Question 1

Of the metals below, only will not dissolve in an aqueous solution containing nickel ions.
Aluminum chromium barium tin potassium

Accepted Answer

A)  potassium 
B)  aluminum 
C)  barium 
D)  chromium 
E)  tin

Question 2

When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is .

Accepted Answer

A)  AgNO3 (aq) + KI (aq) - AgI (aq) + KNO3 (s) 
B)  Ag+ (aq) + NO3- (aq) - AgNO3 (aq) 
C)  Ag+ (aq) + I- (aq) - AgI (s) 
D)  AgNO3 (aq) + KI (aq) - AgI (s) + KNO3 (aq) 
E)  Ag+ (aq) + NO3- (aq) - AgNO3 (s)

Question 3

Oxidation and mean essentially the same thing.

Accepted Answer

A)  reduction 
B)  activity 
C)  decomposition 
D)  corrosion 
E)  metathesis

Question 4

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200 mL to make a 0.88 M solution of sodium hydroxide?

Accepted Answer

A)  26.4 
B)  176 
C)  29.3 
D)  50.0 
E)  2.64

Question 5

The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is .

Accepted Answer

A)  Al(OH)3 (s) + 3NO3- (aq) - 3OH- (aq) + Al(NO3)3 (s) 
B)  Al(OH)3 (s) + 3HNO3 (aq) - 3H2O (l) + Al(NO3)3 (aq) 
C)  Al(OH)3 (s) + 3H+ (aq) - 3H2O (l) + Al3+ (aq) 
D)  Al(OH)3 (s) + 3HNO3 (aq) - 3H2O (l) + Al3+ (aq) + NO3- (aq) 
E)  Al(OH)3 (s) + 3NO3- (aq) - 3OH- (aq) + Al(NO3)3 (aq)

Question 6

The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution is _ .

Accepted Answer

A)  1.85 × 10- 3 
B)  1.85 
C)  0.104 
D)  3.52 
E)  0.0657

Question 7

Which one of the following is a weak acid?

Accepted Answer

A)  HF 
B)  HClO4  
C)  HI 
D)  HCl 
E)  HNO3

Question 8

What is the concentration (M) of sodium ions in 4.57 L of a .398 M Na₃P solution?

Accepted Answer

The answer of What is the concentration (M) of sodium...

Question 9

Calculate the concentration (M) of arsenic acid (H₃AsO₄) in a solution if 25.00 mL of that solution required 35.21 mL of 0.1894 M KOH for neutralization.

Accepted Answer

The answer of Calculate the concentration (M) of arsenic acid...

Question 10

A neutralization reaction between an acid and a metal hydroxide produces .

Accepted Answer

A)  ammonia 
B)  sodium hydroxide 
C)  hydrogen gas 
D)  oxygen gas 
E)  water and a salt

Question 11

Oxidation cannot occur without .

Accepted Answer

A)  reduction 
B)  oxygen 
C)  air 
D)  water 
E)  acid

Question 12

There are mol of bromide ions in 0.500 L of a 0.300 M solution of AlBr3.

Accepted Answer

A)  0.167 
B)  0.500 
C)  0.150 
D)  0.450 
E)  0.0500

Question 13

Which of the following is an oxidation- reduction reaction?

Accepted Answer

A)  Cu (s) + 2AgNO3 (aq) - 2Ag (s) + Cu(NO3)2 (aq) 
B)  Ba(C2H3O2)2 (aq) + Na2SO4 (aq) - BaSO4 (s) + 2NaC2H3O2 (aq) 
C)  HCl (aq) + NaOH (aq) -H2O (l) + NaCl (aq) 
D)  AgNO3 (aq) + HCl (aq) - AgCl (s) + HNO3 (aq) 
E)  H2CO3 (aq) + Ca(NO3)2 (aq) - 2HNO3 (aq) + CaCO3 (s)

Question 14

How many moles of BaCl₂are formed in the neutralization of 393 mL of 0.171 M Ba(OH)₂ with aqueous HCl?

Accepted Answer

The answer of How many moles of BaCl₂are formed...

Question 15

When 0.500 mol of HC2H3O2 is combined with enough water to make a 300 mL solution, the concentration of HC2H3O2 is M.

Accepted Answer

A)  3.33 
B)  0.00167 
C)  0.835 
D)  1.67 
E)  0.150

Question 16

What is the concentration (M) of CH₃OH in a solution prepared by dissolving 16.8 g of C H₃OH in sufficient water to give exactly 230 mL of solution?

Accepted Answer

The answer of What is the concentration (M) of CH₃OH...

Question 17

A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq). It took 51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was .

Accepted Answer

A)  1.02 
B)  0.113 
C)  0.454 
D)  0.114 
E)  0.227

Question 18

What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid?

Accepted Answer

A)  188 
B)  34.5 
C)  1.44 
D)  1.23 
E)  53.6

Question 19

An aliquot (28.7 mL) of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass (g) of KOH was in the original sample?

