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Chapter 4: Problem 7

Decide whether a precipitate will form when the following solutions are mixed. If a precipitate forms, write a net ionic equation for the reaction. (a) potassium nitrate and magnesium sulfate (b) silver nitrate and potassium carbonate (c) ammonium carbonate and cobalt(III) chloride (d) sodium phosphate and barium hydroxide (e) barium nitrate and potassium hydroxide

Short Answer

Expert verified
a) Potassium nitrate mixed with magnesium sulfate. b) Silver nitrate mixed with potassium carbonate. c) Ammonium carbonate mixed with cobalt(III) chloride. d) Sodium phosphate mixed with barium hydroxide. e) Barium nitrate mixed with potassium hydroxide. Answer: b) Silver nitrate mixed with potassium carbonate, c) Ammonium carbonate mixed with cobalt(III) chloride, and d) Sodium phosphate mixed with barium hydroxide will result in the formation of a precipitate.

Step by step solution

01

(a) Potassium nitrate and magnesium sulfate.

Both reactants are soluble in water. When mixed, they will form potassium sulfate and magnesium nitrate. These products are also soluble, so no precipitate will form in this case.
02

(b) Silver nitrate and potassium carbonate.

When mixed, they will form silver carbonate and potassium nitrate. Silver carbonate is insoluble in water and will precipitate. The net ionic equation: Ag^{+}(aq) + CO_3^{2-}(aq) -> Ag_2CO_3(s).
03

(c) Ammonium carbonate and cobalt(III) chloride.

When mixed, they will form cobalt(III) carbonate and ammonium chloride. Cobalt(III) carbonate is insoluble in water and will precipitate. The net ionic equation: Co^{3+}(aq) + 3CO_3^{2-}(aq) -> Co_2(CO_3)_3(s).
04

(d) Sodium phosphate and barium hydroxide.

When mixed, they will form barium phosphate and sodium hydroxide. Barium phosphate is insoluble in water and will precipitate. The net ionic equation: 3Ba^{2+}(aq) + 2PO_4^{3-}(aq) -> Ba_3(PO_4)_2(s).
05

(e) Barium nitrate and potassium hydroxide.

When mixed, they will form barium hydroxide and potassium nitrate. Both products are soluble in water, so no precipitate will form in this case.

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Most popular questions from this chapter

72\. Stomach acid is approximately \(0.020 \mathrm{M}\) HCl. What volume of this acid is neutralized by an antacid tablet that weighs \(330 \mathrm{mg}\) and contains \(41.0 \% \mathrm{Mg}(\mathrm{OH})_{2}, 36.2 \%\) \(\mathrm{NaHCO}_{3}\), and \(22.8 \% \mathrm{NaCl}\) ? The reactions involved are $$ \begin{aligned} \mathrm{Mg}(\mathrm{OH})_{2}(s)+2 \mathrm{H}^{+}(a q) & \longrightarrow \mathrm{Mg}^{2+}(a q)+2 \mathrm{H}_{2} \mathrm{O} \\ \mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}^{+}(a q) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O} \end{aligned} $$

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