solution required by using the equation:-

M1= molarity of solution before dilution

V1 = volume of solution before dilution

M2= molarity of solution after dilution

V2 = volume of solution after dilution

Example: 50 cm of 0.1 mol dm- sodium hydroxide, NaOH solution from 2.0 mol dm- sodium hydroxide,NaOH solution

Before dilution After dilution

M1 V1 M2 V2

2.0 mol dm- ? 0.1 mol dm- 50 cm

2.0 x V1 = 0.1 x 50

V1 = 0.1 x 50 = 2.5 cm3

2.0

Try this: 100 cm of 0.5 mol dm- potassium manganate(VII) ,KMnO4solution is prepared from 1.0 mol dm

- potassium

manganate(VII) ,KMnO4solution. Calculate the volume of the solution

[Answer : 50 cm3]

M1V1= M2V2

When using the equation M1V1= M2V2,

make sure that both V1and V2are of

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Step 2Match the diagram with the correct descriptions below.

(a)

(b)

(c)

(d)

Add water slowly by using a dropper to bring the level of the solution to thecalibration mark.

The volumetric flask is closed tightly and inverted several times to get auniform or homogenous solution.

Transfer the stock solution to a suitable volumetric flask.

Calculate the volume of stock solution required.

Use a pipette to draw up the required volume of stock solution.

Activity 14 : The pH values and molarity of acids and alkalis

Fill in the blanks with correct words . Use words given in the box.

Increases decreases concentration hydrogen

dissociation higher hydroxide alkali

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1 The pH value of an acid or an alkali depends on three factors :

(a) degree of.

(b) molarity or ..

(c) .. of the acid or ..2 The lower the pH value, the .. the concentration of ions.

3 The higher the pH value, the .. the concentration of ... ions.

4 As the molarity of an acid increases , the pH value of the acid .The pH value of an alkali increases when the molarity of the alkali ...

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Fill in the blanks for appropriate substances to be used to prepare insoluble salts

( Remember!!!! All insoluble salts must be prepared from two soluble substances )

Write balanced chemical equation for each reaction from 1)

a) ..+ calcium carbonate + chemical equation:

b) ..+ lead(II) iodide +

chemical equation

c) ..+ barium sulphate +

chemical equation:

d) ..+ silver chloride +

chemical equation:

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React acid with metal/ metal hydroxide

/ metal oxide/ metal carbonate

Is metal hydroxide /

metal carbonate soluble?

Titration methodMix acid and alkali to produce salt

Eg: HCl +NaOHNaCl + H2Oyes

Mix acid and excess metal/ metal oxides/metal carbonate

Eg: CuO+ H2SO4 CuSO4 + H2O

No

pMix solutions of two soluble substances /saltsto precipitate the insoluble salt

Eg: NaCl + AgNO3 AgCl + NaNO3IS IT

SOLUBLE?

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EXIT TICKET INSOLUBLE SALT

TO PREPARE INSOLUBLE SALT (EG BARIUM SULPHATE)

Rearrange the procedures below according to the correct order of method

The mixture is filtered

The insoluble salt is then pressed between 2 filter papers to dry

The residue is rinsed with distilled water to remove impurities

The mixture is stirred with a glass rod

50 cm3

of 1.0 mol dm-3

barium nitrate solution is poured into 50 cm3

of 1.0 mol dm-3

of sodium sulphate in a beaker

Rearrange the pictures below according to the correct order of procedures

1

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Write a balanced chemical equation for the preparation of insoluble salt.

Uses of salts in our daily life

Salts are important to our bodies.

Choose the best salts for use in various fields below. One example has been done for you

b) ..+ calcium carbonate +

chemical equation:

Ammonium sulphate copper(II) sulphate sodium chloride silver salts sodium hypochlorite potassium nitrate

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USES OF SALTS

FOOD INDUSTRY

CHEMICAL INDUSTRYAGRICULTURE

MEDICAL USE

Calcium sulphate

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1) Fill in the blanks for word equation below to prepare soluble salts ( Remember!!!! All soluble salts must be prepared from acids)a) . + magnesium magnesium sulphate + .b) Hydrochloric acid + zinc chloride + water

c) Nitric acid + .. copper (II) nitrate+carbon dioxide + ............d) .. + potassium hydroxidepotassium nitrate + e) Ethanoic acid + zinc ethanoat + hydrogenf) . + calcium oxide calcium nitrate +

2) Write balanced chemical equations for reactions which make the following salts .(Remember, soluble salts must start from acids)a) Magnesium chloride from magnesium metal..

b) copper(II) sulphate from copper(II) oxide.. c) sodium nitrate from sodium hydroxide..

d) lead(II) nitrate from lead(II) carbonate.

TO PREPARE SOLUBLE SALT ( EG SODIUM CHLORIDE) BY TITRATION METHOD

CONSISTS OF 2 STAGESStage 1- Determine the volume of alkali needed to neutralize acid solution by titration method


Fill a burette with hydrochloric acid and record the initial burette reading

Use a pipette to draw up 25.00 cm3of sodium hydroxide solution

Add hydrochloric acid drop by drop into the alkali solution . Swirl the contents of the flask.

Continue adding the acid until the indicator just turns from pink to colourless Record the final burette reading

Transfer the sodium hydroxide solution into a conical flask . Add 2 to 3 drops of phenolphthalein


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stage 2 : TO PREPARE SALT( SODIUM CHLORIDE) FROM THE NEUTRAL SOLUTION OBTAINED FROM TITRATION METHOD


The experiment is now repeated as stage 1 above but no indicator is used

Pour the solution of sodium chloride in an evaporating basin

Filter the sodium chloride crystals and dry them by squeezing them between sheets of filter paperAllow the solution to cool .Crystals of sodium chloride will appear in the cool solution

Heat to evaporate most of the water. This produce a hot saturated solution of sodium chloride

The hydrochloric acid is placed in a burette and the same volume of acid is added to the flask as before. If, for example 30.5 cm3

of theacid was used in the first experiment to just react with the alkali, then 30.5 cm3of acid is added to the second experiment. The flask will

then contain a solution of sodium chloride without excess of acid or alkali

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TO PREPARE SOLUBLE SALT (EG ZINC SULPHATE) BY REACTION OF ACID WITH EXCESS METAL/OXIDE

METAL/CARBONATE METALRearrange the procedures below according to the correct order of method

Filter the zinc sulphate crystals and dry them by squeezing them between sheets of filter paper

Heat to evaporate most of the water. This produce a hot saturated solution of zinc sulphate.

Allow the solution to cool .Crystals of zinc sulphate will appear in the cool solution

Pour the solution of zinc sulphate in an evaporating basin

Remove the excess zinc metal by filtering

Add zinc powder bit by bit with stirring to hot dilute sulphuric acid until some of it no longer reacts, The acid is then used up .There is

excess zinc present1

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SOLUBLE SALT EXIT TICKET

1)A salt is a compound formed when the .. ions from an acid is replaced by a ion or anion

2) Salts are named from acids that they come from.Choose appropriate salts from the corresponding acids in the boxes below . One example has been done for you

Sodium chloride sodium sulphate sodium nitrate

Calcium nitrate magnesium nitrate sodium ethanoat copper(II)

sulphate silver chloride potassium ethanoat

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SALTS

Hydrochloric acid

NitricSulphuric acid

Ethanoic acid

Documents

Buku Latihan Kimia f4 2015