Question 1

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

Accepted Answer

Question 2

When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl,how many grams of AgCl are formed?
AgNO3(aq)+ NH4Cl(aq)→ AgCl(s)+ NH4NO3(aq)

Accepted Answer

A) 1.07 g 
B) 2.24 g 
C) 3.31 g 
D) 6.44 g 
A) 1.07 g 
B) 2.24 g 
C) 3.31 g 
D) 6.44 g

Question 3

What is the concentration (M)of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

Accepted Answer

The answer of What is the concentration (M)of a NaCl...

Question 4

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350.mL of solution?

Accepted Answer

A) 0.0101 M 
B) 0.0404 M 
C) 0.162 M 
D) 0.323 M 
A) 0.0101 M 
B) 0.0404 M 
C) 0.162 M 
D) 0.323 M

Question 5

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol.
4 KNO3(s)→ 2 K2O(s)+ 2 N2(g)+ 5 O2(g)

Accepted Answer

A) 23.2 mol O2 
B) 0.580 mol O2 
C) 18.5 mol O2 
D) 0.724 mol O2 
E) 1.73 mol O2 
A) 23.2 mol O2 
B) 0.580 mol O2 
C) 18.5 mol O2 
D) 0.724 mol O2 
E) 1.73 mol O2

Question 6

According to the following reaction,what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution?
2 KCl(aq)+ Pb(NO3)2(aq)→ PbCl2(s)+ 2 KNO3(aq)

Accepted Answer

A) 97.4 mL 
B) 116 mL 
C) 43.0 mL 
D) 86.1 mL 
E) 58.1 mL 
A) 97.4 mL 
B) 116 mL 
C) 43.0 mL 
D) 86.1 mL 
E) 58.1 mL

Question 7

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

Accepted Answer

Question 8

Which of the following solutions will have the highest electrical conductivity?

Accepted Answer

A) 0.045 M Al2(SO4)3 
B) 0.050 M (NH4)2CO3 
C) 0.10 M LiBr 
D) 0.10 M NaI 
E) 0.10 M KF 
A) 0.045 M Al2(SO4)3 
B) 0.050 M (NH4)2CO3 
C) 0.10 M LiBr 
D) 0.10 M NaI 
E) 0.10 M KF

Question 9

How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

Accepted Answer

A) 0.521 
B) 0.0120 
C) 83.7 
D) 0.0335 
E) 29.9 
A) 0.521 
B) 0.0120 
C) 83.7 
D) 0.0335 
E) 29.9

Question 10

How many aluminum ions are present in 65.5 mL of 0.210 M AlF3 solution?

Accepted Answer

A) 4.02 × 1023 aluminum ions 
B) 5.79 × 1024 aluminum ions 
C) 2.48 × 1022 aluminum ions 
D) 8.28 × 1021 aluminum ions 
E) 1.21 × 1022 aluminum ions 
A) 4.02 × 1023 aluminum ions 
B) 5.79 × 1024 aluminum ions 
C) 2.48 × 1022 aluminum ions 
D) 8.28 × 1021 aluminum ions 
E) 1.21 × 1022 aluminum ions

Question 11

How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution?

Accepted Answer

A) 1.31 × 10-3 mol 
B) 8.74 × 10-3 mol 
C) 1.14 × 10-3 mol 
D) 3.67 × 10-3 mol 
E) 7.65 × 10-3 mol 
A) 1.31 × 10-3 mol 
B) 8.74 × 10-3 mol 
C) 1.14 × 10-3 mol 
D) 3.67 × 10-3 mol 
E) 7.65 × 10-3 mol

Question 12

When 11.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction?
Ca(s)+ 2 H2O(l)→ Ca(OH)2(aq)+ H2(g)

Accepted Answer

A) 12.3% 
B) 24.6% 
C) 45.5% 
D) 84.0% 
A) 12.3% 
B) 24.6% 
C) 45.5% 
D) 84.0%

Question 13

What is the concentration of ions in a 0.25 M Al2(CO3)3 solution?

Accepted Answer

A) 0.25 M 
B) 1.00 M 
C) 1.25 M 
D) 0.50 M 
E) 0.75 M 
A) 0.25 M 
B) 1.00 M 
C) 1.25 M 
D) 0.50 M 
E) 0.75 M

Question 14

What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution? Hint: you will want to write a balanced reaction.

