Question 1

For any buffer system,the buffer capacity depends on the amount of acid and base from which the buffer is made.

Accepted Answer

A) True 
 B)False

Question 2

The pH of a solution prepared by dissolving 0.550 mol of solid methylamine hydrochloride (CH3NH3Cl)in   of   methylamine (CH3NH2)is ________.The Kb for methylamine is   (Assume the final volume is 1.00 L.)

Accepted Answer

A) 11.03 
B) 2.97 
C) 3.75 
D) 10.64 
E) 10.25 
A) 11.03 
B) 2.97 
C) 3.75 
D) 10.64 
E) 10.25

Question 3

The addition of KOH and ________ to water produces a buffer solution.

Accepted Answer

A) HI 
B) NH3 
C) KF 
D) LiC2H3O2 
E) none of the above 
A) HI 
B) NH3 
C) KF 
D) LiC2H3O2 
E) none of the above

Question 4

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (       H)and   of sodium benzoate (Na       )in water sufficient to yield 1.00 L of solution.The   of benzoic acid is

Accepted Answer

A) 4.409 
B) 3.965 
C) 10.035 
D) 9.591 
E) 5.190 
A) 4.409 
B) 3.965 
C) 10.035 
D) 9.591 
E) 5.190

Question 5

acid and   formate are required to prepare a buffer solution with a pH of 4.78 .The   of formic acid is

Accepted Answer

A) 0.17 
B) 0.083 
C) 3.3 × 103 
D) 0.041 
E) 9.8 
A) 0.17 
B) 0.083 
C) 3.3 × 103 
D) 0.041 
E) 9.8

Question 6

Which one of the following pairs cannot be mixed together to form a buffer solution?

Accepted Answer

A) C5H5N, C5H5NHCl 
B) HC2H3O2, NaOH (C2H3O2- = acetate) 
C) KOH, HI 
D) NH2CH3, HCl 
E) NaClO, HNO3 
A) C5H5N, C5H5NHCl 
B) HC2H3O2, NaOH (C2H3O2- = acetate) 
C) KOH, HI 
D) NH2CH3, HCl 
E) NaClO, HNO3

Question 7

The molar solubility of ________ is not affected by the pH of the solution.

Accepted Answer

A) Na3PO4 
B) NaF 
C) KNO3 
D) AlCl3 
E) MnS 
A) Na3PO4 
B) NaF 
C) KNO3 
D) AlCl3 
E) MnS

Question 8

Which is the correct   expression for PbCl2 (s)dissolving in water?

Accepted Answer

A)    = [Pb2+] [Cl-]2 
B)    = [Pb2+] [Cl-] 
C)    = [Pb2+]2 [Cl-] 
D)    = [PbCl+] [Cl-] 
E)    = [Pb+] [Cl2-]2 
A)    = [Pb2+] [Cl-]2 
B)    = [Pb2+] [Cl-] 
C)    = [Pb2+]2 [Cl-] 
D)    = [PbCl+] [Cl-] 
E)    = [Pb+] [Cl2-]2

Question 9

How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of   to the equivalence point?

Accepted Answer

A) 29.5 
B) 0.332 
C) 4.57 
D) 0.208 
E) 21.2 
A) 29.5 
B) 0.332 
C) 4.57 
D) 0.208 
E) 21.2

Question 10

In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility?

Accepted Answer

A) 0.020 M BaCl2 
B) 0.020 M Pb(NO3)2 
C) 0.020 M NaCl 
D) 0.020 M KCl 
E) pure water 
A) 0.020 M BaCl2 
B) 0.020 M Pb(NO3)2 
C) 0.020 M NaCl 
D) 0.020 M KCl 
E) pure water

Question 11

Metal oxides and hydroxides that are relatively insoluble in neutral water,but are soluble in both strongly acidic and strongly basic solutions are said to be ________.

Accepted Answer

The answer of Metal oxides and hydroxides that are relatively...

Question 12

The   of ammonia is 1.76 ×   .What is the pH of a buffer which is prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate?

Accepted Answer

A) 9.372 
B) 4.632 
C) 4.742 
D) 9.291 
E) none of the above 
A) 9.372 
B) 4.632 
C) 4.742 
D) 9.291 
E) none of the above

Question 13

What is the primary buffer system that controls the pH of the blood?

Accepted Answer

A) carbonate, bicarbonate 
B) carbon dioxide, carbonate 
C) carbonic acid, bicarbonate 
D) carbonic acid, carbon dioxide 
E) carbonate, carbonic acid 
A) carbonate, bicarbonate 
B) carbon dioxide, carbonate 
C) carbonic acid, bicarbonate 
D) carbonic acid, carbon dioxide 
E) carbonate, carbonic acid

Question 14

A complex ion is when a metal ion binds to a ________.

Accepted Answer

The answer of A complex ion is when a metal...

