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You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.

b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges.

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You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.

a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any).

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A 1.42-g sample of a pure compound, with formula M2SO4, was dissolved in water and treated with an excess of aqueous calcium chloride, resulting in the precipitation of all the sulfate ions as calcium sulfate. The precipitate was collected, dried, and found to weigh 1.36 g. Determine the atomic mass of M, and identify M.

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What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO 3 is added to 20.0 mL of 1.00 M NaBr?

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What mass of barium sulfate can be produced when 100.0 mL of a 0.100 M solution of barium chloride is mixed with 100.0 mL of a 0.100 M solution of iron(III) sulfate?

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What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?

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What volume of 0.100 M Na3PO4 is required to precipitate all the lead(II) ions from 150.0 mL of 0.250 M Pb(NO3)2?

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What mass of Na2CrO4 is required to precipitate all of the silver ions from 75.0 mL of a 0.100 M solution of AgNO3?

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A sample may contain any or all of the following ions: Hg 22+, Ba2+, and Mn2+.
a. No precipitate formed when an aqueous solution of NaCl was added to the sample solution.
b. No precipitate formed when an aqueous solution of Na2SO4 was added to the sample solution.
c. A precipitate formed when the sample solution was made basic with NaOH.

Which ion or ions are present in the sample solution?

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Separate samples of a solution of an unknown soluble ionic compound are treated with KCl, Na2SO4, and NaOH. A precipitate forms only when Na 2SO4 is added. Which cations could be present in the unknown soluble ionic compound?

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Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.

d. strontium nitrate and potassium iodide

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Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.

c. copper(II) sulfate and mercury(I) nitrate

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Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.

b. silver nitrate and ammonium carbonate

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Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.

a. chromium(III) chloride and sodium hydroxide

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Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in each reaction?

 

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Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in each reaction?

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Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in each reaction?

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When the following solutions are mixed together, what precipitate (if any) will form?

d. Na2CrO4(aq) + AlBr3(aq)

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When the following solutions are mixed together, what precipitate (if any) will form?

c. K2CO3(aq) + MgI2(aq)

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When the following solutions are mixed together, what precipitate (if any) will form?

b. Ni(NO3)2(aq) + CaCl2(aq)

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When the following solutions are mixed together, what precipitate (if any) will form?

a. Hg2(NO3)2(aq) + CuSO4(aq)

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When the following solutions are mixed together, what precipitate (if any) will form?

c. CaCl2(aq) + Na2SO4(aq)

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When the following solutions are mixed together, what precipitate (if any) will form?

b. Al(NO3)3(aq) + Ba(OH)2(aq)

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When the following solutions are mixed together, what precipitate (if any) will form?

a. FeSO4(aq) + KCl(aq)

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On the basis of the general solubility rules given in Table 4.1, predict which of the following substances are likely to be soluble in water.

h. ammonium carbonate

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