Accepted Answer

A)  1.6 
B)  0.21 
C)  7.2 
D)  0.17 
E)  0.42

Question 20

Ammonia is a strong base.

Accepted Answer

A) True 
 B)False

Exam 4: Aqueous Reactions and Solution Stoichiometry

Of the metals below, only will not dissolve in an aqueous solution containing nickel ions. Aluminum chromium barium tin potassium

When aqueous solutions of AgNO₃and KI are mixed, AgI precipitates. The balanced net ionic equation is .

Oxidation and mean essentially the same thing.

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200 mL to make a 0.88 M solution of sodium hydroxide?

The net ionic equation for formation of an aqueous solution of Al(NO₃) ₃via mixing solid Al(OH) ₃ and aqueous nitric acid is .

The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C₁₂H₂₂O₁₁) in 35.5 mL of solution is _ .

Which one of the following is a weak acid?

What is the concentration (M) of sodium ions in 4.57 L of a .398 M Na₃P solution?

Calculate the concentration (M) of arsenic acid (H₃AsO₄) in a solution if 25.00 mL of that solution required 35.21 mL of 0.1894 M KOH for neutralization.

A neutralization reaction between an acid and a metal hydroxide produces .

Oxidation cannot occur without .

There are mol of bromide ions in 0.500 L of a 0.300 M solution of AlBr₃.

Which of the following is an oxidation- reduction reaction?

How many moles of BaCl₂are formed in the neutralization of 393 mL of 0.171 M Ba(OH)₂ with aqueous HCl?

When 0.500 mol of HC₂H₃O₂is combined with enough water to make a 300 mL solution, the concentration of HC₂H₃O₂is M.

What is the concentration (M) of CH₃OH in a solution prepared by dissolving 16.8 g of C H₃OH in sufficient water to give exactly 230 mL of solution?

A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq) . It took 51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was .

What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO₃is treated with an excess of aqueous hydrobromic acid?

An aliquot (28.7 mL) of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass (g) of KOH was in the original sample?

Ammonia is a strong base.

Exam 4: Aqueous Reactions and Solution Stoichiometry

Of the metals below, only will not dissolve in an aqueous solution containing nickel ions. Aluminum chromium barium tin potassium

When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is .

Oxidation and mean essentially the same thing.

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200 mL to make a 0.88 M solution of sodium hydroxide?

The net ionic equation for formation of an aqueous solution of Al(NO3) 3 via mixing solid Al(OH) 3 and aqueous nitric acid is .

The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution is _ .

Which one of the following is a weak acid?

What is the concentration (M) of sodium ions in 4.57 L of a .398 M Na3P solution?

Calculate the concentration (M) of arsenic acid (H3AsO4) in a solution if 25.00 mL of that solution required 35.21 mL of 0.1894 M KOH for neutralization.

A neutralization reaction between an acid and a metal hydroxide produces .

Oxidation cannot occur without .

There are mol of bromide ions in 0.500 L of a 0.300 M solution of AlBr3.

Which of the following is an oxidation- reduction reaction?

How many moles of BaCl2 are formed in the neutralization of 393 mL of 0.171 M Ba(OH)2 with aqueous HCl?

When 0.500 mol of HC2H3O2 is combined with enough water to make a 300 mL solution, the concentration of HC2H3O2 is M.

What is the concentration (M) of CH3OH in a solution prepared by dissolving 16.8 g of C H3OH in sufficient water to give exactly 230 mL of solution?

A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq) . It took 51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was .

What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid?

An aliquot (28.7 mL) of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass (g) of KOH was in the original sample?

Ammonia is a strong base.

When aqueous solutions of AgNO₃and KI are mixed, AgI precipitates. The balanced net ionic equation is .

The net ionic equation for formation of an aqueous solution of Al(NO₃) ₃via mixing solid Al(OH) ₃ and aqueous nitric acid is .

The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C₁₂H₂₂O₁₁) in 35.5 mL of solution is _ .

What is the concentration (M) of sodium ions in 4.57 L of a .398 M Na₃P solution?

Calculate the concentration (M) of arsenic acid (H₃AsO₄) in a solution if 25.00 mL of that solution required 35.21 mL of 0.1894 M KOH for neutralization.

There are mol of bromide ions in 0.500 L of a 0.300 M solution of AlBr₃.

How many moles of BaCl₂are formed in the neutralization of 393 mL of 0.171 M Ba(OH)₂ with aqueous HCl?

When 0.500 mol of HC₂H₃O₂is combined with enough water to make a 300 mL solution, the concentration of HC₂H₃O₂is M.

What is the concentration (M) of CH₃OH in a solution prepared by dissolving 16.8 g of C H₃OH in sufficient water to give exactly 230 mL of solution?

What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO₃is treated with an excess of aqueous hydrobromic acid?