Question 15

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution.The equivalence point is reached when 10.2 mL of the base is added.The concentration of acetic acid in the sample was ________ M.

Accepted Answer

A) 0.365 
B) 0.175 
C) 0.119 
D) 0.0714 
E) none of the above 
A) 0.365 
B) 0.175 
C) 0.119 
D) 0.0714 
E) none of the above

Question 16

What is the pH of a solution that contains 0.800 M weak acid (   = 1.76 ×   )and 0.172 M of its conjugate base?

Accepted Answer

A) 8.578 
B) 5.422 
C) 8.370 
D) 4.087 
E) 9.913 
A) 8.578 
B) 5.422 
C) 8.370 
D) 4.087 
E) 9.913

Question 17

Which one of the following pairs cannot be mixed together to form a buffer solution?

Accepted Answer

A) NH3, NH4Cl 
B) NaC2H3O2, HCl (C2H3O2- = acetate) 
C) RbOH, HBr 
D) KOH, HF 
E) H3PO4, KH2PO4 
A) NH3, NH4Cl 
B) NaC2H3O2, HCl (C2H3O2- = acetate) 
C) RbOH, HBr 
D) KOH, HF 
E) H3PO4, KH2PO4

Question 18

Suppose you have just added 100.0 ml of a solution containing 1.00 mole of acetic acid per liter to 500.0 ml of 0.100 M KOH.What is the final pH?
 The Ka of acetic acid is 1.77 × 10-5.

Accepted Answer

Question 19

Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0 ml of 0.6000 M NaOH.What is the final pH?
 The Ka of HA is 1.77 × 10-5.

Accepted Answer

Question 20

In which of the following aqueous solutions would you expect CuBr to have the highest solubility?

Accepted Answer

A) 0.0100 M KBr 
B) 0.040 M CuNO3 
C) 0.030 M NaBr 
D) 0.020 M LiBr 
E) CuBr will have the same solubility in all solutions. 
A) 0.0100 M KBr 
B) 0.040 M CuNO3 
C) 0.030 M NaBr 
D) 0.020 M LiBr 
E) CuBr will have the same solubility in all solutions.

Exam 17: Additional Aspects of Aqueous Equilibria

For any buffer system,the buffer capacity depends on the amount of acid and base from which the buffer is made.

The pH of a solution prepared by dissolving 0.550 mol of solid methylamine hydrochloride (CH3NH3Cl)in of methylamine (CH3NH2)is ________.The Kb for methylamine is (Assume the final volume is 1.00 L.)

The addition of KOH and ________ to water produces a buffer solution.

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid ( H)and of sodium benzoate (Na )in water sufficient to yield 1.00 L of solution.The of benzoic acid is

acid and formate are required to prepare a buffer solution with a pH of 4.78 .The of formic acid is

Which one of the following pairs cannot be mixed together to form a buffer solution?

The molar solubility of ________ is not affected by the pH of the solution.

Which is the correct expression for PbCl2 (s)dissolving in water?

How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of to the equivalence point?

In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility?

Metal oxides and hydroxides that are relatively insoluble in neutral water,but are soluble in both strongly acidic and strongly basic solutions are said to be ________.

The of ammonia is 1.76 × .What is the pH of a buffer which is prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate?

What is the primary buffer system that controls the pH of the blood?

A complex ion is when a metal ion binds to a ________.

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution.The equivalence point is reached when 10.2 mL of the base is added.The concentration of acetic acid in the sample was ________ M.

What is the pH of a solution that contains 0.800 M weak acid ( = 1.76 × )and 0.172 M of its conjugate base?

Which one of the following pairs cannot be mixed together to form a buffer solution?

Suppose you have just added 100.0 ml of a solution containing 1.00 mole of acetic acid per liter to 500.0 ml of 0.100 M KOH.What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0 ml of 0.6000 M NaOH.What is the final pH? The Ka of HA is 1.77 × 10-5.

In which of the following aqueous solutions would you expect CuBr to have the highest solubility?

Introduction: Matter, energy, and Measurement

Atoms, molecules, and Ions

Chemical Reactions and Reaction Stoichiometry

Reactions in Aqueous Solution

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

The pH of a solution prepared by dissolving 0.550 mol of solid methylamine hydrochloride (CH₃NH₃Cl)in of methylamine (CH₃NH₂)is ________.The K_b for methylamine is (Assume the final volume is 1.00 L.)

Which is the correct expression for PbCl₂ (s)dissolving in water?

In which of the following aqueous solutions would you expect PbCl₂ to have the lowest solubility?

Suppose you have just added 100.0 ml of a solution containing 1.00 mole of acetic acid per liter to 500.0 ml of 0.100 M KOH.What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0 ml of 0.6000 M NaOH.What is the final pH? The K_a of HA is 1.77 × 10^-5.