[PDF] [PDF] Chapter 11 – Acids and Bases – Practice Problems Section 111

[PDF] Ch 17a Acid-Base Practice Problems

Extra Practice Problems General p4 Answers p12 Ka: Sense + In the Brønsted–Lowry definition of acids and bases, an acid ______ a is a proton donor

[PDF] Acid-Base Practice Problems

Acid-Base Practice Problems A Identify each chemical as either an “acid” or a “ base” in the following reactions, and identify “conjugate” relationships

[PDF] Solutions to Review Problems for Acid/Base Chemistry - CSUN

1) are further diluted to exactly 800 mL, the solution pH is 2 74 Calculate Ka for acetic acid First, there is a dilution, followed by an equilibrium calculation 

[PDF] Acid base equilibrium 1-21 KEYpdfpdf - Prospect Ridge Academy

4 déc 2017 · AP Chemistry Chapter 14: Acid-Base Equilibria Practice Problems TTMITTTTTTTT 1) Write the dissociation reaction for each of the following 

[PDF] Chapter 8, Acid-base equilibria

1 M HCl and 1 M ammonia Answer: 4 78 The way to solve these problems is to, as a first step, let any acids and bases react together 100 as

[PDF] WORKSHEET: SOLUTION EQUILIBRIUM (Weak acids and bases

WORKSHEET: SOLUTION EQUILIBRIUM (Weak acids and bases, buffers, Polyprotic acids, and Hydrolysis ) SET A: 1 40 00 ml of 0 350 M CH3NH2 is titrated 

[PDF] Overview of Acid-Base Equilibria Questions

Remember for conjugate acid base pairs (and only for pairs): Kw = Ka*Kb This is a straightforward equilibrium problem Also note that the answer

[PDF] Chapter 11 – Acids and Bases – Practice Problems Section 111

When H2O acts as a base, it gains one H+, which forms its conjugate acid, H3O+ Practice Problems 8 Write the formula for the conjugate base for each of the 

[PDF] Acid / Base Equilibria - Cal State LA

Chem201 Self Quiz - 4 (Acid / Base Equilibria) 1 a Calculate Write the charge balance expression that applies to the solution of this problem (remember all 

[PDF] Practice Problems on Acid-‐Base Chemistry -‐ Answers 1 For each

Practice Problems on Acid-‐Base Chemistry -‐ Answers 1 For each of the following acid base reactions place one of the arrows inside the box to designate the 

[PDF] acid base ph problems with answers

[PDF] acid base practice problems with answers

[PDF] acid base reaction problems with answers

[PDF] acid base titration problems with answers

[PDF] acid base titration problems with answers pdf

[PDF] acid base test review answers

[PDF] acid/base stoichiometry practice problems answers

[PDF] acide acétique

[PDF] acide base ph cours

[PDF] acide base ph exercice

[PDF] acide base ph terminale s

[PDF] acide base physique chimie

[PDF] acide base physique terminale s

[PDF] acide base physique ts

[PDF] acide et base conjuguée

Chapter 11 Acids and Bases Practice Problems

Section 11.1 Acids and Bases

Goal: Describe and name acids and bases.

Summary:

An Arrhenius acid produces H+ and an Arrhenius base produces OH- in aqueous solutions. Acids taste sour, may sting, and neutralize bases. Bases taste bitter, feel slippery, and neutralize acids.

Naming acids:

Binary acids contain a single anion: HnX. To name: hydro [anion with -ic end] acid

HBr hydrobromic acid

H2S hydrosulfuric acid

Polyatomic acids contain a polyatomic ion: HnXOm (XOm = polyatomic ion) [polyatomic ion] acid if the polyatomic ion ends in -ate change to -ic if the polyatomic ion ends in -ite change to -ous

H2SO4 (sulfate) sulfuric acid

H2SO3 (sulfite) sulfous acid

Practice Problems

1. Indicate whether each of the following statements is characteristic of an Arrhenius acid, Arrhenius base,

or both: a. has a sour taste b. neutralizes bases c. produces H+ ions in water d. is named barium hydroxide e. is an electrolyte

2. Indicate whether each of the following statements is characteristics of an Arrhenius acid, Arrhenius

base, or both: a. neutralizes acids b. produces OH- ions in water c. has a slippery feel d. conducts an electrical current in solution

