Solubility Rules Worksheet for predicting solubility of compounds and labeling reaction products as soluble (aq) or insoluble (s).

To solve the problem, we need to use solubility rules to determine whether each compound is soluble (aq) or insoluble/solid (s). Here are the general solubility rules:

1. Salts of alkali metals (Group 1) and ammonium (NH₄⁺) are generally soluble.
2. Nitrates (NO₃⁻) are generally soluble.
3. Chlorides (Cl⁻) are generally soluble, except for AgCl, PbCl₂, and Hg₂Cl₂.
4. Sulfates (SO₄²⁻) are generally soluble, except for BaSO₄, PbSO₄, and CaSO₄ (slightly soluble).
5. Hydroxides (OH⁻) are generally insoluble, except for those of alkali metals and Ba(OH)₂, Sr(OH)₂, and Ca(OH)₂ (slightly soluble).
6. Carbonates (CO₃²⁻) are generally insoluble, except for those of alkali metals and NH₄⁺.
7. Sulfides (S²⁻) are generally insoluble, except for those of alkali metals, alkaline earth metals, and NH₄⁺.
8. Chromates (CrO₄²⁻) and phosphates (PO₄³⁻) are generally insoluble, except for those of alkali metals and NH₄⁺.

Step-by-Step Solution

#### Part 1: Predicting Solubility of Individual Compounds
We will use the solubility rules to determine whether each compound is soluble (aq) or insoluble/solid (s).

1. Cu(NO₃)₂: Nitrates are soluble. → aq
2. NaOH: Hydroxides of alkali metals are soluble. → aq
3. Na₂CrO₄: Chromates of alkali metals are soluble. → aq
4. KCN: Cyanides of alkali metals are soluble. → aq
5. MgCO₃: Carbonates are generally insoluble, except for those of alkali metals and NH₄⁺. → s
6. Mg(OH)₂: Hydroxides of Mg²⁺ are insoluble. → s
7. MgCrO₄: Chromates of Mg²⁺ are insoluble. → s
8. CuSO₄: Sulfates are generally soluble. → aq
9. NH₄Cl: Salts of NH₄⁺ are soluble. → aq
10. PbCrO₄: Chromates of Pb²⁺ are insoluble. → s
11. CuCl₂: Chlorides are generally soluble, except for AgCl, PbCl₂, and Hg₂Cl₂. → aq
12. Hg₂SO₄: Sulfates are generally soluble. → aq
13. NaCl: Salts of Na⁺ are soluble. → aq
14. Ag₂O: Oxides of Ag⁺ are insoluble. → s
15. Sn(SO₃)₂: Sulfites are generally insoluble, except for those of alkali metals and NH₄⁺. → s
16. Ba(C₂H₃O₂)₂: Salts of Ba²⁺ with acetate (C₂H₃O₂⁻) are soluble. → aq

#### Part 2: Labeling Reactants and Products in Reactions
We will use the solubility rules to determine the solubility of each compound in the given reactions.

1. Na₂SO₄ + BaCl₂ → 2 NaCl + BaSO₄
- Na₂SO₄: Sulfates are generally soluble. → aq
- BaCl₂: Chlorides are generally soluble. → aq
- NaCl: Salts of Na⁺ are soluble. → aq
- BaSO₄: Sulfates of Ba²⁺ are insoluble. → s

2. HCl + Ba(ClO₃)₂ → HClO₃ + BaCl₂
- HCl: Halides are generally soluble. → aq
- Ba(ClO₃)₂: Salts of Ba²⁺ with chlorate (ClO₃⁻) are soluble. → aq
- HClO₃: Halides are generally soluble. → aq
- BaCl₂: Chlorides are generally soluble. → aq

3. 2 Cr(NO₃)₃ + 3 (NH₄)₂S → Cr₂S₃ + 6 NH₄NO₃
- Cr(NO₃)₃: Nitrates are generally soluble. → aq
- (NH₄)₂S: Sulfides of NH₄⁺ are soluble. → aq
- Cr₂S₃: Sulfides of transition metals are insoluble. → s
- NH₄NO₃: Salts of NH₄⁺ are soluble. → aq

4. NaOH + NH₄Cl → NaCl + NH₄OH
- NaOH: Hydroxides of Na⁺ are soluble. → aq
- NH₄Cl: Salts of NH₄⁺ are soluble. → aq
- NaCl: Salts of Na⁺ are soluble. → aq
- NH₄OH: Ammonia solutions are considered soluble. → aq

5. KI + Pb(C₂H₃O₂)₂ → PbI₂ + KC₂H₃O₂
- KI: Salts of K⁺ are soluble. → aq
- Pb(C₂H₃O₂)₂: Salts of Pb²⁺ with acetate (C₂H₃O₂⁻) are soluble. → aq
- PbI₂: Iodides of Pb²⁺ are insoluble. → s
- KC₂H₃O₂: Salts of K⁺ are soluble. → aq

