Question 1

The pKa for HC2H3O2(aq)is 4.76. What should be the pH of a mixture containing 100.0 mL of0.300 M NaC2H3O2(aq), 100 mL of 0.300 M HC2H3O2(aq), and 100 mL of 0.100 M NaOH?Hint: After neutralizing the acid and base, treat this solution as a buffer. Organizing your information will be just as important as applying chemistry concepts.

Accepted Answer

Question 2

A 0.075 M solution of a weak base in water has a pH = 11.21 at 25°C. Calculate the value of Kb for this base.

Accepted Answer

A)  1.6 × 10-3
B)  5.1 × 10-22
C)  2.2 × 10-2
D)  3.6 × 10-5
E)  6.2 × 10-12F) B) and E)
G) A) and C)

Question 3

A 0.350 M solution of an unknown base has a pH = 10.3. What is the value of the ionization constant, Kb, for the unknown base?

Accepted Answer

Question 4

Given the following:
0.20 M NaOH(aq) 
0.20 M HCl(aq) A mixture is made using 50.0 mL of the HCl and 50.0 mL of the NaOH.What is its pH at 25.0 °C?

Accepted Answer

A)  3.62
B)  4.57
C)  6.30
D)  7.00
E)  9.46F) B) and E)
G) A) and B)

Question 5

Hydrazine is a base, and the value of its constant, Kb, is 1.70 × 10-6. What is the value of pKb for this base?

Accepted Answer

A)  +4.30
B)  +5.77
C)  -5.77
D)  +8.23
E)  -8.23F) A) and E)
G) A) and B)

Question 6

At 60 °C the value of Kw is 9.5 × 10-14. Considering this, what is the pOH of pure water this temperature?

Accepted Answer

A)  6.02
B)  6.51
C)  7.00
D)  7.49
E)  9.50F) C) and D)
G) A) and B)

Question 7

Given 0.01 M solutions of each of the following acids, which solution would have the lowest pH?

Accepted Answer

A)  Hypoiodous acid (HOI) , Ka = 2.3 × 10-11
B)  Hypobromous acid (HOBr) , Ka = 2.5 × 10-9
C)  Lactic acid (HC3H5O3) , Ka = 1.3 × 10-4
D)  Chlorous acid (HClO2) , Ka = 1.1 × 10-2
E)  Boric acid (H3BO3) , Ka = 5.9 × 10-10F) D) and E)
G) B) and C)

Question 8

The pH at the equivalence point of the titration of ammonia solution by hydrochloric acid solution is

Accepted Answer

A)  
B)  4.00 
C)  7.00.
D)  7.00 
E)  > 11.0.F) A) and B)
G) B) and E)

Question 9

Calculate the pH of a 0.14 M HNO2 solution that is 5.7% ionized.

Accepted Answer

A)  11.90
B)  0.85
C)  1.70
D)  13.10
E)  2.10F) B) and C)
G) A) and C)

Question 10

Calculate the pH of a mixture made by adding 50.0 mL of 0.20 M HCl(aq) to 150.0 mL of water at 25.0 °C.

Accepted Answer

A)  0.70
B)  1.00
C)  1.18
D)  1.30
E)  13.00F) A) and D)
G) A) and B)

Question 11

Formic acid, HCO2H, has an ionization constant with the value: Ka = 1.76 × 10?4. Calculate the value of pKb for the formate ion, CO2H-, the conjugate base of formic acid.

Accepted Answer

A)  3.75
B)  5.35
C)  8.65
D)  10.25
E)  12.24F) All of the above
G) A) and B)

Question 12

Solutions of chlorine bleach contain the hypochlorite ion, OCl−, which is a weakbase. Write the appropriate equation for Kb for this anion.

Accepted Answer

The equation for the...

Question 13

A 0.200 M solution of an acid has a pH = 1.000. What is the value of the ionization constant, Ka, for this acid?

Accepted Answer

A)  0.200
B)  0.0400
C)  1.00 × 10-3
D)  1.00
E)  1.00 × 10-1F) A) and E)
G) A) and C)

Question 14

50.00 mL of 0.10 M HNO2 (nitrous acid, Ka = 4.5 × 10−4)is titrated with a 0.10 M KOH solution. What would be the pH of the solution after 25.00 mL of the KOH solution is added?Hint: After the partial neutralization, treat the solution as a buffer.

Accepted Answer

Question 15

What is the pH of a 1.00 molar solution of NaC2H3O2(aq) ?The Ka for acetic acid (HC2H3O2) is 1.8 × 10-5.

Accepted Answer

A)  2.37
B)  4.63
C)  4.75
D)  9.37
E)  11.63F) A) and E)
G) None of the above

Question 16

An aqueous solution of Ca(NO3)2 would result in a solution that would be ________.

Accepted Answer

Question 17

A scientist is testing a new cleaning chemical and measures the pH of the cleaner to be 10.70. What is the [H3O+] for this cleaner?

