Question 1

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.

Accepted Answer

The answer of The titration curve for the titration of...

Question 2

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?

Accepted Answer

The answer of Consider the titration of 50.0 mL of...

Question 3

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.

Accepted Answer

The answer of What is the pH at the stoichiometric...

Question 4

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.

Accepted Answer

The answer of Consider the titration of 50.0 mL of...

Question 5

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.

Accepted Answer

The answer of Calculate the equilibrium constant for the reaction...

Question 6

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.

Accepted Answer

The answer of Calculate the equilibrium constant for the reaction...

Question 7

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.

Accepted Answer

The answer of Calculate the equilibrium constant for the reaction...

Question 8

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.

Accepted Answer

The answer of What is the pH at the half-stoichiometric...

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 has a pKIn value close to the pKa value of trimethylamine (4.19). As a result, it will act as an effective indicator for the titration. At the equivalence point, the indicator's color changes from yellow to blue/green. As a result, bromocresol green is the most appropriate indicator for the titration of trimethylamine with HCl.

Question 10

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?

Accepted Answer

The answer of The curve for the titration of 50.0...

Question 11

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?

Accepted Answer

The answer of Consider the titration of 10.0 mL of...

Question 12

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

The answer of What is the pH at the stoichiometric...

Question 13

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

The answer of What is the pH at the half-stoichiometric...

Question 14

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 answer of Which of the following indicators would be...

Question 15

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 in the titration of a weak acid (HCOOH) with a strong base (KOH), the solution is basic because the conjugate base of the weak acid (HCOO-) is present in solution. This results in a pH greater than 7.

Question 16

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.

Accepted Answer

At the stoichiometric point, all the CH3COOH has reacted with NaOH and converted to CH3COONa. Therefore, the moles of CH3COOH = moles of NaOH added. 
Moles of CH3COOH = 0.018 M x Volume of CH3COOH = 0.018V 
Moles of NaOH = 0.036 M x Volume of NaOH = 0.036V 
At the stoichiometric point, 
0.018V = 0.036V 
Therefore, V = 0.5 L. 
Moles of CH3COOH = 0.018 x 0.5 = 0.009 mol 
Moles of NaOH = 0.036 x 0.5 = 0.018 mol 
As per the balanced equation, 1 mole of CH3COOH reacts with 1 mole of NaOH to form 1 mole of CH3COONa. 
Therefore, moles of CH3COONa = 0.009 mol 
Now, we can use the equilibrium expression for the reaction: 
CH3COOH + H2O ⇌ CH3COO- + H3O+ 
Ka = [CH3COO-][H3O+] / [CH3COOH] 
At the stoichiometric point, [CH3COOH] = 0. 
Ka = [CH3COO-][H3O+] / 0 = infinity 
pKa = -log(Ka) = -log(infinity) = 0 
pH = pKa + log([CH3COO-]/[CH3COOH]) 
At the stoichiometric point, pH = pKa + log([CH3COO-]/0) = 0 + infinity = infinity 
Therefore, the concentration of acetate ion at the stoichiometric point is infinitely high. However, since none of the answer choices reflect this, we must choose the closest value, which is 0.012 M (Choice D).

Question 17

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.

Accepted Answer

The answer of Calculate the equilibrium constant for the reaction...

Question 18

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 answer of For the titration of 50.0 mL of...

Question 19

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

Accepted Answer

At the stoichiometric point in the titration of a weak base (like CH₃NH₂) with a strong acid (HCl), the solution is acidic, hence the pH is less than 7. This is because the weak base is converted to its conjugate acid, which partially dissociates to release H⁺ ions, lowering the pH.

Question 20

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.

Quiz 13: Aqueous Equilibria

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 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?

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.

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.

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.

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.

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 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.

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.

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?

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?

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.

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.

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 0.130 M HCOOH(aq) with 0.130 M KOH(aq) ,

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.

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.

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.

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

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.

Quiz 13: Aqueous Equilibria

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 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?

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.

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.

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.

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.

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 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.

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.

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?

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?

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.

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.

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 0.130 M HCOOH(aq) with 0.130 M KOH(aq) ,

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.

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.

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.

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

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.

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.

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.

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.

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.

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.

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 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.

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.

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?

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?

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.

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.

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.

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.

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.

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.

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

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.