Question 1

What is the approximate value of the equilibrium constant,K_n,for the neutralization of acetic acid with sodium hydroxide,shown in the equation below? The K_a for acetic acid is 1.8 × 10^-5. CH₃CO₂H(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq)

Accepted Answer

The equilibrium constant for the neutralization reaction can be approximated by the inverse of the K_a of acetic acid, which is 1/(1.8 × 10^-5) ≈ 5.6 × 10⁴. However, considering the reaction involves a strong base (NaOH), the equilibrium constant is very large, indicating the reaction goes to completion, hence the closest choice is 1.8 × 10⁹.

Question 2

The neutralization constant K_n for the neutralization of phenobarbital (C₁₂H₁₂N₂O₃)and morphine (C₁₇H₁₉NO₃)is 2.9.The acid dissociation constant K_a for phenobarbital is 3.9 × 10^-8.What is the base dissociation constant K_b for morphine?

Accepted Answer

The base dissociation constant $K_b$ for morphine can be calculated using the relationship between the neutralization constant $K_{\text{neutralization}}$, the acid dissociation constant $K_a$ for phenobarbital, and the base dissociation constant $K_b$ for morphine: $K_{\text{neutralization}} = K_a \times K_b / K_w$, where $K_w$ is the ion product of water ($1.0 \times 10^{-14}$ at 25°C). Given $K_{\text{neutralization}} = 2.9$ and $K_a = 3.9 \times 10^{-8}$, solving for $K_b$ gives a value close to $7.4 \times 10^{-7}$.

Question 3

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 25.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5 for NH₃.

Accepted Answer

C

Question 4

Which is a net ionic equation for the neutralization of a weak acid with a strong base?

Accepted Answer

The net ionic equation for the neutralization of a weak acid (HF) with a strong base (NaOH) involves the weak acid donating a proton to the hydroxide ion, forming water and the conjugate base (F⁻).

Question 5

What is the approximate value of the equilibrium constant,K_n,for the neutralization of pyridine with hydrochloric acid,shown in the equation below? The K_b for pyridine is 1.8 × 10^-9. HCl(aq)+ C₅H₅N(aq)⇌ C₅H₅NHCl(aq)

Accepted Answer

The answer of What is the approximate value of the...

Question 6

Which of these neutralization reactions has a pH < 7 when equal molar amounts of acid and base are mixed?

Accepted Answer

The reaction between HCl (a strong acid) and C₅H₅N (a weak base) results in a solution with a pH < 7 because the conjugate acid (C₅H₅NH⁺) formed is stronger than the conjugate base, leading to an acidic solution.

Question 7

What is the equation relating the equilibrium constant K_n for the neutralization of a weak acid with a weak base to the K_a of the acid,the K_b of the base and K_w?

Accepted Answer

The answer of What is the equation relating the equilibrium...

Question 8

What is the common ion in a solution prepared by mixing 0.10 M NaCH₃CO₂ with 0.10 M CH₃CO₂H?

Accepted Answer

In the given solution, NaCH₃CO and CH₃COH both contain the common ion CH₃CO- (also known as bisulfite ion). Therefore, the common ion in the solution will also be CH₃CO-. The correct option containing this ion is C, CH₃CO₂^-. None of the other options includes this ion.

Question 9

What is the approximate value of the equilibrium constant,K_n,for the neutralization of hydrochloric acid with sodium hydroxide,shown in the equation below? HCl(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCl(aq)

Accepted Answer

The neutralization of a strong acid (HCl) with a strong base (NaOH) is a reaction that goes to completion, resulting in a very large equilibrium constant, approximately 10^14.

Question 10

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH₃CO₂H with 25.00 mL of 0.050 M CH₃CO₂Na? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃CO₂H.

Accepted Answer

The answer of What is the pH of a solution...

Question 11

When 50 mL of 0.10 M NH₄Cl is added to 50 mL of 0.10 M NH₃,relative to the pH of the 0.10 M NH₃solution the pH of the resulting solution will

Accepted Answer

NH₄Cl is an acidic compound, and adding it to the 0.10 M NH₃ solution will increase the overall concentration of acid in the solution. This will shift the equilibrium towards the formation of H+ ions, causing the pH to decrease. Therefore, the correct answer is (B) decrease.