Accepted Answer

A)  2.0 × 10-11 M
B)  10.7 M
C)  9.3 × 10-10 M
D)  1.03 M
E)  5.0 × 10-10 MF) C) and D)
G) All of the above

Question 18

A mixture contains 400.0 mL of 1.00 M NH3(aq), whose pKb is = 4.76, and 400.0 mL of 1.00 M NH4Cl(aq). 200.0 mL of 0.0500 M HCl(aq)were added to the mixture. What is the pH of the buffer before addition of the acid and after addition of the acid? Hint: Calculate the pH of this buffer solution once before the acid and base are neutralized, and again once after. Organizing your information will be just as important as applying chemistry concepts.

Accepted Answer

Question 19

What is the pH of a 0.210 M solution of protonated pyridine, C5H5NH+?The Kb of pyridine is 1.5 × 10−9.Hint: Use Ka for weak acids and Kb for weak bases.

Accepted Answer

Pyridine is a weak base; the protonated ...

Question 20

The pH of a 0.0085 M HA (weak acid)solution is 4.70. What is the percent ionization of the acid in this solution?

Accepted Answer

The answer of The pH of a 0.0085 M HA...

Exam 17: Acid-Base Equilibria in Aqueous Solutions

At 60 °C the value of K_w is 9.5 × 10^-14. Considering this, what is the pOH of pure water this temperature?

Correct Answer
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Calculate the pH of a 0.14 M HNO₂ solution that is 5.7% ionized.

Correct Answer
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The pH at the equivalence point of the titration of ammonia solution by hydrochloric acid solution is

Correct Answer
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Hydrazine is a base, and the value of its constant, K_b, is 1.70 × 10^-6. What is the value of pK_b for this base?

Correct Answer
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Correct Answer
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An aqueous solution of Ca(NO₃)₂ would result in a solution that would be ________.

Correct Answer
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Given 0.01 M solutions of each of the following acids, which solution would have the lowest pH?

Correct Answer
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A 0.200 M solution of an acid has a pH = 1.000. What is the value of the ionization constant, K_a, for this acid?

Correct Answer
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Given the following: 0.20 M NaOH(aq) 0.20 M HCl(aq) A mixture is made using 50.0 mL of the HCl and 50.0 mL of the NaOH.What is its pH at 25.0 °C?

Correct Answer
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Correct Answer
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Solutions of chlorine bleach contain the hypochlorite ion, OCl⁻, which is a weakbase. Write the appropriate equation for K_b for this anion.

Correct Answer
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The equation for the...
View Answer

What is the pH of a 0.210 M solution of protonated pyridine, C₅H₅NH⁺?The K_b of pyridine is 1.5 × 10⁻⁹.Hint: Use K_a for weak acids and K_b for weak bases.

Correct Answer
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Pyridine is a weak base; the protonated ...
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A 0.075 M solution of a weak base in water has a pH = 11.21 at 25°C. Calculate the value of K_b for this base.

Correct Answer
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50.00 mL of 0.10 M HNO₂ (nitrous acid, K_a = 4.5 × 10⁻⁴)is titrated with a 0.10 M KOH solution. What would be the pH of the solution after 25.00 mL of the KOH solution is added?Hint: After the partial neutralization, treat the solution as a buffer.

Correct Answer
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A 0.350 M solution of an unknown base has a pH = 10.3. What is the value of the ionization constant, K_b, for the unknown base?

Correct Answer
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Calculate the pH of a mixture made by adding 50.0 mL of 0.20 M HCl(aq) to 150.0 mL of water at 25.0 °C.

Correct Answer
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Formic acid, HCO₂H, has an ionization constant with the value: K_a = 1.76 × 10^?4. Calculate the value of pK_b for the formate ion, CO₂H^-, the conjugate base of formic acid.

Correct Answer
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The pH of a 0.0085 M HA (weak acid)solution is 4.70. What is the percent ionization of the acid in this solution?

Correct Answer
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A scientist is testing a new cleaning chemical and measures the pH of the cleaner to be 10.70. What is the [H₃O⁺] for this cleaner?

Correct Answer
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What is the pH of a 1.00 molar solution of NaC₂H₃O₂(aq) ?The K_a for acetic acid (HC₂H₃O₂) is 1.8 × 10^-5.

Correct Answer
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Exam 17: Acid-Base Equilibria in Aqueous Solutions

At 60 °C the value of Kw is 9.5 × 10-14. Considering this, what is the pOH of pure water this temperature?

Correct AnswerverifiedShow Answer

Calculate the pH of a 0.14 M HNO2 solution that is 5.7% ionized.

Correct AnswerverifiedShow Answer

The pH at the equivalence point of the titration of ammonia solution by hydrochloric acid solution is

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Hydrazine is a base, and the value of its constant, Kb, is 1.70 × 10-6. What is the value of pKb for this base?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

An aqueous solution of Ca(NO3)2 would result in a solution that would be ________.

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Given 0.01 M solutions of each of the following acids, which solution would have the lowest pH?

