Solved Chemistry 110 Worksheet Reactions in Aqueous | Chegg.com - Free Printable

Problem Overview:

The task involves balancing chemical equations for reactions in aqueous solutions and identifying which products (if any) form a precipitate. To solve this, we will:
1. Balance each chemical equation.
2. Use solubility rules to determine if any of the products are insoluble in water (i.e., form a precipitate).
3. Indicate precipitates by placing an "(s)" after their formulas.

Solubility Rules (Summary):

- Soluble Compounds:
- All common sodium, potassium, and ammonium salts.
- Nitrates, acetates, and chlorates.
- Most chlorides, bromides, and iodides (except those of Ag⁺, Pb²⁺, and Hg₂²⁺).
- Most sulfates (except those of Ba²⁺, Sr²⁺, Ca²⁺, Pb²⁺, and Hg₂²⁺).
- Insoluble Compounds:
- Most hydroxides (except those of Group 1 metals and Ba²⁺, Sr²⁺, and Ca²⁺).
- Most carbonates, phosphates, and sulfides.
- Chlorides, bromides, and iodides of Ag⁺, Pb²⁺, and Hg₂²⁺.
- Sulfates of Ba²⁺, Sr²⁺, Ca²⁺, Pb²⁺, and Hg₂²⁺.

Solution:

#### 1. \( \text{NaBr} (aq) + \text{AgNO}_3 (aq) \rightarrow \)
- Reaction: Double displacement.
- Products: \( \text{AgBr} \) and \( \text{NaNO}_3 \).
- Balanced Equation:
\[
\text{NaBr} (aq) + \text{AgNO}_3 (aq) \rightarrow \text{AgBr} (s) + \text{NaNO}_3 (aq)
\]
- Precipitate: \( \text{AgBr} \) is insoluble (silver halides are generally insoluble).
- Final Answer:
\[
\boxed{\text{NaBr} (aq) + \text{AgNO}_3 (aq) \rightarrow \text{AgBr} (s) + \text{NaNO}_3 (aq)}
\]

#### 2. \( \text{K}_2\text{S} (aq) + \text{ZnBr}_2 (aq) \rightarrow \)
- Reaction: Double displacement.
- Products: \( \text{ZnS} \) and \( \text{KBr} \).
- Balanced Equation:
\[
\text{K}_2\text{S} (aq) + \text{ZnBr}_2 (aq) \rightarrow \text{ZnS} (s) + 2\text{KBr} (aq)
\]
- Precipitate: \( \text{ZnS} \) is insoluble (most sulfides are insoluble).
- Final Answer:
\[
\boxed{\text{K}_2\text{S} (aq) + \text{ZnBr}_2 (aq) \rightarrow \text{ZnS} (s) + 2\text{KBr} (aq)}
\]

#### 3. \( \text{Li}_3\text{PO}_4 (aq) + \text{AlCl}_3 (aq) \rightarrow \)
- Reaction: Double displacement.
- Products: \( \text{AlPO}_4 \) and \( \text{LiCl} \).
- Balanced Equation:
\[
\text{Li}_3\text{PO}_4 (aq) + \text{AlCl}_3 (aq) \rightarrow \text{AlPO}_4 (s) + 3\text{LiCl} (aq)
\]
- Precipitate: \( \text{AlPO}_4 \) is insoluble (most phosphates are insoluble).
- Final Answer:
\[
\boxed{\text{Li}_3\text{PO}_4 (aq) + \text{AlCl}_3 (aq) \rightarrow \text{AlPO}_4 (s) + 3\text{LiCl} (aq)}
\]

#### 4. \( \text{HI} (aq) + \text{LiOH} (aq) \rightarrow \)
- Reaction: Acid-base neutralization.
- Products: \( \text{LiI} \) and \( \text{H}_2\text{O} \).
- Balanced Equation:
\[
\text{HI} (aq) + \text{LiOH} (aq) \rightarrow \text{LiI} (aq) + \text{H}_2\text{O} (l)
\]
- Precipitate: No precipitate forms (all products are soluble).
- Final Answer:
\[
\boxed{\text{HI} (aq) + \text{LiOH} (aq) \rightarrow \text{LiI} (aq) + \text{H}_2\text{O} (l)}
\]

