The pH of a vinegar solution is 4.15.What is the H3O+ concentration of the solution?

A) 7.1 $\times$ 10-5 M B) 1.6 $\times$ 10-2 M C) 0.62 M D) 1.4 M E) 1.4 $\times$ 104 M A) 7.1 $\times$ 10-5 M B) 1.6 $\times$ 10-2 M C) 0.62 M D) 1.4 M E) 1.4 $\times$ 104 M

Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows: Cu2S(s)+ O2(g)$\to$ 2Cu(s)+ SO2(g) What mass of copper(I)sulfide is required in order to prepare 0.610 kg of copper metal?

A) 0.610 kg B) 0.305 kg C) 0.459 kg D) 1.53 kg E) 0.764 kg A) 0.610 kg B) 0.305 kg C) 0.459 kg D) 1.53 kg E) 0.764 kg

Potassium hydrogen carbonate decomposes with heat as follows: 2KHCO3(s)$\to$ K2CO3(s)+ CO2(g)+ H2O(l) How many moles of potassium carbonate will be produced if 201 g of potassium hydrogen carbonate are heated?

A) 1.00 mol B) 1.45 mol C) 10.8 mol D) 101 mol E) 2.01 mol A) 1.00 mol B) 1.45 mol C) 10.8 mol D) 101 mol E) 2.01 mol

The combustion of 0.0272 mole of a hydrocarbon produces 1.9609 g H2O and 3.5927 g CO2.What is the molar mass of the hydrocarbon?

A) 16.0 g/mol B) 30.1 g/mol C) 44.1 g/mol D) 72.2 g/mol E) 92.1 g/mol A) 16.0 g/mol B) 30.1 g/mol C) 44.1 g/mol D) 72.2 g/mol E) 92.1 g/mol

Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows: Cu2S(s)+ O2(g)$\to$ 2Cu(s)+ SO2(g) If the reaction of 0.630 kg of copper(I)sulfide with excess oxygen produces 0.190 kg of copper metal,what is the percent yield?

A) 75.5 % B) 39.9 % C) 30.2 % D) 151 % E) 37.8 % A) 75.5 % B) 39.9 % C) 30.2 % D) 151 % E) 37.8 %

An aqueous nitric acid solution has a pH of 2.15.What mass of HNO3 is present in 20.0 L of this solution?

A) 0.11 g B) 0.022 g C) 3.7 g D) 6.8 g E) 8.9 g A) 0.11 g B) 0.022 g C) 3.7 g D) 6.8 g E) 8.9 g

What mass of Na2CO3 is present in 0.250 L of a 0.852 M Na2CO3 solution?

A) 22.6 g B) 26.5 g C) 90.3 g D) 31.1 g E) 361 g A) 22.6 g B) 26.5 g C) 90.3 g D) 31.1 g E) 361 g

Zn reacts with hydrochloric acid. Zn(s)+ 2 HCl(aq)$\to$ ZnCl2(aq)+ H2(g) What volume of 3.05 M HCl(aq)will react with 25.0 g Zn(s)?

A) 0.251 L B) 4.01 L C) 0.125 L D) 0.0627 L E) 2.33 L A) 0.251 L B) 4.01 L C) 0.125 L D) 0.0627 L E) 2.33 L

Exam 5: Stoichiometry: Quantitative Information About Chemical Reactions

When strongly heated,boric acid breaks down to boric oxide and water.What mass of boric oxide is formed from the decomposition of 15.0 g B(OH)₃? 2 B(OH)₃(s) $\to$ B₂O₃(s)+ 3 H₂O(g)

(Multiple Choice)

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Question 21

An impure sample of benzoic acid (C₆H₅COOH,122.12 g/mol)is titrated with 0.8067 M NaOH.A 5.109-g sample requires 36.97 mL of titrant to reach the endpoint.What is the percent by mass of benzoic acid in the sample? C₆H₅COOH(aq)+ NaOH(aq) $\to$ NaC₆H₅COO(aq)+ H₂O(l)

(Multiple Choice)

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Question 22

A 50.00-mL sample of a weak monoprotic acid is titrated with 0.0955 M NaOH.At the endpoint,it is found that 32.56 mL of titrant was used.What was the concentration of the weak acid?

(Multiple Choice)

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Question 23

The pH of an aqueous NaOH solution is 12.83.What is the hydrogen ion concentration of this solution?

(Multiple Choice)

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Question 24

Calibration of a spectrophotmeter using a series of green dye containing solutions provides a set of data which follows the Beer-Lambert Law,with a trendline of y = 1.070 $\times$ 10³x (y-axis = absorbance,x-axis = molar concentration).What is the molar concentration of a solution with an absorbance of 0.3131?

