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Chapter 4: Problem 94

You choose to investigate some of the solubility guidelines for two ions not listed in Table \(4.1,\) the chromate ion \(\left(\mathrm{CrO}_{4}^{2-}\right)\) and the oxalate ion \(\left(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\right) .\) You are given \(0.01 \mathrm{M}\) solutions \((\mathrm{A}, \mathrm{B}, \mathrm{C}, \mathrm{D})\) of four water- soluble salts: \begin{tabular}{lll} \hline Solution & Solute & Color of Solution \\ \hline \(\mathrm{A}\) & \(\mathrm{Na}_{2} \mathrm{CrO}_{4}\) & Yellow \\ \(\mathrm{B}\) & $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ & Colorless \\ \(\mathrm{C}\) & \(\mathrm{AgNO}_{3}\) & Colorless \\ \(\mathrm{D}\) & \(\mathrm{CaCl}_{2}\) & Colorless \\ \hline \end{tabular} When these solutions are mixed, the following observations are made: \begin{tabular}{lll} \hline Experiment Number & Solutions Mixed & Result \\ \hline 1 & \(\mathrm{~A}+\mathrm{B}\) & Noprecipitate, yellow solution \\ 2 & \(\mathrm{~A}+\mathrm{C}\) & Red precipitate forms \\ 3 & \(\mathrm{~A}+\mathrm{D}\) & Yellow precipitate forms \\ 4 & \(\mathrm{~B}+\mathrm{C}\) & White precipitate forms \\ 5 & \(\mathrm{~B}+\mathrm{D}\) & White precipitate forms \\ 6 & \(\mathrm{C}+\mathrm{D}\) & White precipitate forms \\ \hline \end{tabular} (a) Write a net ionic equation for the reaction that occurs in each of the experiments. (b) Identify the precipitate formed, if any, in each of the experiments.

Short Answer

Expert verified
(a) Net ionic equations for each experiment: 1. No reaction 2. \(2Ag^+(aq) + CrO_4^{2-}(aq) \rightarrow Ag_2CrO_4(s)\) 3. \(Ca^{2+}(aq) + CrO_4^{2-}(aq) \rightarrow CaCrO_4(s)\) 4. \(2Ag^+(aq) + C_2O_4^{2-}(aq) \rightarrow Ag_2C_2O_4(s)\) 5. \(Ca^{2+}(aq) + C_2O_4^{2-}(aq) \rightarrow CaC_2O_4(s)\) 6. \(Ag^+(aq) + Cl^-(aq) \rightarrow AgCl(s)\) (b) Precipitates formed in each experiment: 1. No precipitate 2. Red precipitate: \(Ag_2CrO_4\) 3. Yellow precipitate: \(CaCrO_4\) 4. White precipitate: \(Ag_2C_2O_4\) 5. White precipitate: \(CaC_2O_4\) 6. White precipitate: \(AgCl\)

Step by step solution

01

Experiment 1: A + B

Mixing Sodium chromate (\(Na_2CrO_4\)) with Ammonium oxalate (\((NH_4)_2C_2O_4\)): No precipitate is formed. So, there is no reaction and thus no net ionic equation.
02

Experiment 2: A + C

Mixing Sodium chromate (\(Na_2CrO_4\)) with Silver nitrate (\(AgNO_3\)): There is a red precipitate observed which means a reaction occurs. The possible reaction and products can be represented as follows: \(Na_2CrO_4(aq) + 2AgNO_3(aq) \rightarrow 2NaNO_3(aq) + Ag_2CrO_4(s)\) Net ionic equation: \(2Ag^+(aq) + CrO_4^{2-}(aq) \rightarrow Ag_2CrO_4(s)\)
03

Experiment 3: A + D

Mixing Sodium chromate (\(Na_2CrO_4\)) with Calcium chloride (\(CaCl_2\)): There is a yellow precipitate which means a reaction occurs. The possible reaction and products can be represented as follows: \(Na_2CrO_4(aq) + CaCl_2(aq) \rightarrow 2NaCl(aq) + CaCrO_4(s)\) Net ionic equation: \(Ca^{2+}(aq) + CrO_4^{2-}(aq) \rightarrow CaCrO_4(s)\)
04

Experiment 4: B + C

Mixing Ammonium oxalate (\((NH_4)_2C_2O_4\)) with Silver nitrate (\(AgNO_3\)): There is a white precipitate which means a reaction occurs. The possible reaction and products can be represented as follows: \(2AgNO_3(aq) + (NH_4)_2C_2O_4(aq) \rightarrow 2NH_4NO_3(aq) + Ag_2C_2O_4(s)\) Net ionic equation: \(2Ag^+(aq) + C_2O_4^{2-}(aq) \rightarrow Ag_2C_2O_4(s)\)
05

Experiment 5: B + D

Mixing Ammonium oxalate (\((NH_4)_2C_2O_4\)) with Calcium chloride (\(CaCl_2\)): There is a white precipitate which means a reaction occurs. The possible reaction and products can be represented as follows: \((NH_4)_2C_2O_4(aq) + CaCl_2(aq) \rightarrow 2NH_4Cl(aq) + CaC_2O_4(s)\) Net ionic equation: \(Ca^{2+}(aq) + C_2O_4^{2-}(aq) \rightarrow CaC_2O_4(s)\)
06

Experiment 6: C + D

Mixing Silver nitrate (\(AgNO_3\)) with Calcium chloride (\(CaCl_2\)): There is a white precipitate which means a reaction occurs. The possible reaction and products can be represented as follows: \(AgNO_3(aq) + CaCl_2(aq) \rightarrow Ca(NO_3)_2(aq) + AgCl(s)\) Net ionic equation: \(Ag^+(aq) + Cl^-(aq) \rightarrow AgCl(s)\) (b) Identify the precipitate formed, if any, in each of the experiments:
07

Experiment 1: A + B

No precipitate
08

Experiment 2: A + C

Red precipitate: \(Ag_2CrO_4\)
09

Experiment 3: A + D

Yellow precipitate: \(CaCrO_4\)
10

Experiment 4: B + C

White precipitate: \(Ag_2C_2O_4\)
11

Experiment 5: B + D

White precipitate: \(CaC_2O_4\)
12

Experiment 6: C + D

White precipitate: \(AgCl\)

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Most popular questions from this chapter

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