Question 1

Match between columns
                        Premises: Brønsted-Lowry base
Arrhenius base
Lewis acid
Arrhenius acid
Brønsted-Lowry acid
Lewis base

Accepted Answer

The Answer of proton donor and produces hydroxide ions in is...

Question 2

What is the autoionization of water?

Accepted Answer

The answer of What is the autoionization of water?...

Question 3

What is the hydronium ion concentration of an acid solution that has a pH of 5.5?

Accepted Answer

The hydronium ion concentration can be calculated using the formula: pH = -log[H3O+]
5.5 = -log[H3O+]
[H3O+] = 3.6 × 10^-6 M, which corresponds to choice B.

Question 4

Calculate the pH of a 0.200 M NaCN solution.The K_a for HCN is 4.9 × 10^-10.

Accepted Answer

NaCN is a salt of a weak acid (HCN) and a strong base (NaOH). The CN- ion will hydrolyze in water to form OH- ions, making the solution basic. Using the formula for the hydrolysis of a salt of a weak acid, pH = 14 - 0.5(pKa - log(C)), where C is the concentration of the salt, we find the pH to be approximately 11.31.

Question 5

What is the pH of a 0.84 M solution of a base that has a K_b = 7.3 × 10^-10?

Accepted Answer

First, we need to find the pOH of the solution using the equation for the ionization constant of a base:

Kb = [OH-]^2/[B]

7.3 × 10-10 = [OH-]^2 / 0.84

[OH-] = 2.34 × 10-6 M

pOH = -log[OH-] = 5.63

pH = 14 - pOH = 8.37

Therefore, the pH of the solution is 9.39 (since it is a base, we need to add the pH to 7 to get the final answer). The answer is C.

Question 6

Calculate the pH of a 0.020 M carbonic acid solution,H₂CO₃₍_aq_),that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Accepted Answer

The pH is primarily determined by the first dissociation constant (Ka1) since it is much larger than Ka2. Using the formula for weak acid dissociation, pH = -log(sqrt(Ka1 * [H2CO3])), we find pH ≈ 4.03.

Question 7

What is the pOH of a 0.0020 M HNO₃ solution?

Accepted Answer

HNO3 is a strong acid, so it dissociates completely. The concentration of H+ ions is 0.0020 M, which means the pH is -log(0.0020) = 2.70. Since pH + pOH = 14, the pOH is 14 - 2.70 = 11.30.

Question 8

Do both protons ionize instantaneously from a diprotic acid such as H₂CO₃? Explain your answer.

Accepted Answer

The answer of Do both protons ionize instantaneously from a...

Question 9

What does the term amphoteric mean?

Accepted Answer

The answer of What does the term amphoteric mean?...

Question 10

Describe the relationship between molecular structure and acid strength.

Accepted Answer

The answer of Describe the relationship between molecular structure and...

Question 11

What is the selenide ion concentration [Se^2-] for a 0.300 M H₂Se solution that has the stepwise dissociation constants of and

Accepted Answer

The answer of What is the selenide ion concentration [Se^2-]...

Question 12

What is the pH of a 0.50 M H₂Se solution that has the stepwise dissociation constants K_a1 = 1.3 × 10^-4 and

Accepted Answer

The answer of What is the pH of a 0.50...

Question 13

Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.030 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Accepted Answer

The correct answer is A because the concentration of bicarbonate ion, HCO3-, in a 0.030 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11 is 1.1 × 10-4 M. This can be calculated using the following equation:[HCO3-] = Ka1 * [H2CO3] / [H+]where Ka1 is the first dissociation constant, [H2CO3] is the concentration of carbonic acid, and [H+] is the concentration of hydrogen ions.In this case, Ka1 = 4.3 × 10-7, [H2CO3] = 0.030 M, and [H+] can be calculated using the following equation:[H+] = sqrt(Ka1 * [H2CO3])where sqrt() is the square root function.Plugging in the values for Ka1 and [H2CO3], we get:[H+] = sqrt(4.3 × 10-7 * 0.030 M) = 1.1 × 10-4 MNow we can plug in the values for Ka1, [H2CO3], and [H+] into the first equation to get:[HCO3-] = 4.3 × 10-7 * 0.030 M / 1.1 × 10-4 M = 1.1 × 10-4 M

Question 14

Determine the K_a of an acid that has a pH of 3.29 and a concentration of 0.55 M.

Accepted Answer

The pH of 3.29 indicates an [H⁺] of 5.13 × 10⁻⁴ M. Using the formula Kₐ = [H⁺]² / [HA], where [HA] is the initial concentration of the acid (0.55 M), we find Kₐ = (5.13 × 10⁻⁴)² / 0.55 = 4.8 × 10⁻⁷.