Question 12

What is the approximate value of the equilibrium constant,K_n,for the neutralization of nitrous acid with ammonia,shown in the equation below? The K_a for HNO₂ is 4.5 × 10^-4 and the K_b for NH₃ is 1)8 × 10^-5. HNO₂(aq)+ NH₃(aq)⇌ NH₄NO₂(aq)

Accepted Answer

The equilibrium constant, K, can be calculated using the formula K = [NH₄NO₂]/[HNO₂][NH₃]. Substituting the given values, K = (1.8 × 10^-5) / (4.5 × 10^-4)^2 = 8.1 × 10⁵. Therefore, the answer is choice A.

Question 13

When 50 mL of 0.10 M NaF is added to 50 mL of 0.10 M HF,relative to the pH of the 0.10 M HF solution the pH of the resulting solution will

Accepted Answer

When NaF is added to HF, F- ions react with the H+ ions of HF to form HF2- ions, thereby decreasing the concentration of H+ ions in solution. This shift in equilibrium causes an increase in pH, making the resulting solution more basic. Therefore, pH of the resulting solution will increase.

Question 14

Which of these neutralization reactions has a pH = 7 when equal molar amounts of acid and base are mixed?

Accepted Answer

The neutralization reaction between HCl and NaOH produces NaCl and water, which has a neutral pH of 7. The other reaction options do not produce neutral solutions when equal molar amounts of acid and base are mixed.

Question 15

Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?

Accepted Answer

The answer of Which is a net ionic equation for...

Question 16

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH₃NH₂,with 25.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

Accepted Answer

First, we need to write out the reaction between methylamine and methylammonium chloride:

CH3NH2 + CH3NH3+Cl- → CH3NH3+ + CH3NH2Cl

Since both starting solutions are 0.10 M, we can assume that the concentration of CH3NH3+ and CH3NH2Cl formed is also 0.10 M.

Next, we need to determine the equilibrium constant (Kb) for methylamine:

Kb = Kw/Ka = 1.0 × 10^-14/4.4 × 10^-4 = 2.27 × 10^-11

Using the Henderson-Hasselbalch equation:

pH = pKb + log([CH3NH3+]/[CH3NH2])

pH = 9.64 + log(0.10/0.10)

pH = 9.64 + 0 = 9.64

Finally, we need to consider the effect of adding equal volumes of the two solutions. Since methylamine is a stronger base than methylammonium ion is an acid, the pH will increase.

The pKa of methylammonium ion (the acid conjugate of methylamine) is around 10.7, so we can expect the pH of the solution to be greater than this value.

The closest answer choice to this value is B) 10.57. Therefore, the best choice is B.

Question 17

Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?

Accepted Answer

The answer of Which of these neutralization reactions has a...

Question 18

The neutralization constant K_n for the neutralization of acetylsalicylic acid (C₉H₈O₄)and codeine (C₁₈H₂₁NO₃)is 4.8 × 10⁴.The acid dissociation constant K_a for acetylsalicylic acid is 3.0 × 10^-4.What is the base dissociation constant K_b for codeine?

Accepted Answer

The answer of The neutralization constant K_n for the neutralization...

Question 19

Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base?

Accepted Answer

In the reaction between a strong acid and a weak base, the weak base will not fully dissociate in water, so it will not have a complete ionic equation. Therefore, we only consider the species that participate in the reaction. In this case, the net ionic equation is:

HSO4- (aq) + NH3 (aq) → NH4+ (aq) + SO42- (aq)

Option D is the only one with this net ionic equation. The other options have different reactants and/or products.

Question 20

Which is a net ionic equation for the neutralization of a strong acid with a strong base?

Accepted Answer

The net ionic equation for the neutralization of a strong acid with a strong base is the reaction between H3O+ and OH- ions to form water.

