Question 1

What is the pH at the stoichiometric point for the titration of 0.26 M CH₃NH₂(aq)with 0.26 M HClO₄(aq)? For CH₃NH₂,K_b = 3.6 * 10^-⁴.

Accepted Answer

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Question 2

Calculate the equilibrium constant for the reaction that occurs when perchloric acid is added to the buffer B(aq)/BHCl(aq).The K_b of B is 3.4 *10^-5.

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Question 3

What is the pH at the half-stoichiometric point for the titration of 0.88 M HNO₂(aq)with 0.10 M KOH(aq)? For HNO₂,K_a = 4.3 * 10^-4.

Accepted Answer

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Question 4

Calculate the equilibrium constant for the reaction that occurs when nitric acid is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 1.2 * 10^-5.

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Question 5

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq)with 0.036 M NaOH(aq)? For acetic acid,K_a = 1.8 * 10^-5.

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Question 6

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq)with 0.10 M KOH(aq)? For HNO₂,K_a = 4.3 * 10^-4.

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Question 7

What is the pH at the stoichiometric point for the titration of 0.100 M CH₃COOH(aq)with 0.100 M KOH(aq)? The value of K_a for acetic acid is 1.8 * 10^-5.

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Question 8

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq)with 0.072 M NaOH(aq)? For acetic acid,K_a = 1.8 * 10^-5.

Accepted Answer

At the stoichiometric point in the titration of a weak acid (CH3COOH) with a strong base (NaOH), the solution contains only the acetate ion (CH3COO-) and water. The concentration of acetate ion can be found using the formula for the equilibrium constant of the acid dissociation reaction (Ka) and the initial concentration of acetic acid. The concentration of acetate ion is not directly given by the initial concentrations of the reactants or the stoichiometry of the reaction but is calculated using the formula for the ionization of acetic acid in water. Given that Ka = 1.8 × 10^-5, we can set up an equation to solve for the concentration of acetate ion ([CH3COO-]) at equilibrium. The concentration of acetate ion is determined by the dissociation of acetic acid in water, which is influenced by the value of Ka and the initial concentration of acetic acid. The calculation involves solving an equilibrium problem where the initial concentration of acetic acid is used to find the concentrations of H+ and CH3COO- at equilibrium. The concentration of acetate ion is not directly proportional to the initial concentration of acetic acid or the concentration of NaOH used in the titration but is calculated based on the equilibrium constant (Ka) and the change in concentration due to the reaction.

Question 9

Which of the following indicators would be most suitable for the titration of 0.10 M (CH₃)₃N(aq)with 0.10 M HClO₄(aq)? For trimethyamine,pK_b = 4.19.

Accepted Answer

Bromocresol green would be the most suitable indicator for the titration of 0.10 M (CH3)3N(aq) with 0.10 M HClO4(aq) because the pKa of trimethylamine is 9.75, which is higher than the pKa of bromocresol green (4.7). This means that trimethylamine will be protonated and present as (CH3)3NH+ during the titration, and bromocresol green will be able to detect the pH change around the equivalence point when all of the trimethylamine has been protonated. The other indicators listed have pKa values that are either too high or too low to be suitable for this titration.

Question 10

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 4.1 *10^-5.

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Question 11

Which of the following indicators would be most suitable for the titration of 0.10 M lactic acid with 0.10 M KOH(aq)? For lactic acid,pK_a = 3.08.

Accepted Answer

The equivalence point of a weak acid-strong base titration is typically above 7. Phenol red, with a pK_In of 7.9, is suitable for detecting this change.

Question 12

At the stoichiometric point in the titration of 0.260 M CH₃NH₂(aq)with 0.260 M HCl(aq),

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Question 13

At the stoichiometric point in the titration of 0.130 M HCOOH(aq)with 0.130 M KOH(aq),

Accepted Answer

At the stoichiometric point, formic acid (HCOOH) is completely neutralized by KOH, forming formate ions (HCOO-) and water. The formate ion is a weak base, which will hydrolyze in water, making the solution slightly basic, so the pH is greater than 7.

Question 14

For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH(aq),calculate the pH after the addition of 55.0 mL of KOH(aq).For salycylic acid,pK_a = 2.97.

Accepted Answer

The correct answer is A because the pH of the solution after the addition of 55.0 mL of KOH(aq) is 10.98. This is because the salicylic acid is a weak acid and the KOH is a strong base, so the reaction will go to completion and the salicylic acid will be completely neutralized. The pH of the solution will then be determined by the concentration of the acetate ion, which is the conjugate base of the salicylic acid. The pKa of salicylic acid is 2.97, so the pH of the solution will be 10.98.

