Question 1

Complete the following reaction. ? + 2HNO3 $\rightarrow$Sr(NO3)2 + 2H2O

Accepted Answer

A)  Sr(OH)2 
B)  SrNO3 
C)  Sr2NO3 
D)  SrOH2 
E)  SrON3 
A)  Sr(OH)2 
B)  SrNO3 
C)  Sr2NO3 
D)  SrOH2 
E)  SrON3

Question 2

What mass of AgOH is present in a sample if it is titrated to its equivalence point with 58.5 mL of 0.0663 M HNO3? The balanced chemical equation is as follows: AgOH + HNO3 $\rightarrow$AgNO3 + H2O

Accepted Answer

A)  0.485 g 
B)  0.00388 g 
C)  258 g 
D)  1.13 g 
E)  2.27 g 
A)  0.485 g 
B)  0.00388 g 
C)  258 g 
D)  1.13 g 
E)  2.27 g

Question 3

Performing chemical reactions quantitatively to determine the exact amount of a reagent is called a(n)_____.

Accepted Answer

The answer of Performing chemical reactions quantitatively to determine the...

Question 4

If pOH < 7, then the solution is acidic.

Accepted Answer

A) True 
 B)False

Question 5

Pure water (pOH = 7) is an acidic solution.

Accepted Answer

A) True 
 B)False

Question 6

The titrant is added to the analyte using a precisely calibrated volumetric delivery tube called a buret.

Accepted Answer

A) True 
 B)False

Question 7

Which of the combinations of compounds can make a buffer solution?

Accepted Answer

A)  Ca(HCO3)2 and Ca(OH)2 
B)  CH3NH2 and CH3NH3Br 
C)  NaOH and NaCl 
D)  HCl and NaCl 
E)  NH3 and Ca(OH)2 
A)  Ca(HCO3)2 and Ca(OH)2 
B)  CH3NH2 and CH3NH3Br 
C)  NaOH and NaCl 
D)  HCl and NaCl 
E)  NH3 and Ca(OH)2

Question 8

What is [H+] in a 0.0066 M solution of Ba(OH)2?

Accepted Answer

A)  7.6 * 10-13 M 
B)  1.0 * 1014 M 
C)  1.0 * 10-13 M 
D)  1.5 * 10-12 M 
E)  0.0066 M 
A)  7.6 * 10-13 M 
B)  1.0 * 1014 M 
C)  1.0 * 10-13 M 
D)  1.5 * 10-12 M 
E)  0.0066 M

Question 9

HCOOH is a strong acid.

Accepted Answer

A) True 
 B)False

Question 10

Briefly describe autoionization of water. What is the autoionization constant of water?

Accepted Answer

Some H₂O molecules act as acids, and othe

Question 11

Which of the combinations of compounds can make a buffer solution?

Accepted Answer

A)  HCl and LiCl 
B)  HNO2 and HF 
C)  RbOH and CsOH 
D)  Rb2SO4 and HNO3 
E)  NH4NO3 and NH3 
A)  HCl and LiCl 
B)  HNO2 and HF 
C)  RbOH and CsOH 
D)  Rb2SO4 and HNO3 
E)  NH4NO3 and NH3

Question 12

Differentiate between strong bases and weak bases. Give an example of two strong acids and two strong bases.

Accepted Answer

Any base that dissociates 100% into ions

Question 13

Which of the following bases does not ionize 100% in aqueous solution?

Accepted Answer

A)  LiOH 
B)  Mg(OH)2 
C)  KOH 
D)  Ca(OH)2 
E)  Ni(OH)2 
A)  LiOH 
B)  Mg(OH)2 
C)  KOH 
D)  Ca(OH)2 
E)  Ni(OH)2

Question 14

Mg(OH)2 is a weak base.

Accepted Answer

A) True 
 B)False

Question 15

Buffers work well only for limited amounts of added strong acid or base. Once either solute is completely reacted, the solution is no longer a buffer, and rapid changes in pH may occur. We say that a buffer has a(n) ______.

Accepted Answer

The answer of Buffers work well only for limited amounts...

Question 16

Describe amphiprotic substances with an example.

Accepted Answer

A substance that can act as a proton don

Question 17

Explain why KNO3 cannot be a component in either an acidic or a basic buffer.

Accepted Answer

KNO₃ is a salt that is derived

Question 18

Salts with ions that are part of weak acids or bases will not hydrolyze, while salts with ions that are part of strong acids or bases will hydrolyze.

Accepted Answer

A) True 
 B)False

Question 19

Which of the following is a basic salt?

Accepted Answer

A)  LiCl 
B)  RbBr 
C)  KNO2 
D)  NaI 
E)  NH4Cl 
A)  LiCl 
B)  RbBr 
C)  KNO2 
D)  NaI 
E)  NH4Cl

Question 20

Which of the combinations of compounds can make a buffer solution?

