Chem 3 Chapter 8 HW

83) What is the molarity of an HCl solution if 35.5 mL of 0.10 M NaOH are needed to neutralize 25.0 mL of the sample?

0.14 M

9) Label the acid and the base and the conjugate acid and the conjugate base in each reaction. a) H₂O(l) + HI(g) ↔I⁻(aq) + H₃O⁺(aq) b) CH₃COOH(l) + NH₃(g) ↔CH₃COO⁻(aq) + NH₄⁻(aq) c) Br⁻(aq) + HNO₃(aq) ↔HBr(aq) + NO₃⁻(aq)

base / acid ↔ conjugate base / conjugate acid a) H₂O(l) + HI(g) ↔ I⁻(aq) + H₃O⁺(aq) acid / base ↔ conjugate base / conjugate acid b) CH₃COOH(l) + NH₃(g) ↔CH₃COO⁻(aq) + NH₄⁺(aq) base / acid ↔ conjugate acid / conjugate base c) Br⁻(aq) + HNO₃(aq) ↔ HBr(aq) + NO₃⁻(aq)

87) How many milliliters of 1.0 M NaOH solution are needed to neutralize 10.0 mL of 2.5 M CH₃COOH solution?

25 mL

5) Classify each reactant as a Bronsted-Lowry acid or base. a) HCl(g) + NH₃(g) →Cl⁻(aq) + NH₄⁺(aq) b) CH₃COOH(l) + H₂O(l) →CH₃OO⁻(aq) + H₃O⁺(aq) c) OH⁻(aq) + HSO₄(aq) →H₂O(l) + SO₄²⁻(aq)

Acid / Base a) HCl(g) + NH₃(g) b) CH₃COOH(l) + H₂O(l) Base / Acid c) OH⁻(aq) + HSO₄⁻(aq)

12) Diagrams D-F represent three acids (HA) dissolved in water. Rank the three acids (D-F) in order of increasing acidity.

D < F < E

77) What are the concentrations of H₃O⁺ and OH⁻ in tomatoes that have a pH of 4.10?

[H₃O⁺] = 7.9 x 10⁻⁵ M [OH⁻] = 1.3 x 10⁻¹⁰

20) What H₃O⁺ concentration corresponds to each pH value: a) 13 b) 7 c) 3 Label the solution as acidic, basic, or neutral.

a) 1 x 10⁻¹³ M basic b) 1 x 10⁻⁷ M neutral c) 1 x 10⁻³ M acidic

71) Calculate the value of [H₃O⁺] from the given [OH⁻] and label the solution as acidic or basic. a) 10⁻² M b) 4.0 x 10⁻⁸ M c) 6.2 x 10⁻⁷ M d) 8.5 x 10⁻¹³ M

a) 10⁻¹² M basic b) 2.5 x 10⁻⁷ M acidic c) 1.6 x 10⁻⁸ M basic d) 1.2 x 10⁻² M acidic

69) Calculate the value of [OH⁻] from the given [H₃O⁺] and label the solution as acidic or basic. a) 10⁻⁸ M b) 10⁻¹⁰ M c) 3.0 x 10⁻⁴ M d) 2.5 x 10⁻¹¹ M

a) 10⁻⁶ M basic b) 10⁻⁴ M basic c) 3.3 x 10⁻¹¹ M acidic d) 4.0 x 10⁻⁴ M basic

22) Convert each H₃O⁺ concentration to a pH value a) 1.8 x 10⁻⁶ M b) 9.21 x 10⁻¹² M c) 0.000088 M d) 0.0000000000762 M

a) 5.74 b) 11.036 c) 4.06 d) 10.118

19) Convert each H₃O⁺ concentration to a pH value. a) 1 x 10⁻⁶ M b) 1 x 10⁻¹² M c) 0.00001 M d) 0.00000000001 M