Question 15

What is the difference between a strong and weak acid?

Accepted Answer

The answer of What is the difference between a strong...

Question 16

Describe a molecule that can be a Lewis acid.

Accepted Answer

The answer of Describe a molecule that can be a...

Question 17

Calculate the pH of a 0.80 M H₂SO₃,solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and

Accepted Answer

The answer of Calculate the pH of a 0.80 M...

Question 18

Which of the following is a Lewis base?

Accepted Answer

A Lewis base is a molecule or ion that donates a pair of electrons to form a covalent bond. In option B, the sulfur atom has a lone pair of electrons and can donate these electrons to form a bond. In option A, aluminum and chlorine do not have any lone pairs to donate, and in option C, silicon and chlorine do not have any lone pairs available for donation. In option D, both carbon and sulfur have lone pairs, but they also have a positively charged hydrogen atom, indicating that they are more likely to act as an acid than a base. Therefore, option B is the best choice for a Lewis base.

Question 19

Which of the following is a Lewis acid?

Accepted Answer

The answer of Which of the following is a Lewis...

Quiz 17: Acids and Bases

Match the following.

What is the autoionization of water?

What is the hydronium ion concentration of an acid solution that has a pH of 5.5?

Calculate the pH of a 0.200 M NaCN solution.The K_a for HCN is 4.9 × 10^-10.

What is the pH of a 0.84 M solution of a base that has a K_b = 7.3 × 10^-10?

Calculate the pH of a 0.020 M carbonic acid solution,H₂CO₃₍_aq_{) ,}that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

What is the pOH of a 0.0020 M HNO₃ solution?

Do both protons ionize instantaneously from a diprotic acid such as H₂CO₃? Explain your answer.

What does the term amphoteric mean?

Describe the relationship between molecular structure and acid strength.

What is the selenide ion concentration [Se^2-] for a 0.300 M H₂Se solution that has the stepwise dissociation constants of and

What is the pH of a 0.50 M H₂Se solution that has the stepwise dissociation constants K_a1 = 1.3 × 10^-4 and

Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.030 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Determine the K_a of an acid that has a pH of 3.29 and a concentration of 0.55 M.

What is the difference between a strong and weak acid?

Describe a molecule that can be a Lewis acid.

Calculate the pH of a 0.80 M H₂SO₃,solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and

Which of the following is a Lewis base?

Which of the following is a Lewis acid?

Quiz 17: Acids and Bases

Match the following.

What is the autoionization of water?

What is the hydronium ion concentration of an acid solution that has a pH of 5.5?

Calculate the pH of a 0.200 M NaCN solution.The Ka for HCN is 4.9 × 10-10.

What is the pH of a 0.84 M solution of a base that has a Kb = 7.3 × 10-10?

Calculate the pH of a 0.020 M carbonic acid solution,H2CO3(aq) ,that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

What is the pOH of a 0.0020 M HNO3 solution?

Do both protons ionize instantaneously from a diprotic acid such as H2CO3? Explain your answer.

What does the term amphoteric mean?

Describe the relationship between molecular structure and acid strength.

What is the selenide ion concentration [Se2-] for a 0.300 M H2Se solution that has the stepwise dissociation constants of and

What is the pH of a 0.50 M H2Se solution that has the stepwise dissociation constants Ka1 = 1.3 × 10-4 and

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.030 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Determine the Ka of an acid that has a pH of 3.29 and a concentration of 0.55 M.

What is the difference between a strong and weak acid?

Describe a molecule that can be a Lewis acid.

Calculate the pH of a 0.80 M H2SO3,solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and

Which of the following is a Lewis base?

Which of the following is a Lewis acid?

Calculate the pH of a 0.200 M NaCN solution.The K_a for HCN is 4.9 × 10^-10.

What is the pH of a 0.84 M solution of a base that has a K_b = 7.3 × 10^-10?

Calculate the pH of a 0.020 M carbonic acid solution,H₂CO₃₍_aq_{) ,}that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

What is the pOH of a 0.0020 M HNO₃ solution?

Do both protons ionize instantaneously from a diprotic acid such as H₂CO₃? Explain your answer.

What is the selenide ion concentration [Se^2-] for a 0.300 M H₂Se solution that has the stepwise dissociation constants of and

What is the pH of a 0.50 M H₂Se solution that has the stepwise dissociation constants K_a1 = 1.3 × 10^-4 and

Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.030 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Determine the K_a of an acid that has a pH of 3.29 and a concentration of 0.55 M.

Calculate the pH of a 0.80 M H₂SO₃,solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and