The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of CO2 gas via mixing solid NiCO3 and aqueous hydriodic acid is ________.

A) 2NiCO3 (s) + HI (aq) → 2H2O (l) + CO2 (g) + 2Ni2+ (aq) B) NiCO3 (s) + I- (aq) → 2H2O (l) + CO2 (g) + Ni2+ (aq) + HI (aq) C) NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) D) NiCO3 (s) + 2HI (aq) → 2H2O (l) + CO2 (g) + NiI2 (aq) E) NiCO3 (s) + 2HI (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) + 2I- (aq) A) 2NiCO3 (s) + HI (aq) → 2H2O (l) + CO2 (g) + 2Ni2+ (aq) B) NiCO3 (s) + I- (aq) → 2H2O (l) + CO2 (g) + Ni2+ (aq) + HI (aq) C) NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) D) NiCO3 (s) + 2HI (aq) → 2H2O (l) + CO2 (g) + NiI2 (aq) E) NiCO3 (s) + 2HI (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) + 2I- (aq)

How many grams of H3PO4 are in 175 mL of a 4.00 M solution of H3PO4?

A) 0.700 B) 20.0 C) 68.6 D) 4.90 E) 612 A) 0.700 B) 20.0 C) 68.6 D) 4.90 E) 612

A 0.200 M K2SO4 solution is produced by ________.

A) dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L B) dissolving 43.6 g of K2SO4 in water and diluting to a total volume of 250.0 mL C) diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL D) dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL E) dilution of 1.00 mL of 250 M K2SO3 to 1.00 L A) dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L B) dissolving 43.6 g of K2SO4 in water and diluting to a total volume of 250.0 mL C) diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL D) dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL E) dilution of 1.00 mL of 250 M K2SO3 to 1.00 L

The molarity (M)of an aqueous solution containing 52.5 g of sucrose (C12H22O11)in 35.5 mL of solution is ________.

A) 5.46 B) 1.48 C) 0.104 D) 4.32 E) 1.85 A) 5.46 B) 1.48 C) 0.104 D) 4.32 E) 1.85

What are the respective concentrations (M)of Mg2+ and C2H3O2- afforded by dissolving 0.600 mol Mg(C2H3O2)2 in water and diluting to 135 mL?

A) 0.444 and 0.889 B) 0.0444 and 0.0889 C) 0..889 and 0.444 D) 0.444 and 0.444 E) 4.44 and 8.89 A) 0.444 and 0.889 B) 0.0444 and 0.0889 C) 0..889 and 0.444 D) 0.444 and 0.444 E) 4.44 and 8.89

The molarity (M)of an aqueous solution containing 22.5 g of glucose (C6H12O6)in 35.5 mL of solution is ________.

A) 3.52 B) 0.634 C) 0.197 D) 0.125 E) 1.85 A) 3.52 B) 0.634 C) 0.197 D) 0.125 E) 1.85

A stock solution of HNO3 is prepared and found to contain 12.7 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M.

A) 0.254 B) 1.57 C) 0.635 D) 635 E) 254 A) 0.254 B) 1.57 C) 0.635 D) 635 E) 254

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

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

Exam 4: Aqueous Reactions and Solution Stoichiometry

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The net ionic equation for formation of an aqueous solution of NiI₂ accompanied by evolution of CO₂ gas via mixing solid NiCO₃ and aqueous hydriodic acid is ________.

(Multiple Choice)

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Question 101

What volume (mL)of a 5.45 M lead nitrate solution must be diluted to 820.7 mL to make a 1.41 M solution of lead nitrate?

(Multiple Choice)

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Question 102

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.

(Short Answer)

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Question 103

How many grams of H₃PO₄ are in 175 mL of a 4.00 M solution of H₃PO₄?

(Multiple Choice)

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Question 104

A 17.5 mL sample of an acetic acid (CH₃CO₂H)solution required 29.6 mL of 0.250 M NaOH for neutralization. The concentration of acetic acid was ________ M.

(Multiple Choice)

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Question 105

A 0.200 M K₂SO₄solution is produced by ________.

(Multiple Choice)

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Question 106

The molarity (M)of an aqueous solution containing 52.5 g of sucrose (C₁₂H₂₂O₁₁)in 35.5 mL of solution is ________.

(Multiple Choice)

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Question 107

You are given two clear solutions of the same unknown monoprotic acid, but with different concentrations. Which statement is true?

(Multiple Choice)

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Question 108

Oxidation cannot occur without ________.