#### 5. \( \text{HBr} (aq) + \text{Ba(OH)}_2 (aq) \rightarrow \)
- Reaction: Acid-base neutralization.
- Products: \( \text{BaBr}_2 \) and \( \text{H}_2\text{O} \).
- Balanced Equation:
\[
2\text{HBr} (aq) + \text{Ba(OH)}_2 (aq) \rightarrow \text{BaBr}_2 (aq) + 2\text{H}_2\text{O} (l)
\]
- Precipitate: No precipitate forms (all products are soluble).
- Final Answer:
\[
\boxed{2\text{HBr} (aq) + \text{Ba(OH)}_2 (aq) \rightarrow \text{BaBr}_2 (aq) + 2\text{H}_2\text{O} (l)}
\]

#### 6. \( (\text{NH}_4)_2\text{CO}_3 (aq) + \text{MgCl}_2 (aq) \rightarrow \)
- Reaction: Double displacement.
- Products: \( \text{MgCO}_3 \) and \( \text{NH}_4\text{Cl} \).
- Balanced Equation:
\[
(\text{NH}_4)_2\text{CO}_3 (aq) + \text{MgCl}_2 (aq) \rightarrow \text{MgCO}_3 (s) + 2\text{NH}_4\text{Cl} (aq)
\]
- Precipitate: \( \text{MgCO}_3 \) is insoluble (most carbonates are insoluble).
- Final Answer:
\[
\boxed{(\text{NH}_4)_2\text{CO}_3 (aq) + \text{MgCl}_2 (aq) \rightarrow \text{MgCO}_3 (s) + 2\text{NH}_4\text{Cl} (aq)}
\]

#### 7. \( \text{CuCl}_2 (aq) + \text{KNO}_3 (aq) \rightarrow \)
- Reaction: No reaction (no precipitate, gas, or water formed).
- Balanced Equation:
\[
\text{CuCl}_2 (aq) + \text{KNO}_3 (aq) \rightarrow \text{No Reaction}
\]
- Precipitate: No precipitate forms.
- Final Answer:
\[
\boxed{\text{CuCl}_2 (aq) + \text{KNO}_3 (aq) \rightarrow \text{No Reaction}}
\]

#### 8. \( \text{MgBr}_2 (aq) + \text{Pb(NO}_3\text{)}_2 (aq) \rightarrow \)
- Reaction: Double displacement.
- Products: \( \text{PbBr}_2 \) and \( \text{Mg(NO}_3\text{)}_2 \).
- Balanced Equation:
\[
\text{MgBr}_2 (aq) + \text{Pb(NO}_3\text{)}_2 (aq) \rightarrow \text{PbBr}_2 (s) + \text{Mg(NO}_3\text{)}_2 (aq)
\]
- Precipitate: \( \text{PbBr}_2 \) is insoluble (lead(II) halides are generally insoluble).
- Final Answer:
\[
\boxed{\text{MgBr}_2 (aq) + \text{Pb(NO}_3\text{)}_2 (aq) \rightarrow \text{PbBr}_2 (s) + \text{Mg(NO}_3\text{)}_2 (aq)}
\]

#### 9. \( \text{H}_2\text{SO}_4 (aq) + \text{KOH} (aq) \rightarrow \)
- Reaction: Acid-base neutralization.
- Products: \( \text{K}_2\text{SO}_4 \) and \( \text{H}_2\text{O} \).
- Balanced Equation:
\[
\text{H}_2\text{SO}_4 (aq) + 2\text{KOH} (aq) \rightarrow \text{K}_2\text{SO}_4 (aq) + 2\text{H}_2\text{O} (l)
\]
- Precipitate: No precipitate forms (all products are soluble).
- Final Answer:
\[
\boxed{\text{H}_2\text{SO}_4 (aq) + 2\text{KOH} (aq) \rightarrow \text{K}_2\text{SO}_4 (aq) + 2\text{H}_2\text{O} (l)}
\]

