Question 1

The active ingredient in the antacid Tums is calcium carbonate, CaCO₃.What volume of 0.15 M stomach acid (HCl) could be neutralized by a dose of two tablets, each containing 500.0 mg of the active ingredient?

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Question 2

A perchloric acid solution is titrated using barium hydroxide.If the complete neutralization of 50.0 mL of the HClO₄ solution requires 37.0 mL of 0.125 M Ba(OH)₂, what is the molarity of the HClO₄?

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Question 3

Write the balanced molecular equation and the net ionic equation for the reaction of aqueous ammonium chloride with aqueous mercuryI) nitrate.

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Question 4

A barium hydroxide solution is titrated using nitric acid.A 260 mL portion of the Ba(OH)₂ solution requires 150 mL of 1.6 M HNO₃ to reach the equivalence point.In a second titration, it is found that 150 mL of the Ba(OH)₂ solution neutralized 450 mL of a sulfuric acid solution.What is the molarity of the H₂SO₄?

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Question 5

Identify which of the following ionic compounds are soluble in water.Answer yes or no in the table below.

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Question 6

Give the oxidation number of the atom in bold: K₂Cr₂O₇; PCl₃; NH₃; HNO₂; CaSO₄; P₄O₁₀.

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Question 7

Arsenic, which is toxic, can be removed from drinking water by precipitation as the sulfide.Write the net ionic equation for the precipitation of AS³⁺ using sodium sulfide, Na₂S.

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Question 8

Define the terms oxidation and reduction.

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Question 9

Write the formula and calculate the mass of the precipitate formed when excess aqueous potassium phosphate is mixed with 55.0 mL of 0.650 M magnesium nitrate.

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Question 10

Write the balanced molecular equation and the net ionic equation for the reaction of aqueous calcium chloride with aqueous sodium phosphate.

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Question 11

Write the balanced molecular equation and the net ionic equation for the reaction of aqueous cobalt(II) nitrate with aqueous potassium carbonate.

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Question 12

Some microorganisms living under anaerobic conditions extract oxygen from sulfate ions, producing hydrogen sulfide gas, which produces a distinctive rotten-egg odor.Write the balanced net ionic equation for this reaction under acidic conditions.

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Question 13

Aqueous potassium phosphate is added to 545 mL of a solution containing calcium chloride to precipitate all of the Ca²⁺ ions as the insoluble phosphate (310.2 g/mol).If 4.51 g calcium phosphate is produced, what is the Ca²⁺ concentration in the calcium chloride solution in g/L?

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Question 14

Define the terms oxidizing agent and reducing agent.

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Question 15

Ammonia, which is highly toxic to fish because it interferes with their uptake of oxygen, is formed from wastes excreted by the fish, uneaten food, and decaying plants.Beneficial bacteria oxidize the ammonia to nitrate, which is not highly toxic to fish in low to moderate levels.Complete and balance the reaction in basic solution.
$ \mathrm{NH}_{4}^{+}(a q)+\mathrm{O}_{2}(a q) \rightarrow \mathrm{NO}_{3}^{-}(a q) $

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Question 16

Outline a method that could be used to separate aqueous silver, chromium(III), and potassium ions from one another by precipitation.You many use any reagent that does not already contain one or more of these ions.

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Question 17

A saturated sucrose (C₁₂H₂₂O₁₁, 342.30 g/mol) solution at 25$\degree$C has an approximate concentration of 5.84 M.A solution is prepared by dissolving 424 g sucrose with water to a final volume of 265 mL.What is the molarity of this solution? If more solid sucrose is added, will it dissolve?

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Question 18

A food chemist determined the concentration of acetic acid in a sample of apple cider vinegar.The volume of 1.215 M NaOH required to titrate a 25.00 mL sample of the vinegar was 19.85 mL.The density of the sample was 1.01 g/mL.What are A) the molar concentration and B) the percent by mass of acetic acid in this vinegar? (CH₃COOH, 60.05 g/mol)

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Question 19

Aqueous sodium phosphate is added to 25.00 mL of a solution containing silver(I) nitrate.If 37.60 mL of 0.1140 M Na ₃PO₄ is required to completely precipitate all of the Ag⁺ ions as the insoluble phosphate (418.6 g/mol), what is the molar concentration of Ag⁺ in the silver(I) nitrate solution?