Accepted Answer

A) 581 mL 
B) 173 mL 
C) 345 mL 
D) 139 mL 
E) 278 mL 
A) 581 mL 
B) 173 mL 
C) 345 mL 
D) 139 mL 
E) 278 mL

Question 15

What reagent could be used to separate Br- from CH3CO2- when added to an aqueous solution containing both?

Accepted Answer

A) AgNO3(aq) 
B) Ba(OH)2(aq) 
C) CuSO4(aq) 
D) NaI(aq) 
A) AgNO3(aq) 
B) Ba(OH)2(aq) 
C) CuSO4(aq) 
D) NaI(aq)

Question 16

According to the following balanced reaction,how many moles of KO are required to exactly react with 5.44 moles of H2O?
4 KO(s)+ 2 H2O(l)→ 4 KOH(s)+ O2(g)

Accepted Answer

A) 5.44 moles H2O 
B) 10.9 moles H2O 
C) 21.8 moles H2O 
D) 2.72 moles H2O 
E) 1.36 moles H2O 
A) 5.44 moles H2O 
B) 10.9 moles H2O 
C) 21.8 moles H2O 
D) 2.72 moles H2O 
E) 1.36 moles H2O

Question 17

Give the theoretical yield,in moles,of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2.
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

Accepted Answer

A) 0.640 moles 
B) 64.0 moles 
C) 2.56 moles 
D) 16.0 moles 
A) 0.640 moles 
B) 64.0 moles 
C) 2.56 moles 
D) 16.0 moles

Question 18

According to the following reaction,how many moles of Fe(OH)2 can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl2.
FeCl2(aq)+ 2 LiOH(aq)→ Fe(OH)2(s)+ 2 LiCl(aq)

Accepted Answer

A) 3.97 × 10-2 moles 
B) 2.52 × 10-2 moles 
C) 1.99 × 10-2 moles 
D) 5.03 × 10-2 moles 
E) 6.49 × 10-2 moles 
A) 3.97 × 10-2 moles 
B) 2.52 × 10-2 moles 
C) 1.99 × 10-2 moles 
D) 5.03 × 10-2 moles 
E) 6.49 × 10-2 moles

Question 19

What mass,in g,of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution?
2 AgC2H3O2(aq)+ MgCl2(aq)→ 2 AgCl(s)+ Mg(C2H3O2)2(aq)

Accepted Answer

A) 0.838 g 
B) 1.72 g 
C) 0.859 g 
D) 2.56 g 
E) 1.70 g 
A) 0.838 g 
B) 1.72 g 
C) 0.859 g 
D) 2.56 g 
E) 1.70 g

Question 20

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

Accepted Answer

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

When 31.2 mL of 0.500 M AgNO₃ is added to 25.0 mL of 0.300 M NH₄Cl,how many grams of AgCl are formed? AgNO₃(aq)+ NH₄Cl(aq)→ AgCl(s)+ NH₄NO₃(aq)

What is the concentration (M)of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K₃PO₄ in enough water to make 350.mL of solution?

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g/mol. 4 KNO₃(s)→ 2 K₂O(s)+ 2 N₂(g)+ 5 O₂(g)

According to the following reaction,what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO₃)₂ solution? 2 KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2 KNO₃(aq)

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

Which of the following solutions will have the highest electrical conductivity?

How many milliliters of 0.132 M HClO₄ solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

How many aluminum ions are present in 65.5 mL of 0.210 M AlF₃ solution?

How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution?

When 11.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s)+ 2 H₂O(l)→ Ca(OH)₂(aq)+ H₂(g)

What is the concentration of ions in a 0.25 M Al₂(CO₃)₃ solution?

What volume of 0.305 M AgNO₃ is required to react exactly with 155.0 mL of 0.274 M Na₂SO₄ solution? Hint: you will want to write a balanced reaction.

What reagent could be used to separate Br^- from CH₃CO₂^-when added to an aqueous solution containing both?

