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Chapter 4: Problem 46

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{CuSO}_{4}(a q)\) b. \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{CaCl}_{2}(a q)\) c. \(\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+\mathrm{MgI}_{2}(a q)\) d. \(\mathrm{Na}_{2} \mathrm{CrO}_{4}(a q)+\mathrm{AlBr}_{3}(a q)\)

Short Answer

Expert verified
When the following solutions are mixed together, these precipitates will form: a. \(Hg_{2}SO_{4}\) b. No precipitate c. \(MgCO_{3}\) d. \(Al_{2}(CrO_{4})_{3}\)

Step by step solution

01

Write Double Replacement Reactions

Write the balanced double replacement reactions for each pair of solutions: a. \(Hg_{2}(NO_{3})_{2}(aq) + CuSO_{4}(aq) \rightarrow Hg_{2}SO_{4}(s?) + Cu(NO_{3})_{2}(aq) \) b. \(Ni(NO_{3})_{2}(aq) + CaCl_{2}(aq) \rightarrow NiCl_{2}(s?) + Ca(NO_{3})_{2}(aq) \) c. \(K_{2}CO_{3}(aq) + MgI_{2}(aq) \rightarrow MgCO_{3}(s?) + 2KI(aq) \) d. \(Na_{2}CrO_{4}(aq) + AlBr_{3}(aq) \rightarrow Al_{2}(CrO_{4})_{3}(s?) + 6NaBr(aq) \)
02

Apply Solubility Rules

Check the solubility rules for each of the potential precipitates: a. \( Hg_{2}SO_{4} \) - Mercury(I) sulfate is insoluble, so it will form a precipitate. b. \( NiCl_{2} \) - Nickel(II) chloride is soluble, so it will not form a precipitate. c. \( MgCO_{3} \) - Magnesium carbonate is insoluble, so it will form a precipitate. d. \( Al_{2}(CrO_{4})_{3} \) - Aluminum chromate is insoluble, so it will form a precipitate.
03

Identify Precipitates

Identify the precipitate for each reaction: a. Precipitate: \( Hg_{2}SO_{4} \) b. Precipitate: None c. Precipitate: \( MgCO_{3} \) d. Precipitate: \( Al_{2}(CrO_{4})_{3} \) Now, we know the result when each of the mentioned solutions is mixed: a. \(Hg_{2}(NO_{3})_{2}(aq) + CuSO_{4}(aq)\) forms the precipitate \(Hg_{2}SO_{4}\). b. \(Ni(NO_{3})_{2}(aq) + CaCl_{2}(aq)\) forms no precipitate. c. \(K_{2}CO_{3}(aq) + MgI_{2}(aq)\) forms the precipitate \(MgCO_{3}\). d. \(Na_{2}CrO_{4}(aq) + AlBr_{3}(aq)\) forms the precipitate \(Al_{2}(CrO_{4})_{3}\).

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Most popular questions from this chapter

A \(1.42-\mathrm{g}\) sample of a pure compound, with formula \(\mathrm{M}_{2} \mathrm{SO}_{4}\), 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 \(1.36 \mathrm{~g}\). Determine the atomic mass of \(\mathrm{M}\), and identify \(\mathrm{M}\).

Differentiate between the following terms. a. species reduced versus the reducing agent b. species oxidized versus the oxidizing agent c. oxidation state versus actual charge

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{UO}_{2}^{2+}\) f. \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}\) b. \(\mathrm{As}_{2} \mathrm{O}_{3} \quad\) g. \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) c. \(\mathrm{NaBiO}_{3}\) h. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) d. As i. \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) e. \(\mathrm{HAsO}_{2}\)

How would you prepare \(1.00 \mathrm{~L}\) of a \(0.50 M\) solution of each of the following? a. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from "concentrated" \((18 M)\) sulfuric acid b. \(\mathrm{HCl}\) from "concentrated" \((12 \mathrm{M})\) reagent c. \(\mathrm{NiCl}_{2}\) from the salt \(\mathrm{NiCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) d. HNO \(_{3}\) from "concentrated" (16 M) reagent e. Sodium carbonate from the pure solid

When organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of \(\mathrm{SO}_{2}\) formed can be determined by reaction with hydrogen peroxide: $$ \mathrm{H}_{2} \mathrm{O}_{2}(a q)+\mathrm{SO}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q) $$ The resulting sulfuric acid is then titrated with a standard \(\mathrm{NaOH}\) solution. A \(1.325-\mathrm{g}\) sample of coal is burned and the \(\mathrm{SO}_{2}\) collected in a solution of hydrogen peroxide. It took \(28.44 \mathrm{~mL}\) of \(0.1000 \mathrm{M} \mathrm{NaOH}\) to neutralize the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.
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