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Question 20

Give the formula for the precipitate that will form when the following aqueous solutions are mixed.If no precipitate forms, write "none."

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Quiz 8: Aqueous Solutions Chemistry of the Hydrosphere

The active ingredient in the antacid Tums is calcium carbonate, CaCO3.What volume of 0.15 M stomach acid (HCl) could be neutralized by a dose of two tablets, each containing 500.0 mg of the active ingredient?

A perchloric acid solution is titrated using barium hydroxide.If the complete neutralization of 50.0 mL of the HClO4 solution requires 37.0 mL of 0.125 M Ba(OH)2, what is the molarity of the HClO4?

Write the balanced molecular equation and the net ionic equation for the reaction of aqueous ammonium chloride with aqueous mercuryI) nitrate.

Identify which of the following ionic compounds are soluble in water.Answer yes or no in the table below.

Give the oxidation number of the atom in bold: K2Cr2O7; PCl3; NH3; HNO2; CaSO4; P4O10.

Arsenic, which is toxic, can be removed from drinking water by precipitation as the sulfide.Write the net ionic equation for the precipitation of AS3+ using sodium sulfide, Na2S.

Define the terms oxidation and reduction.

Write the formula and calculate the mass of the precipitate formed when excess aqueous potassium phosphate is mixed with 55.0 mL of 0.650 M magnesium nitrate.

Write the balanced molecular equation and the net ionic equation for the reaction of aqueous calcium chloride with aqueous sodium phosphate.

Write the balanced molecular equation and the net ionic equation for the reaction of aqueous cobalt(II) nitrate with aqueous potassium carbonate.

Some microorganisms living under anaerobic conditions extract oxygen from sulfate ions, producing hydrogen sulfide gas, which produces a distinctive rotten-egg odor.Write the balanced net ionic equation for this reaction under acidic conditions.

Aqueous potassium phosphate is added to 545 mL of a solution containing calcium chloride to precipitate all of the Ca2+ ions as the insoluble phosphate (310.2 g/mol).If 4.51 g calcium phosphate is produced, what is the Ca2+ concentration in the calcium chloride solution in g/L?

Define the terms oxidizing agent and reducing agent.

Outline a method that could be used to separate aqueous silver, chromium(III), and potassium ions from one another by precipitation.You many use any reagent that does not already contain one or more of these ions.

A saturated sucrose (C12H22O11, 342.30 g/mol) solution at 25 °\degree° C has an approximate concentration of 5.84 M.A solution is prepared by dissolving 424 g sucrose with water to a final volume of 265 mL.What is the molarity of this solution? If more solid sucrose is added, will it dissolve?

Aqueous sodium phosphate is added to 25.00 mL of a solution containing silver(I) nitrate.If 37.60 mL of 0.1140 M Na 3PO4 is required to completely precipitate all of the Ag+ ions as the insoluble phosphate (418.6 g/mol), what is the molar concentration of Ag+ in the silver(I) nitrate solution?

Give the formula for the precipitate that will form when the following aqueous solutions are mixed.If no precipitate forms, write "none."

The active ingredient in the antacid Tums is calcium carbonate, CaCO₃.What volume of 0.15 M stomach acid (HCl) could be neutralized by a dose of two tablets, each containing 500.0 mg of the active ingredient?

A perchloric acid solution is titrated using barium hydroxide.If the complete neutralization of 50.0 mL of the HClO₄ solution requires 37.0 mL of 0.125 M Ba(OH)₂, what is the molarity of the HClO₄?

Give the oxidation number of the atom in bold: K₂Cr₂O₇; PCl₃; NH₃; HNO₂; CaSO₄; P₄O₁₀.

Arsenic, which is toxic, can be removed from drinking water by precipitation as the sulfide.Write the net ionic equation for the precipitation of AS³⁺ using sodium sulfide, Na₂S.

Aqueous potassium phosphate is added to 545 mL of a solution containing calcium chloride to precipitate all of the Ca²⁺ ions as the insoluble phosphate (310.2 g/mol).If 4.51 g calcium phosphate is produced, what is the Ca²⁺ concentration in the calcium chloride solution in g/L?