Solubility Rules Worksheet featuring solubility predictions for various compounds and chemical reactions to balance.

Problem Overview:

The task involves using solubility rules to determine whether certain compounds are soluble (aq) or insoluble (s) in water. Additionally, we need to analyze chemical reactions and label the products as either soluble (aq) or insoluble (s).

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Step 1: Solubility Rules Recap

Here are some key solubility rules for common ions:
1. All nitrates (NO₃⁻) are soluble.
2. All chlorides (Cl⁻) are soluble, except those of Ag⁺, Pb²⁺, and Hg₂²⁺.
3. All sulfates (SO₄²⁻) are soluble, except those of Ba²⁺, Sr²⁺, Ca²⁺, Pb²⁺, and Hg₂²⁺.
4. All hydroxides (OH⁻) are insoluble, except those of Group 1 metals (Li⁺, Na⁺, K⁺, etc.) and Ca²⁺, Sr²⁺, and Ba²⁺.
5. All carbonates (CO₃²⁻) are insoluble, except those of Group 1 metals (Li⁺, Na⁺, K⁺, etc.) and NH₄⁺.
6. All chromates (CrO₄²⁻) are soluble, except those of Ag⁺, Hg₂²⁺, and Pb²⁺.
7. All sulfides (S²⁻) are insoluble, except those of Group 1 metals (Li⁺, Na⁺, K⁺, etc.), NH₄⁺, and some transition metals like Zn²⁺, Cd²⁺, and Hg²⁺.

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Step 2: Predicting Solubility of Compounds

Using the solubility rules, let's predict whether each compound is soluble (aq) or insoluble (s):

| Compound | Solubility (aq/s) | Explanation |
|----------------|--------------------|---------------------------------------|
| Cu(NO₃)₂ | aq | All nitrates are soluble. |
| NaOH | aq | Hydroxides of Group 1 metals are soluble. |
| Na₂CrO₄ | aq | Chromates are generally soluble. |
| KCN | aq | Cyanides are generally soluble. |
| MgCO₃ | s | Carbonates are insoluble, except those of Group 1 metals. |
| Mg(OH)₂ | s | Hydroxides of Mg²⁺ are insoluble. |
| MgCrO₄ | aq | Chromates are generally soluble. |
| CuSO₄ | aq | Sulfates are generally soluble. |
| NH₄Cl | aq | Chlorides are generally soluble. |
| PbCrO₄ | s | Chromates of Pb²⁺ are insoluble. |
| CuCl₂ | aq | Chlorides are generally soluble. |
| Hg₂SO₄ | s | Sulfates of Hg₂²⁺ are insoluble. |
| NaCl | aq | Chlorides are generally soluble. |
| Ag₂O | s | Oxides of Ag⁺ are insoluble. |
| Sn(SO₄)₂ | aq | Sulfates are generally soluble. |
| Ba(C₂H₅O₂)₂ | aq | Salts of C₂H₅O₂⁻ (acetate) are soluble. |

---

Step 3: Analyzing Chemical Reactions

Now, let's analyze each reaction and label the products as soluble (aq) or insoluble (s):

#### Reaction 1:
$$
\text{Na}_2\text{SO}_4 + \text{BaCl}_2 \rightarrow 2\text{NaCl} + \text{BaSO}_4
$$
- NaCl: Soluble (all chlorides are soluble).
- BaSO₄: Insoluble (sulfates of Ba²⁺ are insoluble).

Label:
$$
\text{Na}_2\text{SO}_4 + \text{BaCl}_2 \rightarrow 2\text{NaCl (aq)} + \text{BaSO}_4 (\text{s})
$$

#### Reaction 2:
$$
\text{HCl} + \text{Ba(ClO}_3)_2 \rightarrow \text{HClO}_3 + \text{BaCl}_2
$$
- HClO₃: Soluble (all chlorates are soluble).
- BaCl₂: Soluble (chlorides are generally soluble).

Label:
$$
\text{HCl} + \text{Ba(ClO}_3)_2 \rightarrow \text{HClO}_3 (\text{aq}) + \text{BaCl}_2 (\text{aq})
$$

#### Reaction 3:
$$
2\text{Cr(NO}_3)_2 + 3(\text{NH}_4)_2\text{S} \rightarrow \text{Cr}_2\text{S}_3 + 6\text{NH}_4\text{NO}_3
$$
- Cr₂S₃: Insoluble (sulfides are generally insoluble).
- NH₄NO₃: Soluble (all nitrates are soluble).

Label:
$$
2\text{Cr(NO}_3)_2 + 3(\text{NH}_4)_2\text{S} \rightarrow \text{Cr}_2\text{S}_3 (\text{s}) + 6\text{NH}_4\text{NO}_3 (\text{aq})
$$

#### Reaction 4:
$$
\text{NaOH} + \text{NH}_4\text{Cl} \rightarrow \text{NaCl} + \text{NH}_4\text{OH}
$$
- NaCl: Soluble (all chlorides are soluble).
- NH₄OH: Soluble (hydroxides of NH₄⁺ are soluble).

Label:
$$
\text{NaOH} + \text{NH}_4\text{Cl} \rightarrow \text{NaCl (\text{aq})} + \text{NH}_4\text{OH (\text{aq})}
$$

#### Reaction 5:
$$
\text{KI} + \text{Pb(C}_2\text{H}_5\text{O}_2)_2 \rightarrow \text{PbI}_2 + \text{KC}_2\text{H}_5\text{O}_2
$$
- PbI₂: Insoluble (iodides of Pb²⁺ are insoluble).
- KC₂H₅O₂: Soluble (salts of C₂H₅O₂⁻ are soluble).