3. Identify each of the following as an Arrhenius acid, Arrhenius base, or none:

b. CsOH c. Mg(NO3)2 d. HClO4 e. HNO2 f. MgBr2 g. NH3 h. Li2SO3

4. Name each of the following acids or bases:

a. HCl b. Ca(OH)2 c. HClO4 d. HNO3 e. H2SO3

5. Name each of the following acids or bases:

a. Al(OH)3 b. H2SO4 c. HBr d. KOH e. HNO2 f. HClO2

6. Write formulas for each of the following acids or bases:

a. rubidium hydroxide b. hydrofluoric acid c. phosphoric acid d. lithium hydroxide e. ammonium hydroxide

7. Write formulas for each of the following acids or bases:

a. barium hydroxide b. hydroiodic acid c. nitric acid d. acetic acid e. hypochlorous acid

Section 11.2 Bronsted-Lowery Acids

Goal: Identify conjugate acid-base pairs for Bronsted-Lowry acids and bases.

Summary:

A Bronsted-Lowry acid donates H+ and a Bronsted-Lowry base accepts H+.

Identifying Conjugate Acid-Base Pairs

According to Bronsted-Lowry theory, a conjugate acid-base pair consists of molecules or ions related by

the loss of one H+ by an acid, an the gain of one H+ by a base.

Every acid-base reaction contains two conjugate acid-base pairs because an H+ is transferred in both the

forward and reverse directions. When an acid such as HF loses one H+, the conjugate base F- is formed. When H2O acts as a base, it gains one H+, which forms its conjugate acid, H3O+.

Practice Problems

8. Write the formula for the conjugate base for each of the following acids:

a. HCO3- b. HPO42- c. HBrO

9. Write the formula for the conjugate acid for each of the following bases:

a. CO32- b. H2O c. H2PO4-

10. In the following reaction, the acid-conjugate base pair is __i__ and the base-conjugate acid pair is

__ii__.

H3PO4(aq) + H2O(l) H2PO4-(aq) + H3O+(aq)

a. (i) H3PO4/H3O+ (ii) H2O/H2PO4- b. (i) H3PO4/H2O (ii) H2PO4-/H3O+ c. (i) H2O/H3O+ (ii) H3PO4/H2PO4- d. (i) H2O/H2PO4- (ii) H3PO4/H3O+ e. (i) H3PO4/H2PO4- (ii) H2O/H3O+

11. In the following reaction, the acid-conjugate base pair is __i__ and the base-conjugate acid pair is

__ii__.

CO32-(aq) + H2O(l) HCO3-(aq) + OH-(aq)

a. (i) CO32-/ H2O (ii) HCO3-/OH- b. (i) H2O/HCO3- (ii) CO32-/OH- c. (i) H2O/OH- (ii) CO32-/HCO3- d. (i) CO32-/OH- (ii) H2O/HCO3- e. (i) CO32-/HCO3- (ii) H2O/OH-

12. In the following reaction, the acid-conjugate base pair is __i__ and the base-conjugate acid pair is

__ii__. H3PO4(aq) + NH3(aq) H2PO4-(aq) + NH4+(aq) a. (i) H3PO4/H2PO4- (ii) NH3/NH4+ b. (i) H3PO4/NH4+ (ii) NH3/H2PO4- c. (i) H3PO4/NH3 (ii) H2PO4-/NH4+ d. (i) H2PO4-/H3PO4 (ii) NH4+/NH3 e. (i) NH3/NH4+ (ii) H3PO4/H2PO4-

13. Complete the following table:

Acid Conjugate Base

HI Cl- NH4+ HS-

14. Complete the following table:

Base Conjugate Acid

F-

HC2H3O2

HSO3- ClO-

15. When ammonium chloride dissolves in water, the ammonium ion NH4+ donates an H+ to water. Write a

balanced equation for the reaction of the ammonium ion with water. a. NH4+ + H2O NH3 + H3O+ b. NH4+ + H3O+ NH3 + H2O + H+ c. NH4+ + H3O+ NH3 + H2O + OH- d. NH3 + H2O NH2- + H3O+ e. NH3 + H3O+ NH4+ + H2O

16. When sodium carbonate dissolves in water, the carbonate ion CO32- acts as a base. Write a balanced

equation for the reaction of the carbonate ion with water. a. CO32- + H2O CO2 + H3O+ b. CO32- + H2O HCO3- + OH- c. CO32- + H2O H2CO4 d. CO32- + OH- CO32- + H2O e. CO32- + H2O H2CO3

Section 11.3 Strengths of Acids and Bases

Goal: Write equations for the dissociation of strong and weak acids; identify the direction of reaction.