(Multiple Choice)

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Question 25

The pH of a vinegar solution is 4.15.What is the H₃O⁺ concentration of the solution?

(Multiple Choice)

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Question 26

A compound consists of only C and F.It contains 38.71% C by mass.What is the empirical formula of the compound?

(Multiple Choice)

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Question 27

Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows: Cu₂S(s)+ O₂(g) $\to$ 2Cu(s)+ SO₂(g) What mass of copper(I)sulfide is required in order to prepare 0.610 kg of copper metal?

(Multiple Choice)

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Question 28

The reaction of 0.779 g K with O₂ forms 1.417 g potassium superoxide,a substance used in self-contained breathing devices.Determine the formula for potassium superoxide.

(Multiple Choice)

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Question 29

Potassium hydrogen carbonate decomposes with heat as follows: 2KHCO₃(s) $\to$ K₂CO₃(s)+ CO₂(g)+ H₂O(l) How many moles of potassium carbonate will be produced if 201 g of potassium hydrogen carbonate are heated?

(Multiple Choice)

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Question 30

Which of the following statements is/are CORRECT? 1)Absorbance is directly proportional to the intensity of the incident light. 2)Absorbance is inversely proportional to the analyte concentration. 3)Absorbance is directly proportional to the path length of the light.

(Multiple Choice)

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Question 31

The combustion of 0.0272 mole of a hydrocarbon produces 1.9609 g H₂O and 3.5927 g CO₂.What is the molar mass of the hydrocarbon?

(Multiple Choice)

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Question 32

Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows: Cu₂S(s)+ O₂(g) $\to$ 2Cu(s)+ SO₂(g) If the reaction of 0.630 kg of copper(I)sulfide with excess oxygen produces 0.190 kg of copper metal,what is the percent yield?

(Multiple Choice)

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Question 33

An aqueous nitric acid solution has a pH of 2.15.What mass of HNO₃ is present in 20.0 L of this solution?

(Multiple Choice)

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Question 34

One step in the isolation of pure rhodium metal (Rh)is the precipitation of rhodium(III)hydroxide from a solution containing rhodium(III)sulfate according to the following balanced chemical equation: Rh₂(SO₄)₃(aq)+ 6NaOH(aq) → 2Rh(OH)₃(s)+ 3Na₂SO₄(aq) If 6.20 g of rhodium(III)sulfate reacts with excess sodium hydroxide,what mass of rhodium(III)hydroxide may be produced?

(Multiple Choice)

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Question 35

What mass of Na₂CO₃ is present in 0.250 L of a 0.852 M Na₂CO₃ solution?

(Multiple Choice)

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Question 36

How many grams of dioxygen are required to completely burn 4.3 g of C₂H₅OH?

(Multiple Choice)

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Question 37

Zn reacts with hydrochloric acid. Zn(s)+ 2 HCl(aq) $\to$ ZnCl₂(aq)+ H₂(g) What volume of 3.05 M HCl(aq)will react with 25.0 g Zn(s)?

(Multiple Choice)

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Question 38

If 5.00 g Br₂ and 1.10 g NH₃ react according to the equation below,what is the maximum mass of ammonium bromide produced?

(Multiple Choice)

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Question 39

How many moles of Mg₃P₂(s)can be produced from the reaction of 0.14 mol Mg(s)with 0.020 mol P₄(s)? 6 Mg(s)+ P₄(s) $\to$ 2 Mg₃P₂(s)

(Multiple Choice)

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Question 40

Showing 21 - 40 of 76

Exam 5: Stoichiometry: Quantitative Information About Chemical Reactions

When strongly heated,boric acid breaks down to boric oxide and water.What mass of boric oxide is formed from the decomposition of 15.0 g B(OH)3? 2 B(OH)3(s) →\to→ B2O3(s)+ 3 H2O(g)

An impure sample of benzoic acid (C6H5COOH,122.12 g/mol)is titrated with 0.8067 M NaOH.A 5.109-g sample requires 36.97 mL of titrant to reach the endpoint.What is the percent by mass of benzoic acid in the sample? C6H5COOH(aq)+ NaOH(aq) →\to→ NaC6H5COO(aq)+ H2O(l)

A 50.00-mL sample of a weak monoprotic acid is titrated with 0.0955 M NaOH.At the endpoint,it is found that 32.56 mL of titrant was used.What was the concentration of the weak acid?

The pH of an aqueous NaOH solution is 12.83.What is the hydrogen ion concentration of this solution?

The pH of a vinegar solution is 4.15.What is the H3O+ concentration of the solution?

A compound consists of only C and F.It contains 38.71% C by mass.What is the empirical formula of the compound?

Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows: Cu2S(s)+ O2(g) →\to→ 2Cu(s)+ SO2(g) What mass of copper(I)sulfide is required in order to prepare 0.610 kg of copper metal?