Quiz 15: Applications of Aqueous Equilibria

What is the approximate value of the equilibrium constant,K_n,for the neutralization of acetic acid with sodium hydroxide,shown in the equation below? The K_a for acetic acid is 1.8 × 10^-5. CH₃CO₂H(aq) + NaOH(aq) ⇌ H₂O(l) + NaCH₃CO₂(aq)

The neutralization constant K_n for the neutralization of phenobarbital (C₁₂H₁₂N₂O₃) and morphine (C₁₇H₁₉NO₃) is 2.9.The acid dissociation constant K_a for phenobarbital is 3.9 × 10^-8.What is the base dissociation constant K_b for morphine?

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 25.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5 for NH₃.

Which is a net ionic equation for the neutralization of a weak acid with a strong base?

What is the approximate value of the equilibrium constant,K_n,for the neutralization of pyridine with hydrochloric acid,shown in the equation below? The K_b for pyridine is 1.8 × 10^-9. HCl(aq) + C₅H₅N(aq) ⇌ C₅H₅NHCl(aq)

Which of these neutralization reactions has a pH < 7 when equal molar amounts of acid and base are mixed?

What is the equation relating the equilibrium constant K_n for the neutralization of a weak acid with a weak base to the K_a of the acid,the K_b of the base and K_w?

What is the common ion in a solution prepared by mixing 0.10 M NaCH₃CO₂ with 0.10 M CH₃CO₂H?

What is the approximate value of the equilibrium constant,K_n,for the neutralization of hydrochloric acid with sodium hydroxide,shown in the equation below? HCl(aq) + NaOH(aq) ⇌ H₂O(l) + NaCl(aq)

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH₃CO₂H with 25.00 mL of 0.050 M CH₃CO₂Na? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃CO₂H.

When 50 mL of 0.10 M NH₄Cl is added to 50 mL of 0.10 M NH₃,relative to the pH of the 0.10 M NH₃solution the pH of the resulting solution will

What is the approximate value of the equilibrium constant,K_n,for the neutralization of nitrous acid with ammonia,shown in the equation below? The K_a for HNO₂ is 4.5 × 10^-4 and the K_b for NH₃ is 1) 8 × 10^-5. HNO₂(aq) + NH₃(aq) ⇌ NH₄NO₂(aq)

When 50 mL of 0.10 M NaF is added to 50 mL of 0.10 M HF,relative to the pH of the 0.10 M HF solution the pH of the resulting solution will

Which of these neutralization reactions has a pH = 7 when equal molar amounts of acid and base are mixed?

Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH₃NH₂,with 25.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?

The neutralization constant K_n for the neutralization of acetylsalicylic acid (C₉H₈O₄) and codeine (C₁₈H₂₁NO₃) is 4.8 × 10⁴.The acid dissociation constant K_a for acetylsalicylic acid is 3.0 × 10^-4.What is the base dissociation constant K_b for codeine?

Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base?

Which is a net ionic equation for the neutralization of a strong acid with a strong base?

Quiz 15: Applications of Aqueous Equilibria

What is the approximate value of the equilibrium constant,Kn,for the neutralization of acetic acid with sodium hydroxide,shown in the equation below? The Ka for acetic acid is 1.8 × 10-5. CH3CO2H(aq) + NaOH(aq) ⇌ H2O(l) + NaCH3CO2(aq)

The neutralization constant Kn for the neutralization of phenobarbital (C12H12N2O3) and morphine (C17H19NO3) is 2.9.The acid dissociation constant Ka for phenobarbital is 3.9 × 10-8.What is the base dissociation constant Kb for morphine?

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 25.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

Which is a net ionic equation for the neutralization of a weak acid with a strong base?

What is the approximate value of the equilibrium constant,Kn,for the neutralization of pyridine with hydrochloric acid,shown in the equation below? The Kb for pyridine is 1.8 × 10-9. HCl(aq) + C5H5N(aq) ⇌ C5H5NHCl(aq)

Which of these neutralization reactions has a pH < 7 when equal molar amounts of acid and base are mixed?

What is the equation relating the equilibrium constant Kn for the neutralization of a weak acid with a weak base to the Ka of the acid,the Kb of the base and Kw?