a) 6 b) 12 c) 5 d) 11

21) What H₃O⁺ concentration corresponds to each pH value: a) 10.2 b) 7.8 c) 4.3

a) 6 x 10⁻¹¹ M b) 2 x 10⁻⁸ M c) 5 x 10⁻⁵ M

61) Use the data in table 8.2 to label the stronger acid in each pair a) H₂O or CH₃COOH b) H₃PO₄ or H₂SO₄

a) CH₃COOH b) H₂SO₄

81) Write a balanced equation for each reaction. a) HBr(aq) + KOH(aq) → b) HNO₃(aq) + Ca(OH)₂(aq) → c) HCl(aq) + NaHCO₃(aq) → d) H₂SO₄(aq) + Mg(OH)₂(aq) →

a) HBr(aq) + KOH(aq) → KBr(aq) + H₂O(l) b) 2 HNO₃(aq) + Ca(OH)₂(aq) → 2 H₂O(l) + Ca(NO₃)₂(aq) c) HCl(aq) + NaHCO₃(aq) → NaCl(aq) + H₂O(l) + CO₂(g) d) H₂SO₄(aq) + Mg(OH)₂(aq) → 2 H₂O(l) + MgSO₄(aq)

55) Label the conjugate acid-base pairs in each equation. a) HI(g) + NH₃(g) →NH₄⁺(aq) + I⁻(aq) b) HCOOH(l) + H₂O(l) → H₃O⁺(aq) + HCOO⁻(aq) c) HSO₄⁻(aq) + H₂O →H₂SO₄(aq) + OH⁻(aq)

a) HI (acid) NH₃ (base) →NH₄⁺ (conjugate acid) + I⁻ (conjugate base) b) HCOOH (acid) + H₂O (base) → H₃O⁺ (conjugate acid) + HCOO⁻ (conjugate base) c) HSO₄⁻ (base) + H₂O (acid) →H₂SO₄ (conjugate acid) + OH⁻ (conjugate base)

7) Draw the conjugate base of each species: a) H₂S b) HCN c) HSO₄⁻

a) HS⁻ b) CN⁻ c) SO₄²⁻

6) Draw the conjugate acid of each species: a) H₂O b) I⁻ c) HCO₃⁻

a) H₃O⁺ b) HI c) H₂CO₃

91) Consider a buffer prepared from the weak acid HF and its conjugate base F⁻ HF(aq) + H₂O(l) ↔F⁻(aq) + H₃O⁺(aq) a) What happens to the concentrations of HF and F⁻ when a small amount of acid is added to the buffer? b) What happens to the concentrations of HF and F⁻ when a small amount of base is added to the buffer?

a) When a small amount of acid is added to the buffer, the concentration of HF increases and the concentration of F⁻ decreases. b) The concentration of HF decreases and the centration of F⁻ increases when a small amount of base is added to the buffer.

35) Identify the acid, base, conjugate acid, and conjugate base in each diagram. Gray spheres correspond to H atoms.

a) acid + base → conjugate base + conjugate acid b) base + acid →conjugate acid + conjugate base

49) Which of the following species can be Bronsted-Lowry bases? a) OH⁻ b) Ca²⁺ c) C₂H₆ d) PO₄³⁻ e) OCl⁻ f) MgCO₃

a,d,e,f

47) Which of the following species can be Bronsted-Lowry acids? a) HBr b) Br₂ c) AlCl₃ d) HCOOH e) NO₂⁻ f) HNO₂

a,d,f

11) When ascorbic acid (vitamin C, molecular formula C₆H₈O₆) is dissolved in water, the following acid-base reaction occurs. Label the conjugate acid-base pairs in the given equation. C₆H₈O₆(aq) + H₂O(l) ↔C₆H₇O₆⁻(aq) + H₃O⁺(aq)

acid / base ↔ conjugate base / conjugate acid C₆H₈O₆(aq) + H₂O(l) ↔C₆H₇O₆⁻(aq) + H₃O⁺(aq)