Question 1

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr.Determine the pH of the solution before the addition of any HBr.

Accepted Answer

A) 12.86 
B) 13.00 
C) 13.30 
D) 0.70 
E) 1.00 
A) 12.86 
B) 13.00 
C) 13.30 
D) 0.70 
E) 1.00

Question 2

Match the following.
-pH = 7

Accepted Answer

A) half-way to equivalence point of a weak acid/strong base titration 
B) equivalence point of a strong acid/strong base titration 
C) equivalence point of a weak base/strong acid titration 
D) equivalence point of a weak acid/strong base titration 
A) half-way to equivalence point of a weak acid/strong base titration 
B) equivalence point of a strong acid/strong base titration 
C) equivalence point of a weak base/strong acid titration 
D) equivalence point of a weak acid/strong base titration

Question 3

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C?

Accepted Answer

A) 0.1 M HBr 
B) 0.1 M NaBr 
C) 0.1 M CaBr2 
D) 0.1 M K NO3 
A) 0.1 M HBr 
B) 0.1 M NaBr 
C) 0.1 M CaBr2 
D) 0.1 M K NO3

Question 4

Which of the following is true?

Accepted Answer

A) An effective buffer has a [base]/[acid] ratio in the range of 10 - 100. 
B) A buffer is most resistant to pH change when [acid] = [conjugate base] 
C) An effective buffer has very small absolute concentrations of acid and conjugate base. 
D) A buffer cannot be destroyed by adding too much strong base.It can only be destroyed by adding too much strong acid. 
E) None of the above are true. 
A) An effective buffer has a [base]/[acid] ratio in the range of 10 - 100. 
B) A buffer is most resistant to pH change when [acid] = [conjugate base] 
C) An effective buffer has very small absolute concentrations of acid and conjugate base. 
D) A buffer cannot be destroyed by adding too much strong base.It can only be destroyed by adding too much strong acid. 
E) None of the above are true.

Question 5

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of
0.30 M KClO.The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A) 5.99 
B) 8.01 
C) 7.54 
D) 7.71 
E) 6.46 
A) 5.99 
B) 8.01 
C) 7.54 
D) 7.71 
E) 6.46

Question 6

When titrating a monoprotic strong acid with a weak base at 25°C,the

Accepted Answer

A) pH will be 7 at the equivalence point. 
B) pH will be greater than 7 at the equivalence point. 
C) titration will require more moles of the base than acid to reach the equivalence point. 
D) titration will require more moles of acid than base to reach the equivalence point. 
E) pH will be less than 7 at the equivalence point. 
A) pH will be 7 at the equivalence point. 
B) pH will be greater than 7 at the equivalence point. 
C) titration will require more moles of the base than acid to reach the equivalence point. 
D) titration will require more moles of acid than base to reach the equivalence point. 
E) pH will be less than 7 at the equivalence point.

Question 7

A 1.0 L buffer solution is 0.050 M HC2H3O2 and 0.250 M LiC2H3O2.Which of the following actions will destroy the buffer?

Accepted Answer

A) adding 0.050 moles of NaOH 
B) adding 0.050 moles of HCl 
C) adding 0.050 moles of HC2H3O2 
D) adding 0.050 moles of LiC2H3O2 
E) None of the above will destroy the buffer. 
A) adding 0.050 moles of NaOH 
B) adding 0.050 moles of HCl 
C) adding 0.050 moles of HC2H3O2 
D) adding 0.050 moles of LiC2H3O2 
E) None of the above will destroy the buffer.

Question 8

Define a buffer.

Accepted Answer

Buffers contain significant am

A 100.0 mL sample of 0.10 M Ca(OH)₂ is titrated with 0.10 M HBr.Determine the pH of the solution before the addition of any HBr.

Match the following. -pH = 7

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25°C?

Which of the following is true?

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M KClO.The K_a for HClO is 2.9 × 10^-8.

When titrating a monoprotic strong acid with a weak base at 25°C,the

A 1.0 L buffer solution is 0.050 M HC₂H₃O₂ and 0.250 M LiC₂H₃O₂.Which of the following actions will destroy the buffer?

Define a buffer.

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Exam 16: Aqueous Ionic Equilibrium

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr.Determine the pH of the solution before the addition of any HBr.

Match the following. -pH = 7

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C?

Which of the following is true?

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M KClO.The Ka for HClO is 2.9 × 10-8.

When titrating a monoprotic strong acid with a weak base at 25°C,the

A 1.0 L buffer solution is 0.050 M HC2H3O2 and 0.250 M LiC2H3O2.Which of the following actions will destroy the buffer?

Define a buffer.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

A 100.0 mL sample of 0.10 M Ca(OH)₂ is titrated with 0.10 M HBr.Determine the pH of the solution before the addition of any HBr.

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25°C?

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M KClO.The K_a for HClO is 2.9 × 10^-8.

A 1.0 L buffer solution is 0.050 M HC₂H₃O₂ and 0.250 M LiC₂H₃O₂.Which of the following actions will destroy the buffer?