Ch.16 - Acids and Bases

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Ch.16 - Acids and Bases

Problema 96c

Determine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. c. NO₃^–

Problema 97

Determine the [OH^–] and pH of a solution that is 0.140 M in F^–.

Problema 98

Determine the [OH-] and pH of a solution that is 0.250 M in HCO3⁻.

Problema 99a

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. a. NH₄⁺

Problema 99b

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. b. Na⁺

Problema 99c

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. c. Co³⁺

Problema 99d

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. d. CH₂NH₃⁺

Problema 100a,b,c

Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. a. Sr²⁺ b. Mn³⁺ c. C₅H₅NH⁺

Problema 100d

Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. d. Li⁺

Problema 101a,b,c,d

Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. FeCl₃ b. NaF c. CaBr₂ d. NH₄Br

Problema 101e

Determine if each salt will form a solution that is acidic, basic, or pH-neutral. e. C₆H₅NH₃NO₂

Problema 102a

Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. Al(NO₃)₃

Problema 102b,c,d,e

Determine if each salt will form a solution that is acidic, basic, or pH-neutral. b. C₂H₅NH₃NO₃ c. K₂CO₃ d. RbI e. NH₄ClO

Problema 103

Arrange the solutions in order of increasing acidity. NaCl, NH₄Cl, NaHCO₃, NH₄ClO₂, NaOH

Problema 104

Arrange the solutions in order of increasing basicity: CH3NH3Br, KOH, KBr, KCN, C5H5NHNO2.

Problema 105a

Determine the pH of each solution. a. 0.10 M NH₄Cl

Problema 106

Determine the pH of each solution. a. 0.20 M KCHO₂ b. 0.20 M CH₃NH₃I c. 0.20 M KI

Problema 107

Calculate the concentration of all species in a 0.15 M KF solution.

Problema 108

Calculate the concentration of all species in a 0.225 M C₆H₅NH₃Cl solution.

Problema 109

Write chemical equations and corresponding equilibrium expressions for each of the three ionization steps of phosphoric acid.

Problema 110

Write chemical equations and corresponding equilibrium expressions for each of the two ionization steps of carbonic acid.

Problema 111a

Calculate the [H₃O⁺] and pH of each polyprotic acid solution. a. 0.350 M H₃PO₄

Problema 111b

Calculate the [H₃O⁺] and pH of each polyprotic acid solution. b. 0.350 M H₂C₂O₄

Problema 112a

Calculate the [H₃O⁺] and pH of each polyprotic acid solution.

a. 0.125 M H₂CO₃

Problema 112b

Calculate the [H₃O⁺] and pH of each polyprotic acid solution.

b. 0.125 M H₃C₆H₅O₇

Problema 113

Is this question correctly formulated? If so, could you provide it as is; if not, modify it as needed and return it in JSON format: Calculate the concentration of all species in a 0.500 M solution of H2SO3.

Problema 114

Calculate the concentration of all species in a 0.155 M solution of H₂CO₃.

Problema 115

Calculate the [H₃O⁺] and pH of each H₂SO₄ solution. At approximately what concentration does the x is small approximation break down?

a. 0.50 M b. 0.10 M c. 0.050 M

Problema 116a

Consider a 0.10 M solution of a weak polyprotic acid (H₂A) with the possible values of K_a1 and K_a2 given here.

a. K_a1 = 1.0 × 10^–4; K_a2 = 5.0 × 10^–5

Calculate the contributions to [H₃O⁺] from each ionization step. At what point can the contribution of the second step be neglected?

Problema 116b

Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2 given here: b. Ka1 = 1.0 * 10^-4; Ka2 = 1.0 * 10^-5. Calculate the contributions to [H3O+] from each ionization step. At what point can the contribution of the second step be neglected? c. Ka1 = 1.0 * 10^-4; Ka2 = 1.0 * 10^-6.