Question 1

How many grams of H3PO4 are in 175 mL of a 2.50 M solution of H3PO4?

Accepted Answer

A)  0.438
B)  20.0
C)  42.9
D)  4.90
E)  612 C

Question 2

What volume (mL)of a concentrated solution of sodium hydroxide (6.00 M)must be diluted to 200. mL to make a 1.50 M solution of sodium hydroxide?

Accepted Answer

A)  0.0500
B)  50.0
C)  45.0
D)  800.
E)  0.800 B

Question 3

Which hydroxides are weak bases?

Accepted Answer

A)  KOH, Ba(OH) 2
B)  Sr(OH) 2, KOH, NaOH, Ba(OH) 2
C)  KOH, NaOH
D)  KOH, NaOH, Ba(OH) 2
E)  None of these is a weak base. E

Question 4

Which combination will produce a precipitate?

Accepted Answer

A)  NaC2H3O2 (aq) and HCl (aq) 
B)  NaOH (aq) and HCl (aq) 
C)  AgNO3 (aq) and Ca(C2H3O2) 2 (aq) 
D)  KOH (aq) and Mg(NO3) 2 (aq)

Question 5

The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is __________.

Accepted Answer

A)  2H+ (aq) + 2OH- (aq) → 2 H2O (l) 
B)  2H+ (aq) + 2KOH (aq) → 2 H2O (l) + 2K+ (aq) 
C)  H2SO4 (aq) + 2OH- (aq) → 2 H2O (l) + SO42- (aq) 
D)  H2SO4 (aq) + 2KOH (aq) → 2 H2O (l) + K2SO4 (s) 
E)  H2SO4 (aq) + 2KOH (aq) → 2 H2O (l) + K2SO4 (aq)

Question 6

A 0.100 M solution of __________ will contain the highest concentration of potassium ions.

Accepted Answer

A)  potassium phosphate
B)  potassium hydrogen carbonate
C)  potassium hypochlorite
D)  potassium iodide
E)  potassium oxide

Question 7

How many grams of H₃PO₄ are in 265 mL of a 1.50 M solution of H₃PO₄?

Accepted Answer

The answer of How many grams of H₃PO₄ are in...

Question 8

The spectator ions in the reaction between aqueous chloric acid and aqueous barium hydroxide are __________.

Accepted Answer

A)  OH- and ClO3-
B)  H+, OH-, ClO3-, and Ba2+
C)  H+ and OH-
D)  H+ and Ba2+
E)  ClO3- and Ba2+

Question 9

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)  0.114
C)  0.454
D)  0.113
E)  0.227

Question 10

Which of the following reactions will not occur as written?

Accepted Answer

A)  Zn (s) + Pb(NO3) 2 (aq) → Pb (s) + Zn(NO3) 2 (aq) 
B)  Mg (s) + Ca(OH) 2 (aq) → Ca (s) + Mg(OH) 2 (aq) 
C)  Sn (s) + 2AgNO3 (aq) → 2Ag (s) + Sn(NO3) 2 (aq) 
D)  Co (s) + 2AgCl (aq) → 2Ag (s) + CoCl2 (aq) 
E)  Co (s) + 2HI (aq) → H2 (g) + CoI2 (aq)

Question 11

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

Accepted Answer

A)  0.0657
B)  1.85 × 12H22O11) in 35.5 mL of solution is __________. 
A)  0.0657 
B)  1.85 ×   
C)  1.85 
D)  3.52 
E)  0.104" class="answers-bank-image d-inline" rel="preload" >
C)  1.85
D)  3.52
E)  0.104

Question 12

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

Question 13

The reaction between strontium hydroxide and chloric acid produces __________.

Accepted Answer

A)  a molecular compound and a weak electrolyte
B)  two weak electrolytes
C)  two strong electrolytes
D)  a molecular compound and a strong electrolyte
E)  two molecular compounds

Question 14

Which one of the following substances is produced during the reaction of an acid with a metal hydroxide?

Accepted Answer

A)  H2
B)  H2O
C)  CO2
D)  NaOH
E)  O2

Question 15

Which one of the following compounds is insoluble in water?

Accepted Answer

A)  K2SO4
B)  Ca(C2H3O2) 2
C)  MgC2O4
D)  ZnCl2
E)  Mn(NO3) 2

Question 16

Which ion(s)is/are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl2 and AgNO3?

Accepted Answer

A)  Co2+ and NO3-
B)  NO3- and Cl-
C)  Co2+ and Ag+
D)  Cl-
E)  NO3-

Question 17

Which solution has the same number of moles of NaOH as 50.00 mL of 0.100M solution of NaOH?