Question 15

The curve for the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq)with 0.100 M NaOH(aq)is given below.What are the main species in the solution after 7.5 mL of base have been added?

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Question 16

The titration curve for the titration of 0.100 M H₂SO₃(aq)with 0.100 M KOH(aq)is given below. Estimate pK_a1 and pK_a2 of H₂SO₃.

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Question 17

Consider the titration of 10.0 mL of 0.100 M (CH₃)₃N(aq)with 0.100 M HClO₄(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of acid?

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Question 18

Consider the titration of 50.0 mL of 0.0200 M HClO(aq)with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base?

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Question 19

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer B(aq)/BHCl(aq).The K_b of B is 1.5 * 10^-5.

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Question 20

Consider the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq),with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.

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Quiz 13: Aqueous Equilibria

What is the pH at the stoichiometric point for the titration of 0.26 M CH₃NH₂(aq) with 0.26 M HClO₄(aq) ? For CH₃NH₂,K_b = 3.6 * 10^-⁴.

Calculate the equilibrium constant for the reaction that occurs when perchloric acid is added to the buffer B(aq)/BHCl(aq).The K_b of B is 3.4 *10^-5.

What is the pH at the half-stoichiometric point for the titration of 0.88 M HNO₂(aq) with 0.10 M KOH(aq) ? For HNO₂,K_a = 4.3 * 10^-4.

Calculate the equilibrium constant for the reaction that occurs when nitric acid is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 1.2 * 10^-5.

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq) with 0.036 M NaOH(aq) ? For acetic acid,K_a = 1.8 * 10^-5.

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq) with 0.10 M KOH(aq) ? For HNO₂,K_a = 4.3 * 10^-4.

What is the pH at the stoichiometric point for the titration of 0.100 M CH₃COOH(aq) with 0.100 M KOH(aq) ? The value of K_a for acetic acid is 1.8 * 10^-5.

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq) with 0.072 M NaOH(aq) ? For acetic acid,K_a = 1.8 * 10^-5.

Which of the following indicators would be most suitable for the titration of 0.10 M (CH₃) ₃N(aq) with 0.10 M HClO₄(aq) ? For trimethyamine,pK_b = 4.19.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 4.1 *10^-5.

Which of the following indicators would be most suitable for the titration of 0.10 M lactic acid with 0.10 M KOH(aq) ? For lactic acid,pK_a = 3.08.

At the stoichiometric point in the titration of 0.260 M CH₃NH₂(aq) with 0.260 M HCl(aq) ,

At the stoichiometric point in the titration of 0.130 M HCOOH(aq) with 0.130 M KOH(aq) ,

For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH(aq) ,calculate the pH after the addition of 55.0 mL of KOH(aq) .For salycylic acid,pK_a = 2.97.

The curve for the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq)with 0.100 M NaOH(aq)is given below.What are the main species in the solution after 7.5 mL of base have been added?

The titration curve for the titration of 0.100 M H₂SO₃(aq)with 0.100 M KOH(aq)is given below. Estimate pK_a1 and pK_a2 of H₂SO₃.

Consider the titration of 10.0 mL of 0.100 M (CH₃)₃N(aq)with 0.100 M HClO₄(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of acid?

Consider the titration of 50.0 mL of 0.0200 M HClO(aq)with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base?

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer B(aq)/BHCl(aq).The K_b of B is 1.5 * 10^-5.

Consider the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq),with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.

Quiz 13: Aqueous Equilibria

What is the pH at the stoichiometric point for the titration of 0.26 M CH3NH2(aq) with 0.26 M HClO4(aq) ? For CH3NH2,Kb = 3.6 * 10-4.

Calculate the equilibrium constant for the reaction that occurs when perchloric acid is added to the buffer B(aq)/BHCl(aq).The Kb of B is 3.4 *10-5.

What is the pH at the half-stoichiometric point for the titration of 0.88 M HNO2(aq) with 0.10 M KOH(aq) ? For HNO2,Ka = 4.3 * 10-4.

Calculate the equilibrium constant for the reaction that occurs when nitric acid is added to the buffer HA(aq)/NaA(aq).The Ka of HA is 1.2 * 10-5.