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A 0.200 M solution of an acid has a pH = 1.000. What is the value of the ionization constant, Ka, for this acid?

Correct AnswerverifiedShow Answer

Given the following: 0.20 M NaOH(aq) 0.20 M HCl(aq) A mixture is made using 50.0 mL of the HCl and 50.0 mL of the NaOH.What is its pH at 25.0 °C?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Solutions of chlorine bleach contain the hypochlorite ion, OCl−, which is a weakbase. Write the appropriate equation for Kb for this anion.

Correct AnswerverifiedThe equation for the...View AnswerShow Answer

What is the pH of a 0.210 M solution of protonated pyridine, C5H5NH+?The Kb of pyridine is 1.5 × 10−9.Hint: Use Ka for weak acids and Kb for weak bases.

Correct AnswerverifiedPyridine is a weak base; the protonated ...View AnswerShow Answer

A 0.075 M solution of a weak base in water has a pH = 11.21 at 25°C. Calculate the value of Kb for this base.

Correct AnswerverifiedShow Answer

50.00 mL of 0.10 M HNO2 (nitrous acid, Ka = 4.5 × 10−4)is titrated with a 0.10 M KOH solution. What would be the pH of the solution after 25.00 mL of the KOH solution is added?Hint: After the partial neutralization, treat the solution as a buffer.

Correct AnswerverifiedShow Answer

A 0.350 M solution of an unknown base has a pH = 10.3. What is the value of the ionization constant, Kb, for the unknown base?

Correct AnswerverifiedShow Answer

Calculate the pH of a mixture made by adding 50.0 mL of 0.20 M HCl(aq) to 150.0 mL of water at 25.0 °C.

Correct AnswerverifiedShow Answer

Formic acid, HCO2H, has an ionization constant with the value: Ka = 1.76 × 10?4. Calculate the value of pKb for the formate ion, CO2H-, the conjugate base of formic acid.

Correct AnswerverifiedShow Answer

The pH of a 0.0085 M HA (weak acid)solution is 4.70. What is the percent ionization of the acid in this solution?

Correct AnswerverifiedShow Answer

A scientist is testing a new cleaning chemical and measures the pH of the cleaner to be 10.70. What is the [H3O+] for this cleaner?

Correct AnswerverifiedShow Answer

What is the pH of a 1.00 molar solution of NaC2H3O2(aq) ?The Ka for acetic acid (HC2H3O2) is 1.8 × 10-5.

Correct AnswerverifiedShow Answer

At 60 °C the value of K_w is 9.5 × 10^-14. Considering this, what is the pOH of pure water this temperature?

Correct Answer
verified

Calculate the pH of a 0.14 M HNO₂ solution that is 5.7% ionized.

Correct Answer
verified

Correct Answer
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Hydrazine is a base, and the value of its constant, K_b, is 1.70 × 10^-6. What is the value of pK_b for this base?

Correct Answer
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Correct Answer
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An aqueous solution of Ca(NO₃)₂ would result in a solution that would be ________.

Correct Answer
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Correct Answer
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A 0.200 M solution of an acid has a pH = 1.000. What is the value of the ionization constant, K_a, for this acid?

Correct Answer
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Correct Answer
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Correct Answer
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Solutions of chlorine bleach contain the hypochlorite ion, OCl⁻, which is a weakbase. Write the appropriate equation for K_b for this anion.

Correct Answer
verified
The equation for the...
View Answer

What is the pH of a 0.210 M solution of protonated pyridine, C₅H₅NH⁺?The K_b of pyridine is 1.5 × 10⁻⁹.Hint: Use K_a for weak acids and K_b for weak bases.

Correct Answer
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Pyridine is a weak base; the protonated ...
View Answer

A 0.075 M solution of a weak base in water has a pH = 11.21 at 25°C. Calculate the value of K_b for this base.

Correct Answer
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50.00 mL of 0.10 M HNO₂ (nitrous acid, K_a = 4.5 × 10⁻⁴)is titrated with a 0.10 M KOH solution. What would be the pH of the solution after 25.00 mL of the KOH solution is added?Hint: After the partial neutralization, treat the solution as a buffer.

Correct Answer
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A 0.350 M solution of an unknown base has a pH = 10.3. What is the value of the ionization constant, K_b, for the unknown base?

Correct Answer
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Correct Answer
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Formic acid, HCO₂H, has an ionization constant with the value: K_a = 1.76 × 10^?4. Calculate the value of pK_b for the formate ion, CO₂H^-, the conjugate base of formic acid.

Correct Answer
verified

Correct Answer
verified

A scientist is testing a new cleaning chemical and measures the pH of the cleaner to be 10.70. What is the [H₃O⁺] for this cleaner?

Correct Answer
verified

What is the pH of a 1.00 molar solution of NaC₂H₃O₂(aq) ?The K_a for acetic acid (HC₂H₃O₂) is 1.8 × 10^-5.

Correct Answer
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