(Multiple Choice)

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Question 109

The reaction between strontium hydroxide and chloric acid produces ________.

(Multiple Choice)

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Question 110

What are the respective concentrations (M)of Mg²⁺ and C₂H₃O₂^- afforded by dissolving 0.600 mol Mg(C₂H₃O₂)₂in water and diluting to 135 mL?

(Multiple Choice)

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Question 111

With which of the following will the ammonium ion form an insoluble salt?

(Multiple Choice)

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Question 112

An aqueous ethanol solution (400 mL)was diluted to 4.00 L, giving a concentration of 0.0400 M. The concentration of the original solution was ________ M.

(Multiple Choice)

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Question 113

The molarity (M)of an aqueous solution containing 22.5 g of glucose (C₆H₁₂O₆)in 35.5 mL of solution is ________.

(Multiple Choice)

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Question 114

A stock solution of HNO₃ is prepared and found to contain 12.7 M of HNO₃. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M.

(Multiple Choice)

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Question 115

Which one of the following is a triprotic acid?

(Multiple Choice)

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Question 116

There are ________ mol of bromide ions in 0.500 L of a 0.350 M solution of AlBr₃.

(Multiple Choice)

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Question 117

A tenfold dilution of a sample solution can be obtained by taking ________.

(Multiple Choice)

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Question 118

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

(Multiple Choice)

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Question 119

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

(Multiple Choice)

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Question 120

Showing 101 - 120 of 180

Exam 4: Aqueous Reactions and Solution Stoichiometry

The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of CO2 gas via mixing solid NiCO3 and aqueous hydriodic acid is ________.

What volume (mL)of a 5.45 M lead nitrate solution must be diluted to 820.7 mL to make a 1.41 M solution of lead nitrate?

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.

How many grams of H3PO4 are in 175 mL of a 4.00 M solution of H3PO4?

A 17.5 mL sample of an acetic acid (CH3CO2H)solution required 29.6 mL of 0.250 M NaOH for neutralization. The concentration of acetic acid was ________ M.

A 0.200 M K2SO4 solution is produced by ________.

The molarity (M)of an aqueous solution containing 52.5 g of sucrose (C12H22O11)in 35.5 mL of solution is ________.

You are given two clear solutions of the same unknown monoprotic acid, but with different concentrations. Which statement is true?

Oxidation cannot occur without ________.

The reaction between strontium hydroxide and chloric acid produces ________.

What are the respective concentrations (M)of Mg2+ and C2H3O2- afforded by dissolving 0.600 mol Mg(C2H3O2)2 in water and diluting to 135 mL?

With which of the following will the ammonium ion form an insoluble salt?

An aqueous ethanol solution (400 mL)was diluted to 4.00 L, giving a concentration of 0.0400 M. The concentration of the original solution was ________ M.

The molarity (M)of an aqueous solution containing 22.5 g of glucose (C6H12O6)in 35.5 mL of solution is ________.

A stock solution of HNO3 is prepared and found to contain 12.7 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M.

Which one of the following is a triprotic acid?

There are ________ mol of bromide ions in 0.500 L of a 0.350 M solution of AlBr3.

A tenfold dilution of a sample solution can be obtained by taking ________.

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

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

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

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

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

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Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

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The net ionic equation for formation of an aqueous solution of NiI₂ accompanied by evolution of CO₂ gas via mixing solid NiCO₃ and aqueous hydriodic acid is ________.

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.

How many grams of H₃PO₄ are in 175 mL of a 4.00 M solution of H₃PO₄?

A 17.5 mL sample of an acetic acid (CH₃CO₂H)solution required 29.6 mL of 0.250 M NaOH for neutralization. The concentration of acetic acid was ________ M.

A 0.200 M K₂SO₄solution is produced by ________.

The molarity (M)of an aqueous solution containing 52.5 g of sucrose (C₁₂H₂₂O₁₁)in 35.5 mL of solution is ________.

What are the respective concentrations (M)of Mg²⁺ and C₂H₃O₂^- afforded by dissolving 0.600 mol Mg(C₂H₃O₂)₂in water and diluting to 135 mL?

The molarity (M)of an aqueous solution containing 22.5 g of glucose (C₆H₁₂O₆)in 35.5 mL of solution is ________.

A stock solution of HNO₃ is prepared and found to contain 12.7 M of HNO₃. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M.

There are ________ mol of bromide ions in 0.500 L of a 0.350 M solution of AlBr₃.

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