Accepted Answer

A)  LiOH and LiCl 
B)  NaOH and NaBr 
C)  NaNO3 and Ca(NO3)2 
D)  NaHCO3 and Na2CO3 
E)  HN3 and NH3 
A)  LiOH and LiCl 
B)  NaOH and NaBr 
C)  NaNO3 and Ca(NO3)2 
D)  NaHCO3 and Na2CO3 
E)  HN3 and NH3

Complete the following reaction. ? + 2HNO₃ $\rightarrow$ Sr(NO₃)₂ + 2H₂O

What mass of AgOH is present in a sample if it is titrated to its equivalence point with 58.5 mL of 0.0663 M HNO₃? The balanced chemical equation is as follows: AgOH + HNO₃ $\rightarrow$ AgNO₃ + H₂O

Performing chemical reactions quantitatively to determine the exact amount of a reagent is called a(n)_____.

If pOH < 7, then the solution is acidic.

Pure water (pOH = 7) is an acidic solution.

The titrant is added to the analyte using a precisely calibrated volumetric delivery tube called a buret.

Which of the combinations of compounds can make a buffer solution?

What is [H⁺] in a 0.0066 M solution of Ba(OH)₂?

HCOOH is a strong acid.

Briefly describe autoionization of water. What is the autoionization constant of water?

Which of the combinations of compounds can make a buffer solution?

Differentiate between strong bases and weak bases. Give an example of two strong acids and two strong bases.

Which of the following bases does not ionize 100% in aqueous solution?

Mg(OH)₂ is a weak base.

Buffers work well only for limited amounts of added strong acid or base. Once either solute is completely reacted, the solution is no longer a buffer, and rapid changes in pH may occur. We say that a buffer has a(n) ______.

Describe amphiprotic substances with an example.

Explain why KNO₃ cannot be a component in either an acidic or a basic buffer.

Salts with ions that are part of weak acids or bases will not hydrolyze, while salts with ions that are part of strong acids or bases will hydrolyze.

Which of the following is a basic salt?

Which of the combinations of compounds can make a buffer solution?

What Is Chemistry

Measurements

Atoms, Molecules, and Ions

Chemical Reactions and Equations

Stoichiometry and the Mole

Gases

Energy and Chemistry

Electronic Structure

Chemical Bonds

Solids and Liquids

Solutions

Chemical Equilibrium

Oxidation and Reduction

Nuclear Chemistry

Organic Chemistry

Filters

Exam 12: Acids and Bases

Complete the following reaction. ? + 2HNO3 →\rightarrow→ Sr(NO3)2 + 2H2O

What mass of AgOH is present in a sample if it is titrated to its equivalence point with 58.5 mL of 0.0663 M HNO3? The balanced chemical equation is as follows: AgOH + HNO3 →\rightarrow→ AgNO3 + H2O

Performing chemical reactions quantitatively to determine the exact amount of a reagent is called a(n)_____.

If pOH < 7, then the solution is acidic.

Pure water (pOH = 7) is an acidic solution.

The titrant is added to the analyte using a precisely calibrated volumetric delivery tube called a buret.

Which of the combinations of compounds can make a buffer solution?

What is [H+] in a 0.0066 M solution of Ba(OH)2?

HCOOH is a strong acid.

Briefly describe autoionization of water. What is the autoionization constant of water?

Which of the combinations of compounds can make a buffer solution?

Differentiate between strong bases and weak bases. Give an example of two strong acids and two strong bases.

Which of the following bases does not ionize 100% in aqueous solution?

Mg(OH)2 is a weak base.

Buffers work well only for limited amounts of added strong acid or base. Once either solute is completely reacted, the solution is no longer a buffer, and rapid changes in pH may occur. We say that a buffer has a(n) ______.

Describe amphiprotic substances with an example.

Explain why KNO3 cannot be a component in either an acidic or a basic buffer.

Salts with ions that are part of weak acids or bases will not hydrolyze, while salts with ions that are part of strong acids or bases will hydrolyze.

Which of the following is a basic salt?

Which of the combinations of compounds can make a buffer solution?

What Is Chemistry

Measurements

Atoms, Molecules, and Ions

Chemical Reactions and Equations

Stoichiometry and the Mole

Gases

Energy and Chemistry

Electronic Structure

Chemical Bonds

Solids and Liquids

Solutions

Chemical Equilibrium

Oxidation and Reduction

Nuclear Chemistry

Organic Chemistry

Filters

Complete the following reaction. ? + 2HNO₃ $\rightarrow$ Sr(NO₃)₂ + 2H₂O

What mass of AgOH is present in a sample if it is titrated to its equivalence point with 58.5 mL of 0.0663 M HNO₃? The balanced chemical equation is as follows: AgOH + HNO₃ $\rightarrow$ AgNO₃ + H₂O

What is [H⁺] in a 0.0066 M solution of Ba(OH)₂?

Mg(OH)₂ is a weak base.

Explain why KNO₃ cannot be a component in either an acidic or a basic buffer.