The reaction of 0.779 g K with O2 forms 1.417 g potassium superoxide,a substance used in self-contained breathing devices.Determine the formula for potassium superoxide.

Potassium hydrogen carbonate decomposes with heat as follows: 2KHCO3(s) →\to→ K2CO3(s)+ CO2(g)+ H2O(l) How many moles of potassium carbonate will be produced if 201 g of potassium hydrogen carbonate are heated?

Which of the following statements is/are CORRECT? 1)Absorbance is directly proportional to the intensity of the incident light. 2)Absorbance is inversely proportional to the analyte concentration. 3)Absorbance is directly proportional to the path length of the light.

The combustion of 0.0272 mole of a hydrocarbon produces 1.9609 g H2O and 3.5927 g CO2.What is the molar mass of the hydrocarbon?

Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows: Cu2S(s)+ O2(g) →\to→ 2Cu(s)+ SO2(g) If the reaction of 0.630 kg of copper(I)sulfide with excess oxygen produces 0.190 kg of copper metal,what is the percent yield?

An aqueous nitric acid solution has a pH of 2.15.What mass of HNO3 is present in 20.0 L of this solution?

What mass of Na2CO3 is present in 0.250 L of a 0.852 M Na2CO3 solution?

How many grams of dioxygen are required to completely burn 4.3 g of C2H5OH?

Zn reacts with hydrochloric acid. Zn(s)+ 2 HCl(aq) →\to→ ZnCl2(aq)+ H2(g) What volume of 3.05 M HCl(aq)will react with 25.0 g Zn(s)?

If 5.00 g Br2 and 1.10 g NH3 react according to the equation below,what is the maximum mass of ammonium bromide produced?

How many moles of Mg3P2(s)can be produced from the reaction of 0.14 mol Mg(s)with 0.020 mol P4(s)? 6 Mg(s)+ P4(s) →\to→ 2 Mg3P2(s)

Basic Concepts of Chemistry

Mathlets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

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Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

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Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Chemistry of Solids

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Reactivity: Chemical Equilibria

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When strongly heated,boric acid breaks down to boric oxide and water.What mass of boric oxide is formed from the decomposition of 15.0 g B(OH)₃? 2 B(OH)₃(s) $\to$ B₂O₃(s)+ 3 H₂O(g)

An impure sample of benzoic acid (C₆H₅COOH,122.12 g/mol)is titrated with 0.8067 M NaOH.A 5.109-g sample requires 36.97 mL of titrant to reach the endpoint.What is the percent by mass of benzoic acid in the sample? C₆H₅COOH(aq)+ NaOH(aq) $\to$ NaC₆H₅COO(aq)+ H₂O(l)

The pH of a vinegar solution is 4.15.What is the H₃O⁺ concentration of the solution?

Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows: Cu₂S(s)+ O₂(g) $\to$ 2Cu(s)+ SO₂(g) What mass of copper(I)sulfide is required in order to prepare 0.610 kg of copper metal?

The reaction of 0.779 g K with O₂ forms 1.417 g potassium superoxide,a substance used in self-contained breathing devices.Determine the formula for potassium superoxide.

Potassium hydrogen carbonate decomposes with heat as follows: 2KHCO₃(s) $\to$ K₂CO₃(s)+ CO₂(g)+ H₂O(l) How many moles of potassium carbonate will be produced if 201 g of potassium hydrogen carbonate are heated?

The combustion of 0.0272 mole of a hydrocarbon produces 1.9609 g H₂O and 3.5927 g CO₂.What is the molar mass of the hydrocarbon?

Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows: Cu₂S(s)+ O₂(g) $\to$ 2Cu(s)+ SO₂(g) If the reaction of 0.630 kg of copper(I)sulfide with excess oxygen produces 0.190 kg of copper metal,what is the percent yield?

An aqueous nitric acid solution has a pH of 2.15.What mass of HNO₃ is present in 20.0 L of this solution?

What mass of Na₂CO₃ is present in 0.250 L of a 0.852 M Na₂CO₃ solution?

How many grams of dioxygen are required to completely burn 4.3 g of C₂H₅OH?

Zn reacts with hydrochloric acid. Zn(s)+ 2 HCl(aq) $\to$ ZnCl₂(aq)+ H₂(g) What volume of 3.05 M HCl(aq)will react with 25.0 g Zn(s)?

If 5.00 g Br₂ and 1.10 g NH₃ react according to the equation below,what is the maximum mass of ammonium bromide produced?

How many moles of Mg₃P₂(s)can be produced from the reaction of 0.14 mol Mg(s)with 0.020 mol P₄(s)? 6 Mg(s)+ P₄(s) $\to$ 2 Mg₃P₂(s)