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 (A, B, C, D) of four water-soluble salts: $$ \begin{array}{lll} \hline \text { Solution } & \text { Solute } & \text { Color of Solution } \\ \hline \text { A } & \mathrm{Na}_{2} \mathrm{CrO}_{4} & \text { Yellow } \\ \mathrm{B} & \left(\mathrm{NH}_{4}\right)_{2} \mathrm{C}_{2} \mathrm{O}_{4} & \text { Colorless } \\ \mathrm{C} & \mathrm{AgNO}_{3} & \text { Colorless } \\ \mathrm{D} & \mathrm{CaCl}_{2} & \text { Colorless } \\ \hline \end{array} $$ When these solutions are mixed, the following observations are made: $$ \begin{array}{lll} \hline \text { Expt } & \text { Solutions } & \\ \text { Number } & \text { Mixed } & \text { Result } \\ \hline 1 & \mathrm{~A}+\mathrm{B} & \text { No precipitate, yellow solution } \\\ 2 & \mathrm{~A}+\mathrm{C} & \text { Red precipitate forms } \\ 3 & \mathrm{~A}+\mathrm{D} & \text { Yellow precipitate forms } \\ 4 & \mathrm{~B}+\mathrm{C} & \text { White precipitate forms } \\ 5 & \mathrm{~B}+\mathrm{D} & \text { White precipitate forms } \\ 6 & \mathrm{C}+\mathrm{D} & \text { White precipitate forms } \end{array} $$ (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.

Step by step solution

01

(Step 1: Identify the Interacting Ions)

Let's examine the reactions occurring in each experiment and determine which ions are interacting with each other to produce a precipitate. The experiments are: 1. A + B (No precipitate) 2. A + C (Red precipitate) 3. A + D (Yellow precipitate) 4. B + C (White precipitate) 5. B + D (White precipitate) 6. C + D (White precipitate) From these observations, we can see which salts are reacting with each other in each experiment, and it is apparent that the chromate ion is reacting with silver or calcium ions to form precipitates, while the oxalate ion is reacting with silver or calcium ions to form precipitates as well.

02

(Step 2: Write the Ion Interaction Equations)

Now that we have identified the ions interacting with each other, let's write the ion interaction equations for each experiment where a precipitate is formed: - For experiment 2: \(CrO^{2-}_4 + Ag^+ \rightarrow Ag_2CrO_4\) - For experiment 3: \(CrO^{2-}_4 + Ca^{2+} \rightarrow CaCrO_4\) - For experiment 4: \(C^{2-}_2O^2-_4 + Ag^+ \rightarrow Ag_2C_2O_4\) - For experiment 5: \(C^{2-}_2O^2-_4 + Ca^{2+} \rightarrow CaC_2O_4\) - For experiment 6: \(Cl^- + Ag^+ \rightarrow AgCl\)

03

(Step 3: Write the Net Ionic Equations)

Now, let's write the net ionic equations for each experiment: - Experiment 2: \(2Ag^+_{(aq)} + CrO^{2-}_{4(aq)} \rightarrow Ag_2CrO_{4(s)}\) - Experiment 3: \(Ca^{2+}_{(aq)} + CrO^{2-}_{4(aq)} \rightarrow CaCrO_{4(s)}\) - Experiment 4: \(2Ag^+_{(aq)} + C^{2-}_{2O^2-_4(aq)} \rightarrow Ag_2C_2O_{4(s)}\) - Experiment 5: \(Ca^{2+}_{(aq)} + C^{2-}_{2O^2-_4(aq)} \rightarrow CaC_2O_{4(s)}\) - Experiment 6: \(Ag^+_{(aq)} + Cl^-_{(aq)} \rightarrow AgCl_{(s)}\)

04

(Step 4: Identify the Precipitates Formed)

Finally, let's identify the precipitates formed in each experiment: - Experiment 2: Red precipitate (Silver chromate, \(Ag_2CrO_4\)) - Experiment 3: Yellow precipitate (Calcium chromate, \(CaCrO_4\)) - Experiment 4: White precipitate (Silver oxalate, \(Ag_2C_2O_4\)) - Experiment 5: White precipitate (Calcium oxalate, \(CaC_2O_4\)) - Experiment 6: White precipitate (Silver chloride, \(AgCl\))

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