Summary:

Strong acids dissociate completely in water, and the H+ is accepted by H2O acting as a base.

HCl + H2O H3O+ + Cl-

A weak acid dissociates only slightly in water, producing only a small amount of H+ and therefore a small

amount of H3O+

HI + H2O H3O+ + I-

Strong bases are hydroxides with metals from Groups 1 and 2 and dissociate completely in water. (NaOH,

Ca(OH)2

An important weak base is ammonia, NH3.

Understanding the Concepts:

In diagrams A and B, determine if the diagram represents a strong acid or a weak acid.

The acid has the formula HX.

Practice Problems

17. Using Table 11.3, identify the stronger acid in each of the following pairs:

a. NH4+ or H3O+ b. H2SO4 or HCl c. H2O or H2CO3

18. Using Table 11.3, identify the weaker acid in each of the following pairs:

a. HCl or HSO4- b. HNO2 or HF c. HCO3- or NH4+

19. Predict whether the following reaction contains mostly reactants or products at equilibrium:

H2CO3(aq) + H2O(l) HCO3-(aq) + H3O+(aq) a. mostly products b. mostly reactants

20. Predict whether the following reaction contains mostly reactants or products at equilibrium:

NH4+(aq) + H2O(l) NH3(aq) + H3O+(aq)

a. mostly products b. mostly reactants

21. Predict whether the following reaction contains mostly reactants or products at equilibrium:

HNO2(aq) + NH3(aq) NO2-(aq) + NH4+(aq)

a. mostly products b. mostly reactants

22. Predict whether the following reaction contains mostly reactants or products at equilibrium:

H3PO4(aq) + H2O(l) H3O+(aq) + H2PO4-(aq) a. mostly products b. mostly reactants

Challenge Problems

23. a. Write the formula for the conjugate base of H2S

b. Write the formula for the conjugate base of H3PO4 c. Which is the weaker acid: H2S or H3PO4?

24. a. Write the formula for the conjugate base of HCO3-

b. Write the formula for the conjugate base of HC2H3O2 c. Which is the stronger acid: HCO3- or HC2H3O2? Section 11.4 Dissociation Constants for Acids and Bases Goal: Write the expression for the dissociation constant of a weak acid or weak base.

Summary:

In water, weak acids and weak bases produce only a few ions when equilibrium is reached.

Weak acids have small Ka values, whereas strong acids, which are essentially 100% dissociated, have very large

Ka values.

The reaction for a weak acid can be written as HA + H2O H3O+ + A-. The acid dissociation constant expression is written as

For a weak base the equation is B + H2O BH+ + OH-, and the base dissociation constant expression is

written as

Practice Problems

25. Answer true or false for each of the following: A strong acid

a. is completely dissociated in aqueous solution b. has a small value of Ka c. has a strong conjugate base d. has a weak conjugate base e. is slightly dissociated in aqueous solution

26. Answer true or false for each of the following:

a. is completely dissociated in aqueous solution b. has a small value of Ka c. has a strong conjugate base d. has a weak conjugate base e. is slightly dissociated in aqueous solution

27. Consider the following acids and their dissociation constants:

H2SO3(aq) + H2O(l) H3O+(aq) + HSO3-(aq) Ka = 1.2 x 10-2 HS-(aq) + H2O(l) H3O+(aq) + S2-(aq) Ka = 1.3 x 10-19 a. Which is the stronger acid, H2SO3 or HS-? b. What is the conjugate base of H2SO3? c. Which acid has the weaker conjugate base? d. Which acid has the stronger conjugate base? e. Which acid produces more ions?

28. Consider the following acids and their dissociation constants:

HPO42-(aq) + H2O(l) H3O+(aq) + PO43-(aq) Ka = 2.2 x 10-13 HCHO2(aq) + H2O(l) H3O+(aq) + CHO2-(aq) Ka = 1.8 x 10-4 a. Which is the weaker acid, HPO42- or HCHO2? b. What is the conjugate base of HPO42-? c. Which acid has the weaker conjugate base? d. Which acid has the stronger conjugate base?quotesdbs_dbs19.pdfusesText_25