What is the common ion in a solution prepared by mixing 0.10 M NaCH3CO2 with 0.10 M CH3CO2H?

What is the approximate value of the equilibrium constant,Kn,for the neutralization of hydrochloric acid with sodium hydroxide,shown in the equation below? HCl(aq) + NaOH(aq) ⇌ H2O(l) + NaCl(aq)

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3CO2H with 25.00 mL of 0.050 M CH3CO2Na? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3CO2H.

When 50 mL of 0.10 M NH4Cl is added to 50 mL of 0.10 M NH3,relative to the pH of the 0.10 M NH3 solution the pH of the resulting solution will

What is the approximate value of the equilibrium constant,Kn,for the neutralization of nitrous acid with ammonia,shown in the equation below? The Ka for HNO2 is 4.5 × 10-4 and the Kb for NH3 is 1) 8 × 10-5. HNO2(aq) + NH3(aq) ⇌ NH4NO2(aq)

When 50 mL of 0.10 M NaF is added to 50 mL of 0.10 M HF,relative to the pH of the 0.10 M HF solution the pH of the resulting solution will

Which of these neutralization reactions has a pH = 7 when equal molar amounts of acid and base are mixed?

Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH3NH2,with 25.00 mL of 0.10 M methylammonium chloride,CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10-4 for methylamine.

Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?

The neutralization constant Kn for the neutralization of acetylsalicylic acid (C9H8O4) and codeine (C18H21NO3) is 4.8 × 104.The acid dissociation constant Ka for acetylsalicylic acid is 3.0 × 10-4.What is the base dissociation constant Kb for codeine?

Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base?

Which is a net ionic equation for the neutralization of a strong acid with a strong base?

What is the approximate value of the equilibrium constant,K_n,for the neutralization of acetic acid with sodium hydroxide,shown in the equation below? The K_a for acetic acid is 1.8 × 10^-5. CH₃CO₂H(aq) + NaOH(aq) ⇌ H₂O(l) + NaCH₃CO₂(aq)

The neutralization constant K_n for the neutralization of phenobarbital (C₁₂H₁₂N₂O₃) and morphine (C₁₇H₁₉NO₃) is 2.9.The acid dissociation constant K_a for phenobarbital is 3.9 × 10^-8.What is the base dissociation constant K_b for morphine?

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 25.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5 for NH₃.

What is the approximate value of the equilibrium constant,K_n,for the neutralization of pyridine with hydrochloric acid,shown in the equation below? The K_b for pyridine is 1.8 × 10^-9. HCl(aq) + C₅H₅N(aq) ⇌ C₅H₅NHCl(aq)

What is the equation relating the equilibrium constant K_n for the neutralization of a weak acid with a weak base to the K_a of the acid,the K_b of the base and K_w?

What is the common ion in a solution prepared by mixing 0.10 M NaCH₃CO₂ with 0.10 M CH₃CO₂H?

What is the approximate value of the equilibrium constant,K_n,for the neutralization of hydrochloric acid with sodium hydroxide,shown in the equation below? HCl(aq) + NaOH(aq) ⇌ H₂O(l) + NaCl(aq)

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH₃CO₂H with 25.00 mL of 0.050 M CH₃CO₂Na? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃CO₂H.

When 50 mL of 0.10 M NH₄Cl is added to 50 mL of 0.10 M NH₃,relative to the pH of the 0.10 M NH₃solution the pH of the resulting solution will

What is the approximate value of the equilibrium constant,K_n,for the neutralization of nitrous acid with ammonia,shown in the equation below? The K_a for HNO₂ is 4.5 × 10^-4 and the K_b for NH₃ is 1) 8 × 10^-5. HNO₂(aq) + NH₃(aq) ⇌ NH₄NO₂(aq)

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH₃NH₂,with 25.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

The neutralization constant K_n for the neutralization of acetylsalicylic acid (C₉H₈O₄) and codeine (C₁₈H₂₁NO₃) is 4.8 × 10⁴.The acid dissociation constant K_a for acetylsalicylic acid is 3.0 × 10^-4.What is the base dissociation constant K_b for codeine?