Accepted Answer

A)  20.00 mL of 0.200M solution of NaOH
B)  25.00 mL of 0.175M solution of NaOH
C)  30.00 mL of 0.145M solution of NaOH
D)  50.00 mL of 0.125M solution of NaOH
E)  100.00 mL of 0.0500M solution of NaOH

Question 18

The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is __________.

Accepted Answer

A)  HNO3 (aq) + Sr(OH) 2 (aq) → Sr(NO3) 2 (aq) + H2 (g) 
B)  HNO3 (aq) + Sr(OH) 2 (aq) → H2O (l) + Sr(NO3) 2 (aq) 
C)  HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq) 
D)  2HNO3 (aq) + Sr(OH) 2 (aq) → 2 H2O (l) + Sr(NO3) 2 (aq) 
E)  2HNO3 (aq) + Sr(OH) 2 (aq) → Sr(NO3) 2 (aq) + 2 H2 (g)

Question 19

What volume (ml)of a 3.45 M lead nitrate solution must be diluted to 450.0 ml to make a 0.990 M solution of lead nitrate?

Accepted Answer

A)  129
B)  109
C)  101
D)  56
E)  45

Question 20

In a titration of 35.00 mL of 0.737 M H2SO4, __________ mL of a 0.827 M KOH solution is required for neutralization.

Accepted Answer

A)  35.0
B)  1.12
C)  25.8
D)  62.4
E)  39.3

Exam 4: Aqueous Reactions and Solution Stoichiometry

How many grams of H₃PO₄ are in 175 mL of a 2.50 M solution of H₃PO₄?

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200. mL to make a 1.50 M solution of sodium hydroxide?

Which hydroxides are weak bases?

Which combination will produce a precipitate?

The balanced molecular equation for complete neutralization of H₂SO₄ by KOH in aqueous solution is __________.

A 0.100 M solution of __________ will contain the highest concentration of potassium ions.

How many grams of H₃PO₄ are in 265 mL of a 1.50 M solution of H₃PO₄?

The spectator ions in the reaction between aqueous chloric acid and aqueous barium hydroxide are __________.

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 __________.

Which of the following reactions will not occur as written?

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

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?

The reaction between strontium hydroxide and chloric acid produces __________.

Which one of the following substances is produced during the reaction of an acid with a metal hydroxide?

Which one of the following compounds is insoluble in water?

Which ion(s) is/are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl₂ and AgNO₃?

Which solution has the same number of moles of NaOH as 50.00 mL of 0.100M solution of NaOH?

The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is __________.

What volume (ml) of a 3.45 M lead nitrate solution must be diluted to 450.0 ml to make a 0.990 M solution of lead nitrate?

In a titration of 35.00 mL of 0.737 M H₂SO₄, __________ mL of a 0.827 M KOH solution is required for neutralization.

Exam 4: Aqueous Reactions and Solution Stoichiometry

How many grams of H3PO4 are in 175 mL of a 2.50 M solution of H3PO4?

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200. mL to make a 1.50 M solution of sodium hydroxide?

Which hydroxides are weak bases?

Which combination will produce a precipitate?

The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is __________.

A 0.100 M solution of __________ will contain the highest concentration of potassium ions.

How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?

The spectator ions in the reaction between aqueous chloric acid and aqueous barium hydroxide are __________.

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 __________.

Which of the following reactions will not occur as written?

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

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?

The reaction between strontium hydroxide and chloric acid produces __________.

Which one of the following substances is produced during the reaction of an acid with a metal hydroxide?

Which one of the following compounds is insoluble in water?

Which ion(s) is/are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl2 and AgNO3?

Which solution has the same number of moles of NaOH as 50.00 mL of 0.100M solution of NaOH?

The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is __________.

What volume (ml) of a 3.45 M lead nitrate solution must be diluted to 450.0 ml to make a 0.990 M solution of lead nitrate?

In a titration of 35.00 mL of 0.737 M H2SO4, __________ mL of a 0.827 M KOH solution is required for neutralization.

How many grams of H₃PO₄ are in 175 mL of a 2.50 M solution of H₃PO₄?

The balanced molecular equation for complete neutralization of H₂SO₄ by KOH in aqueous solution is __________.

How many grams of H₃PO₄ are in 265 mL of a 1.50 M solution of H₃PO₄?

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

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?

Which ion(s) is/are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl₂ and AgNO₃?

In a titration of 35.00 mL of 0.737 M H₂SO₄, __________ mL of a 0.827 M KOH solution is required for neutralization.