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH3COOH(aq) with 0.036 M NaOH(aq) ? For acetic acid,Ka = 1.8 * 10-5.

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO2(aq) with 0.10 M KOH(aq) ? For HNO2,Ka = 4.3 * 10-4.

What is the pH at the stoichiometric point for the titration of 0.100 M CH3COOH(aq) with 0.100 M KOH(aq) ? The value of Ka for acetic acid is 1.8 * 10-5.

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH3COOH(aq) with 0.072 M NaOH(aq) ? For acetic acid,Ka = 1.8 * 10-5.

Which of the following indicators would be most suitable for the titration of 0.10 M (CH3) 3N(aq) with 0.10 M HClO4(aq) ? For trimethyamine,pKb = 4.19.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The Ka of HA is 4.1 *10-5.

Which of the following indicators would be most suitable for the titration of 0.10 M lactic acid with 0.10 M KOH(aq) ? For lactic acid,pKa = 3.08.

At the stoichiometric point in the titration of 0.260 M CH3NH2(aq) with 0.260 M HCl(aq) ,

At the stoichiometric point in the titration of 0.130 M HCOOH(aq) with 0.130 M KOH(aq) ,

For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH(aq) ,calculate the pH after the addition of 55.0 mL of KOH(aq) .For salycylic acid,pKa = 2.97.

The curve for the titration of 50.0 mL of 0.0200 M C6H5COOH(aq)with 0.100 M NaOH(aq)is given below.What are the main species in the solution after 7.5 mL of base have been added?

The titration curve for the titration of 0.100 M H2SO3(aq)with 0.100 M KOH(aq)is given below. Estimate pKa1 and pKa2 of H2SO3.

Consider the titration of 10.0 mL of 0.100 M (CH3)3N(aq)with 0.100 M HClO4(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of acid?

Consider the titration of 50.0 mL of 0.0200 M HClO(aq)with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base?

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer B(aq)/BHCl(aq).The Kb of B is 1.5 * 10-5.

Consider the titration of 50.0 mL of 0.0200 M C6H5COOH(aq),with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.

What is the pH at the stoichiometric point for the titration of 0.26 M CH₃NH₂(aq) with 0.26 M HClO₄(aq) ? For CH₃NH₂,K_b = 3.6 * 10^-⁴.

Calculate the equilibrium constant for the reaction that occurs when perchloric acid is added to the buffer B(aq)/BHCl(aq).The K_b of B is 3.4 *10^-5.

What is the pH at the half-stoichiometric point for the titration of 0.88 M HNO₂(aq) with 0.10 M KOH(aq) ? For HNO₂,K_a = 4.3 * 10^-4.

Calculate the equilibrium constant for the reaction that occurs when nitric acid is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 1.2 * 10^-5.

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq) with 0.036 M NaOH(aq) ? For acetic acid,K_a = 1.8 * 10^-5.

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq) with 0.10 M KOH(aq) ? For HNO₂,K_a = 4.3 * 10^-4.

What is the pH at the stoichiometric point for the titration of 0.100 M CH₃COOH(aq) with 0.100 M KOH(aq) ? The value of K_a for acetic acid is 1.8 * 10^-5.

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq) with 0.072 M NaOH(aq) ? For acetic acid,K_a = 1.8 * 10^-5.

Which of the following indicators would be most suitable for the titration of 0.10 M (CH₃) ₃N(aq) with 0.10 M HClO₄(aq) ? For trimethyamine,pK_b = 4.19.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 4.1 *10^-5.

Which of the following indicators would be most suitable for the titration of 0.10 M lactic acid with 0.10 M KOH(aq) ? For lactic acid,pK_a = 3.08.

At the stoichiometric point in the titration of 0.260 M CH₃NH₂(aq) with 0.260 M HCl(aq) ,

For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH(aq) ,calculate the pH after the addition of 55.0 mL of KOH(aq) .For salycylic acid,pK_a = 2.97.

The curve for the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq)with 0.100 M NaOH(aq)is given below.What are the main species in the solution after 7.5 mL of base have been added?

The titration curve for the titration of 0.100 M H₂SO₃(aq)with 0.100 M KOH(aq)is given below. Estimate pK_a1 and pK_a2 of H₂SO₃.

Consider the titration of 10.0 mL of 0.100 M (CH₃)₃N(aq)with 0.100 M HClO₄(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of acid?

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer B(aq)/BHCl(aq).The K_b of B is 1.5 * 10^-5.

Consider the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq),with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.