Label:
$$
\text{KI} + \text{Pb(C}_2\text{H}_5\text{O}_2)_2 \rightarrow \text{PbI}_2 (\text{s}) + \text{KC}_2\text{H}_5\text{O}_2 (\text{aq})
$$

#### Reaction 6:
$$
\text{Ag(NO}_3) + \text{NH}_4\text{Cl} \rightarrow \text{NH}_4\text{NO}_3 + \text{AgCl}
$$
- NH₄NO₃: Soluble (all nitrates are soluble).
- AgCl: Insoluble (chlorides of Ag⁺ are insoluble).

Label:
$$
\text{Ag(NO}_3) + \text{NH}_4\text{Cl} \rightarrow \text{NH}_4\text{NO}_3 (\text{aq}) + \text{AgCl (\text{s})}
$$

#### Reaction 7:
$$
2\text{HCl} + \text{K}_2\text{SO}_3 \rightarrow \text{H}_2\text{SO}_3 + 2\text{KCl}
$$
- H₂SO₃: Soluble (weak acids are generally soluble).
- KCl: Soluble (all chlorides are soluble).

Label:
$$
2\text{HCl} + \text{K}_2\text{SO}_3 \rightarrow \text{H}_2\text{SO}_3 (\text{aq}) + 2\text{KCl (\text{aq})}
$$

#### Reaction 8:
$$
2\text{RbOH} + \text{Cu(ClO}_3)_2 \rightarrow \text{Cu(OH)}_2 + 2\text{RbClO}_3
$$
- Cu(OH)₂: Insoluble (hydroxides of Cu²⁺ are insoluble).
- RbClO₃: Soluble (all chlorates are soluble).

Label:
$$
2\text{RbOH} + \text{Cu(ClO}_3)_2 \rightarrow \text{Cu(OH)}_2 (\text{s}) + 2\text{RbClO}_3 (\text{aq})
$$

#### Reaction 9:
$$
2\text{Fe(CN)}_3 + 3\text{Li}_2\text{CO}_3 \rightarrow \text{Fe}_2(\text{CO}_3)_3 + 6\text{LiCN}
$$
- Fe₂(CO₃)₃: Insoluble (carbonates are generally insoluble).
- LiCN: Soluble (cyanides are generally soluble).

Label:
$$
2\text{Fe(CN)}_3 + 3\text{Li}_2\text{CO}_3 \rightarrow \text{Fe}_2(\text{CO}_3)_3 (\text{s}) + 6\text{LiCN (\text{aq})}
$$

#### Reaction 10:
$$
2\text{NaI} + \text{Pb(NO}_3)_2 \rightarrow \text{PbI}_2 + 2\text{NaNO}_3
$$
- PbI₂: Insoluble (iodides of Pb²⁺ are insoluble).
- NaNO₃: Soluble (all nitrates are soluble).

Label:
$$
2\text{NaI} + \text{Pb(NO}_3)_2 \rightarrow \text{PbI}_2 (\text{s}) + 2\text{NaNO}_3 (\text{aq})
$$

---

Final Answer:

$$
\boxed{
\begin{aligned}
1. & \quad \text{Na}_2\text{SO}_4 + \text{BaCl}_2 \rightarrow 2\text{NaCl (\text{aq})} + \text{BaSO}_4 (\text{s}) \\
2. & \quad \text{HCl} + \text{Ba(ClO}_3)_2 \rightarrow \text{HClO}_3 (\text{aq}) + \text{BaCl}_2 (\text{aq}) \\
3. & \quad 2\text{Cr(NO}_3)_2 + 3(\text{NH}_4)_2\text{S} \rightarrow \text{Cr}_2\text{S}_3 (\text{s}) + 6\text{NH}_4\text{NO}_3 (\text{aq}) \\
4. & \quad \text{NaOH} + \text{NH}_4\text{Cl} \rightarrow \text{NaCl (\text{aq})} + \text{NH}_4\text{OH (\text{aq})} \\
5. & \quad \text{KI} + \text{Pb(C}_2\text{H}_5\text{O}_2)_2 \rightarrow \text{PbI}_2 (\text{s}) + \text{KC}_2\text{H}_5\text{O}_2 (\text{aq}) \\
6. & \quad \text{Ag(NO}_3) + \text{NH}_4\text{Cl} \rightarrow \text{NH}_4\text{NO}_3 (\text{aq}) + \text{AgCl (\text{s})} \\
7. & \quad 2\text{HCl} + \text{K}_2\text{SO}_3 \rightarrow \text{H}_2\text{SO}_3 (\text{aq}) + 2\text{KCl (\text{aq})} \\
8. & \quad 2\text{RbOH} + \text{Cu(ClO}_3)_2 \rightarrow \text{Cu(OH)}_2 (\text{s}) + 2\text{RbClO}_3 (\text{aq}) \\
9. & \quad 2\text{Fe(CN)}_3 + 3\text{Li}_2\text{CO}_3 \rightarrow \text{Fe}_2(\text{CO}_3)_3 (\text{s}) + 6\text{LiCN (\text{aq})} \\
10. & \quad 2\text{NaI} + \text{Pb(NO}_3)_2 \rightarrow \text{PbI}_2 (\text{s}) + 2\text{NaNO}_3 (\text{aq})
\end{aligned}
}
$$