How many milliliters of a stock solution of 11.1 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?

A) 0.0444 B) 22.5 C) 2.78 D) 44.4 E) 0.0225 A) 0.0444 B) 22.5 C) 2.78 D) 44.4 E) 0.0225

What are the respective concentrations (M)of Cu+2 and Cl- afforded by dissolving 0.200 mol CuCl2 in water and diluting to 345 mL?

A) 0.200 and 0.200 B) 0.580 and 1.16 C) 0.200 and 0.400 D) 1.16 and 2.32 E) 0.580 and 0.290 A) 0.200 and 0.200 B) 0.580 and 1.16 C) 0.200 and 0.400 D) 1.16 and 2.32 E) 0.580 and 0.290

How many grams of H3PO4 are in 175 mL of a 3.50 M solution of H3PO4?

A) 0.610 B) 60.0 C) 20.0 D) 4.90 E) 612 A) 0.610 B) 60.0 C) 20.0 D) 4.90 E) 612

What are the respective concentrations (M)of K+ and PO43- afforded by dissolving 0.800 mol K3PO4 in water and diluting to 1.63 L?

A) 0.800 and 0.800 B) 0.491 and 0.491 C) 0.800 and 0.491 D) 1.44 and 0.491 E) 0.489 and 0.163 A) 0.800 and 0.800 B) 0.491 and 0.491 C) 0.800 and 0.491 D) 1.44 and 0.491 E) 0.489 and 0.163

Exam 4: Aqueous Reactions and Solution Stoichiometry

A compound was found to be soluble in water. It was also found that addition of acid to an aqueous solution of this compound resulted in the formation of carbon dioxide. Which one of the following cations would form a precipitate when added to an aqueous solution of this compound?

(Multiple Choice)

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Question 81

What volume (mL)of a concentrated solution of magnesium chloride (9.00 M)must be diluted to 350. mL to make a 2.75 M solution of magnesium chloride?

(Multiple Choice)

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Question 82

What mass (g)of barium iodide is contained in 250 mL of a barium iodide solution that has an iodide ion concentration of 0.193 M?

(Multiple Choice)

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Question 83

Calculate the concentration (M)of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M solution of sodium sulfide to a total volume of 300 mL.

(Short Answer)

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Question 84

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 85

How many milliliters of a stock solution of 11.1 M HNO₃ would be needed to prepare 0.500 L of 0.500 M HNO₃?

(Multiple Choice)

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Question 86

How many moles of Co²⁺ are present in 0.150 L of a 0.200 M solution of CoI₂?

(Short Answer)

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Question 87

The point in a titration at which the indicator changes is called the __________.

(Multiple Choice)

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Question 88

What volume (L)of 0.250 M HNO₃ is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water?

(Multiple Choice)

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Question 89

Mixing 10.00 mL of an aqueous solution with 10.00 mL of water represents a __________.

(Multiple Choice)

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Question 90

What are the respective concentrations (M)of Cu⁺² and Cl^- afforded by dissolving 0.200 mol CuCl₂ in water and diluting to 345 mL?

(Multiple Choice)

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Question 91

How many grams of H₃PO₄ are in 175 mL of a 3.50 M solution of H₃PO₄?

(Multiple Choice)

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Question 92

The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is __________.

(Multiple Choice)

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Question 93

How many moles of K⁺ are present in 343 mL of a 1.27 M solution of K₃PO₄?

(Multiple Choice)

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Question 94

A 31.5 mL aliquot of HNO₃ (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M)of the acid was __________.

(Multiple Choice)

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Question 95

Which of these metals is the most easily oxidized? Na Au Fe Ca Ag

(Multiple Choice)

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Question 96

What volume (mL)of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl?

(Multiple Choice)

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Question 97

Which solution contains the largest number of moles of chloride ions?

(Multiple Choice)

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Question 98

What are the respective concentrations (M)of K⁺ and PO₄^3- afforded by dissolving 0.800 mol K₃PO₄in water and diluting to 1.63 L?

(Multiple Choice)

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Question 99

When aqueous solutions of __________ are mixed, a precipitate forms.

(Multiple Choice)

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Question 100

Showing 81 - 100 of 177

Exam 4: Aqueous Reactions and Solution Stoichiometry

A compound was found to be soluble in water. It was also found that addition of acid to an aqueous solution of this compound resulted in the formation of carbon dioxide. Which one of the following cations would form a precipitate when added to an aqueous solution of this compound?

What volume (mL)of a concentrated solution of magnesium chloride (9.00 M)must be diluted to 350. mL to make a 2.75 M solution of magnesium chloride?

What mass (g)of barium iodide is contained in 250 mL of a barium iodide solution that has an iodide ion concentration of 0.193 M?

Calculate the concentration (M)of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M solution of sodium sulfide to a total volume of 300 mL.

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.

How many milliliters of a stock solution of 11.1 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?

How many moles of Co2+ are present in 0.150 L of a 0.200 M solution of CoI2?

The point in a titration at which the indicator changes is called the __________.

What volume (L)of 0.250 M HNO3 is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water?

Mixing 10.00 mL of an aqueous solution with 10.00 mL of water represents a __________.

What are the respective concentrations (M)of Cu+2 and Cl- afforded by dissolving 0.200 mol CuCl2 in water and diluting to 345 mL?

How many grams of H3PO4 are in 175 mL of a 3.50 M solution of H3PO4?

The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is __________.

How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?

A 31.5 mL aliquot of HNO3 (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M)of the acid was __________.

Which of these metals is the most easily oxidized? Na Au Fe Ca Ag

What volume (mL)of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl?

Which solution contains the largest number of moles of chloride ions?

What are the respective concentrations (M)of K+ and PO43- afforded by dissolving 0.800 mol K3PO4 in water and diluting to 1.63 L?

When aqueous solutions of __________ are mixed, a precipitate forms.

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

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

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How many milliliters of a stock solution of 11.1 M HNO₃ would be needed to prepare 0.500 L of 0.500 M HNO₃?

How many moles of Co²⁺ are present in 0.150 L of a 0.200 M solution of CoI₂?

What volume (L)of 0.250 M HNO₃ is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water?

What are the respective concentrations (M)of Cu⁺² and Cl^- afforded by dissolving 0.200 mol CuCl₂ in water and diluting to 345 mL?

How many grams of H₃PO₄ are in 175 mL of a 3.50 M solution of H₃PO₄?

How many moles of K⁺ are present in 343 mL of a 1.27 M solution of K₃PO₄?

A 31.5 mL aliquot of HNO₃ (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M)of the acid was __________.

What are the respective concentrations (M)of K⁺ and PO₄^3- afforded by dissolving 0.800 mol K₃PO₄in water and diluting to 1.63 L?