Test 6 Review

As temperature increases, the molecules velocity increases, increasing the pressure on the container.

States of Matter

State Shape Volume Compressible?

Flows?

Solid Definite Definite No No

Liquid Indefinite

Definite No Yes

Gas Indefinite

Indefinite

Yes Yes

Critical Point – above this temperature, no amount of pressure can liquefy it.

Triple Point – all three phases are in equilibrium

Phase Diagrams

Homogeneous mixtures

Solvent – the substance there is more of; it does the dissolving.

Solute – the substance there is less of; it is being dissolved.

Solute is dissolved in solvent

Solutions

Are all things soluble?◦ No

Polar solvents dissolve polar solutes.◦ Ex: water (polar)

Non polar solvents dissolve non polar solutes.◦ Ex: oil (non polar)

“Like Dissolves Like”

Intermolecular Forces

Temperature

Pressure◦ For gases

What states of matter are required to form solutions?◦ Any: solid, liquid or gas

Factors Determining Solubility

Heating

Stirring

Crushing

One exception: gases dissolve better in colder temperatures.

How do you increase rate of dissolving?

Solubility of gas increases with pressure

Henry’s Law

Solubility – the amount of solute that will dissolve in a given amount of solvent at a given temperature.

Saturated Solution – solution that contains all the solute it can at a given temperature.

Unsaturated Solution – solution that contains less than the saturated amount of solute.

Supersaturated Solution – solution that contains more solute than it could normally hold.

Every compound has its own solubility curve.

Typically, when heated, solubility will increase

Solubility Curves

Acids produce hydrogen ions

HCl H+ + Cl-

Bases produce hydroxide ions

NaOH Na+ + OH-

Arrhenius Theory

H+

OH-

Acids donate protons (+)

Bases accept protons (+)

Conjugate acid – particle formed when a base gains a hydrogen ion

Conjugate bases – particle that remains when an acid has donated a hydrogen ion

Conjugate acid-base pair – 2 substances that are related by the loss or gain of a single hydrogen ion◦ Ex: NH3 and NH4

+

Bronsted- Lowry Theory

HCl(g) + H2O(l) Cl-(aq) + H3O+(aq)

Acid Conj. AcidConj. BaseBase

Acid + Base Conj. Base + Conj. Acid

NH3(g) + H2O(l) NH4+

(aq) + OH-(aq)

AcidBase Conj. BaseConj. Acid

Taste sour pH from 0-6.99 Has H+ at the beginning of the formula Produce H2(g) when reacting with most metals Neutralize bases Conducts electricity (because they contain

electrolytes) Turns litmus paper red

Characteristics of Acids

HCl hydrochloric acid

HBr hydrobromic acid

HI hydroiodic acid

HNO3 nitric acid

H2SO4 sulfuric acid

HClO4 perchloric acid

Strong acids that ionize completely

The stronger an acid, the weaker its conjugate base and vice versa.

Taste bitter pH between 7.01-14 Have OH- ions Feels slippery Neutralize acids Turns litmus paper blue

Characteristics of Bases

LiOH lithium hydroxide NaOH sodium hydroxide KOH potassium hydroxide RbOH rubidium hydroxide CsOH cesium hydroxide Ca(OH)2 calcium hydroxide Sr(OH)2 strontium hydroxide Ba(OH)2 barium hydroxide

Mg(OH)2 magnesium hydroxide◦ Milk of magnesia, it is not completely soluble, but

what does dissolve is a strong base.

Strong Bases

Anion Acid Name Example

-ide hydro—ic HCl hydrochloric acid

-ite --ous HNO2

nitrous acid

-ate --ic HNO3

nitric acid

Naming Acids

**only binary acids use “hydro”

H2SO4

HF

H3PO4

H2SO3

H2CO3

HNO3

Try these. . .Sulfuric AcidHydrofluoric AcidPhosphoric Acid

Sulfurous Acid

Carbonic Acid

Nitric Acid

Monoprotic – has 1 hydrogen◦ HCl

Diprotic – has 2 hydrogens◦ H2SO4

Triprotic – has 3 hydrogens◦ H3PO4

Categories of Acids

Always form a salt and water

Salt – a crystalline compound formed form an acids anion and a bases cation.

Neutralization Reactions

HCl(aq) + NaOH(aq) NaCl(s) + H2O(l)

Can act as either an acid or a base

Water is amphoteric

Amphoteric

Acid pH<7 Base pH>7[H+] pH pOH [OH-]

1410 OHH

14 pOHpH

Once you have 1 item, you can get any other one.

An unknown concentration of acid or base can be determined by measuring the amount of known acid or base that will neutralize the unknown.

An indicator changes color when the “end point” or neutralization occurs

Titration

Standard solution◦ Solution in which the concentration is known

End point◦ The point at which equivalent amounts of

reactants are present

For one to one ratios

For non one to one ratios◦ Need to calculate a mole ratio.

bbaa VMVM

L

molM molVM

If 15.0 mL of 0.500M NaOH is used to neutralize 25 mL of HCl, what is the concentration of the acid?

NaOH + HCl H2O + NaCl Since the ratio is 1:1, use MaVa=MbVb

(0.500M)(15.0mL)=Mb(25.0mL)

Mb=0.300M HCl

Practice

Alternative

L

xM

015.0500.0 x = 0.0075 mol NaOH

molNaOH

molHClmolNaOH

1

10075.0 0.0075 mol HCl

L

molM

025.0

0075.00.300M HCl

A 25 mL solution of H2SO4 is completely neutralized by 18 mL of 1.0M NaOH. What is the concentration of the acid?

NaOH + H2SO4 H2O + Na2SO4

Practice

2 1 12

L

xM

018.00.1 x = 0.018mol NaOH

molNaOH

SOmolHmolNaOH

2

1018.0 42

0.0090mol H2SO4

L

mol

025.0

0090.00.36M H2SO4

Can absorb moderate amounts of acid or base without a significant change in pH

Consists of a weak acid and its salt or a weak base and its salt.

Example◦ Acetic acid: HC2H3O2

◦ Sodium acetate: NaC2H3O2

Buffers

How it works

HA H+ + A-

HA H+ + A-

Strong Acid

Weak Acid

Lots of H+, very little HA

Lots of HA, very little H+