6. Ag(NO₃) + NH₄Cl → NH₄NO₃ + AgCl
- Ag(NO₃): Nitrates are generally soluble. → aq
- NH₄Cl: Salts of NH₄⁺ are soluble. → aq
- NH₄NO₃: Salts of NH₄⁺ are soluble. → aq
- AgCl: Chlorides of Ag⁺ are insoluble. → s

7. 2 HCl + K₂SO₃ → H₂SO₃ + 2 KCl
- HCl: Halides are generally soluble. → aq
- K₂SO₃: Sulfites of K⁺ are soluble. → aq
- H₂SO₃: Sulfurous acid is soluble. → aq
- KCl: Salts of K⁺ are soluble. → aq

8. 2 Rb(OH) + Cu(ClO₃)₂ → Cu(OH)₂ + 2 RbClO₃
- Rb(OH): Hydroxides of Rb⁺ are soluble. → aq
- Cu(ClO₃)₂: Salts of Cu²⁺ with chlorate (ClO₃⁻) are soluble. → aq
- Cu(OH)₂: Hydroxides of Cu²⁺ are insoluble. → s
- RbClO₃: Salts of Rb⁺ are soluble. → aq

9. 2 Fe(CN)₃ + 3 Li₂(CO₃) → Fe₂(CO₃)₃ + 6 LiCN
- Fe(CN)₃: Cyanides of Fe³⁺ are insoluble. → s
- Li₂(CO₃): Carbonates of Li⁺ are soluble. → aq
- Fe₂(CO₃)₃: Carbonates of Fe³⁺ are insoluble. → s
- LiCN: Cyanides of Li⁺ are soluble. → aq

10. 2 NaI + Pb(NO₃)₂ → PbI₂ + 2 NaNO₃
- NaI: Salts of Na⁺ are soluble. → aq
- Pb(NO₃)₂: Nitrates are generally soluble. → aq
- PbI₂: Iodides of Pb²⁺ are insoluble. → s
- NaNO₃: Salts of Na⁺ are soluble. → aq

Final Answer

\[
\boxed{
\begin{array}{cccc}
\text{Compound} & \text{Solubility} & \text{Compound} & \text{Solubility} \\
\hline
\text{Cu(NO₃)₂} & \text{aq} & \text{NaOH} & \text{aq} \\
\text{MgCO₃} & \text{s} & \text{Mg(OH)₂} & \text{s} \\
\text{NH₄Cl} & \text{aq} & \text{PbCrO₄} & \text{s} \\
\text{NaCl} & \text{aq} & \text{Ag₂O} & \text{s} \\
\text{Na₂CrO₄} & \text{aq} & \text{MgCrO₄} & \text{s} \\
\text{CuCl₂} & \text{aq} & \text{Sn(SO₃)₂} & \text{s} \\
\text{KCN} & \text{aq} & \text{Ba(C₂H₃O₂)₂} & \text{aq} \\
\text{CuSO₄} & \text{aq} & \text{Hg₂SO₄} & \text{aq} \\
\end{array}
}
\]
\[
\boxed{
\begin{array}{l}
1. \text{Na₂SO₄ (aq) + BaCl₂ (aq) → 2 NaCl (aq) + BaSO₄ (s)} \\
2. \text{HCl (aq) + Ba(ClO₃)₂ (aq) → HClO₃ (aq) + BaCl₂ (aq)} \\
3. \text{2 Cr(NO₃)₃ (aq) + 3 (NH₄)₂S (aq) → Cr₂S₃ (s) + 6 NH₄NO₃ (aq)} \\
4. \text{NaOH (aq) + NH₄Cl (aq) → NaCl (aq) + NH₄OH (aq)} \\
5. \text{KI (aq) + Pb(C₂H₃O₂)₂ (aq) → PbI₂ (s) + KC₂H₃O₂ (aq)} \\
6. \text{Ag(NO₃) (aq) + NH₄Cl (aq) → NH₄NO₃ (aq) + AgCl (s)} \\
7. \text{2 HCl (aq) + K₂SO₃ (aq) → H₂SO₃ (aq) + 2 KCl (aq)} \\
8. \text{2 Rb(OH) (aq) + Cu(ClO₃)₂ (aq) → Cu(OH)₂ (s) + 2 RbClO₃ (aq)} \\
9. \text{2 Fe(CN)₃ (s) + 3 Li₂(CO₃) (aq) → Fe₂(CO₃)₃ (s) + 6 LiCN (aq)} \\
10. \text{2 NaI (aq) + Pb(NO₃)₂ (aq) → PbI₂ (s) + 2 NaNO₃ (aq)}
\end{array}
}
\]