According to the following balanced reaction,how many moles of KO are required to exactly react with 5.44 moles of H₂O? 4 KO(s)+ 2 H₂O(l)→ 4 KOH(s)+ O₂(g)

Give the theoretical yield,in moles,of CO₂from the reaction of 4.00 moles of C₈H₁₈ with 4.00 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

According to the following reaction,how many moles of Fe(OH)₂ can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl₂. FeCl₂(aq)+ 2 LiOH(aq)→ Fe(OH)₂(s)+ 2 LiCl(aq)

What mass,in g,of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC₂H₃O₂ solution with 55.0 mL of 0.109 M MgCl₂ solution? 2 AgC₂H₃O₂(aq)+ MgCl₂(aq)→ 2 AgCl(s)+ Mg(C₂H₃O₂)₂(aq)

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

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Exam 4: Chemical Quantities and Aqueous Reactions

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

When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl,how many grams of AgCl are formed? AgNO3(aq)+ NH4Cl(aq)→ AgCl(s)+ NH4NO3(aq)

What is the concentration (M)of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350.mL of solution?

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s)→ 2 K2O(s)+ 2 N2(g)+ 5 O2(g)

According to the following reaction,what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution? 2 KCl(aq)+ Pb(NO3)2(aq)→ PbCl2(s)+ 2 KNO3(aq)

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

Which of the following solutions will have the highest electrical conductivity?

How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

How many aluminum ions are present in 65.5 mL of 0.210 M AlF3 solution?

How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution?

When 11.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s)+ 2 H2O(l)→ Ca(OH)2(aq)+ H2(g)

What is the concentration of ions in a 0.25 M Al2(CO3)3 solution?

What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution? Hint: you will want to write a balanced reaction.

What reagent could be used to separate Br- from CH3CO2- when added to an aqueous solution containing both?

According to the following balanced reaction,how many moles of KO are required to exactly react with 5.44 moles of H2O? 4 KO(s)+ 2 H2O(l)→ 4 KOH(s)+ O2(g)

Give the theoretical yield,in moles,of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

According to the following reaction,how many moles of Fe(OH)2 can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl2. FeCl2(aq)+ 2 LiOH(aq)→ Fe(OH)2(s)+ 2 LiCl(aq)

What mass,in g,of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution? 2 AgC2H3O2(aq)+ MgCl2(aq)→ 2 AgCl(s)+ Mg(C2H3O2)2(aq)

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

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Liquids, Solids, and Intermolecular Forces

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

When 31.2 mL of 0.500 M AgNO₃ is added to 25.0 mL of 0.300 M NH₄Cl,how many grams of AgCl are formed? AgNO₃(aq)+ NH₄Cl(aq)→ AgCl(s)+ NH₄NO₃(aq)

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K₃PO₄ in enough water to make 350.mL of solution?

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g/mol. 4 KNO₃(s)→ 2 K₂O(s)+ 2 N₂(g)+ 5 O₂(g)

According to the following reaction,what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO₃)₂ solution? 2 KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2 KNO₃(aq)

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

How many milliliters of 0.132 M HClO₄ solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

How many aluminum ions are present in 65.5 mL of 0.210 M AlF₃ solution?

When 11.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction? Ca(s)+ 2 H₂O(l)→ Ca(OH)₂(aq)+ H₂(g)

What is the concentration of ions in a 0.25 M Al₂(CO₃)₃ solution?

What volume of 0.305 M AgNO₃ is required to react exactly with 155.0 mL of 0.274 M Na₂SO₄ solution? Hint: you will want to write a balanced reaction.

What reagent could be used to separate Br^- from CH₃CO₂^-when added to an aqueous solution containing both?

According to the following balanced reaction,how many moles of KO are required to exactly react with 5.44 moles of H₂O? 4 KO(s)+ 2 H₂O(l)→ 4 KOH(s)+ O₂(g)

Give the theoretical yield,in moles,of CO₂from the reaction of 4.00 moles of C₈H₁₈ with 4.00 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

According to the following reaction,how many moles of Fe(OH)₂ can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl₂. FeCl₂(aq)+ 2 LiOH(aq)→ Fe(OH)₂(s)+ 2 LiCl(aq)

What mass,in g,of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC₂H₃O₂ solution with 55.0 mL of 0.109 M MgCl₂ solution? 2 AgC₂H₃O₂(aq)+ MgCl₂(aq)→ 2 AgCl(s)+ Mg(C₂H₃O₂)₂(aq)

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