19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1.What can you say about the K a value of a strong

Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

19.1 Acid-Base Theories>19.1 Acid-Base Theories>

1

1. What can you say about the Ka value of a strong acid?

2. In a 0.100 M solution of a monoprotic acid [H+] = 2.5 * 10-2 M. Calculate the Ka of this acid?

Day 4 4-30

8.33 * 10-3

3. The pH for a 0.20 M solution of a monoprotic acid is 2.5, what is the Ka? 5.08 * 10-5



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http://wps.prenhall.com/esm_brown_chemistry_9/2/660/169060.cw/index.html

Homework # 1 Chapter 16 – show me successful screen (100%) OR email to me – due Tues. 4-24







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Day 5 5-1

1. The pH for a 0.10 M solution of a monoprotic acid is 1.2, what is the Ka?

0.108



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Titration

Titration = the process of adding a measured amount of a solution of known concentration to a solution of unknown concentration – using a neutralization reaction to determine concentration

Steps:1. a measured volume of an acid solution of unknown concentration is added to a flask2. an indicator is added3. measured volumes of a base of known

concentration are mixed into the acid until the indicator just barely changes color



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Titration

The solution of known concentration is called the standard solution.

Neutralization occurs (titration is complete) when the number of hydrogen ions equals the number of hydroxide ions. = the equivalence point = end point



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Titration

Determining the concentration by titration mathematically:

Example: A 25 mL solution of H2SO4 is neutralized by 18 mL of 1.0 M NaOH. What is the concentration of the H2SO4 solution? The equation for the reaction is:

H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l)

Conversion plan:you need mols H2SO4 to calculate molarity0.018 L NaOH mols NaOH mols H2SO4



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Titration

Determining the concentration by titration mathematically:

Additional Example: How many milliliters of 0.45 M HCl will neutralize 25.0 mL of 1.00 M KOH?

Period 1 stopped Wed. 5-1



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V. Salts in Solution

A. Salt Hydrolysis

Recall that some salts can hydrolyze water – remove hydrogen ions from or donate hydrogen ions to water (Hydrolysis of Salts Lab) salt hydrolysis.

salts that produce acidic solutions have positive ions that release hydrogen ions to water

salts that produce basic solutions have negative ions that attract hydrogen ions from water



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Example: ammonium chloride

Ammonium chloride completely ionizes in water:

NH4Cl(aq) NH+4(aq) + Cl-

(aq)

the ammonium ion is a strong enough acid to donate a hydrogen ion to a water molecule:

NH+4(aq) + H2O(l) NH3(aq) + H3O+

(aq)

the resulting H3O+ ions make the solution somewhat acidic



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Strong acid + Strong base neutral solution

Strong acid + Weak base acidic solution (salt’s cation releases hydrogens to water)

Weak acid + Strong base basic solution (salt’s anion attracts hydrogens from water)



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page 669 #s 27-34



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1.0 * 10-14

Arrhenius base

Amphoteric

Kb

Conjugate acid

Diprotic acid

Lewis acid

Self-ionization

Strong acid

Ka

Weak base

Bronsted-Lowry base



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1. HNO3 is a strong acid – assume it completely dissociates in water. Calculate the pH of a solution containing 1.02 g of HNO3 in 250. mL of solution.

1.19

Day 1 5-3



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Day 2 5-6

How many moles of nitric acid are needed to neutralize 0.50 moles of calcium hydroxide?

2HNO3 + Ca(OH)2 Ca(NO3)2 + 2H2O

1 mole



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Day 3 5-7

1. Carbonic acid is a weak acid, if it reacts with a strong base like NaOH, what type of solution will result?

2. Write an equation for the ionization of sodium bicarbonate.

3. Write an equation for the reaction between bicarbonate ions and water

NaHCO3 Na+(aq) + HCO3

-(aq)

HCO3-(aq) + H2O(l) H2CO3(aq) + OH-

(aq)



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Day 6 4-26

Arrhenius acidHydrolysisKw

-log[H+] Lewis baseUniversal IndicatorTitration

Bronsted-Lowry acid

Ka

Strong baseConcentrated acidNeutralization reactionStandard solution



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page 675 #s 39-43



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A 50 mL solution of H2SO4 is neutralized by 20 mL of 2.0 M NaOH. What is the concentration of the H2SO4 solution? The equation for the reaction is:

H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l)

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19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1.What can you say about the K a value of a strong