#### 10. \( \text{Na}_3\text{PO}_4 (aq) + \text{MgCl}_2 (aq) \rightarrow \)
- Reaction: Double displacement.
- Products: \( \text{Mg}_3(\text{PO}_4)_2 \) and \( \text{NaCl} \).
- Balanced Equation:
\[
2\text{Na}_3\text{PO}_4 (aq) + 3\text{MgCl}_2 (aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2 (s) + 6\text{NaCl} (aq)
\]
- Precipitate: \( \text{Mg}_3(\text{PO}_4)_2 \) is insoluble (most phosphates are insoluble).
- Final Answer:
\[
\boxed{2\text{Na}_3\text{PO}_4 (aq) + 3\text{MgCl}_2 (aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2 (s) + 6\text{NaCl} (aq)}
\]

#### 11. \( \text{HCl} (aq) + \text{KOH} (aq) \rightarrow \)
- Reaction: Acid-base neutralization.
- Products: \( \text{KCl} \) and \( \text{H}_2\text{O} \).
- Balanced Equation:
\[
\text{HCl} (aq) + \text{KOH} (aq) \rightarrow \text{KCl} (aq) + \text{H}_2\text{O} (l)
\]
- Precipitate: No precipitate forms (all products are soluble).
- Final Answer:
\[
\boxed{\text{HCl} (aq) + \text{KOH} (aq) \rightarrow \text{KCl} (aq) + \text{H}_2\text{O} (l)}
\]

#### 12. \( \text{Pb(NO}_3\text{)}_2 (aq) + \text{AlCl}_3 (aq) \rightarrow \)
- Reaction: Double displacement.
- Products: \( \text{PbCl}_2 \) and \( \text{Al(NO}_3\text{)}_3 \).
- Balanced Equation:
\[
\text{Pb(NO}_3\text{)}_2 (aq) + 2\text{AlCl}_3 (aq) \rightarrow 2\text{PbCl}_2 (s) + 2\text{Al(NO}_3\text{)}_3 (aq)
\]
- Precipitate: \( \text{PbCl}_2 \) is insoluble (lead(II) halides are generally insoluble).
- Final Answer:
\[
\boxed{\text{Pb(NO}_3\text{)}_2 (aq) + 2\text{AlCl}_3 (aq) \rightarrow 2\text{PbCl}_2 (s) + 2\text{Al(NO}_3\text{)}_3 (aq)}
\]

#### 13. \( \text{H}_3\text{PO}_4 (aq) + \text{NaOH} (aq) \rightarrow \)
- Reaction: Acid-base neutralization.
- Products: \( \text{Na}_3\text{PO}_4 \) and \( \text{H}_2\text{O} \).
- Balanced Equation:
\[
\text{H}_3\text{PO}_4 (aq) + 3\text{NaOH} (aq) \rightarrow \text{Na}_3\text{PO}_4 (aq) + 3\text{H}_2\text{O} (l)
\]
- Precipitate: No precipitate forms (all products are soluble).
- Final Answer:
\[
\boxed{\text{H}_3\text{PO}_4 (aq) + 3\text{NaOH} (aq) \rightarrow \text{Na}_3\text{PO}_4 (aq) + 3\text{H}_2\text{O} (l)}
\]

Final Boxed Answers:

1. \( \boxed{\text{NaBr} (aq) + \text{AgNO}_3 (aq) \rightarrow \text{AgBr} (s) + \text{NaNO}_3 (aq)} \)
2. \( \boxed{\text{K}_2\text{S} (aq) + \text{ZnBr}_2 (aq) \rightarrow \text{ZnS} (s) + 2\text{KBr} (aq)} \)
3. \( \boxed{\text{Li}_3\text{PO}_4 (aq) + \text{AlCl}_3 (aq) \rightarrow \text{AlPO}_4 (s) + 3\text{LiCl} (aq)} \)
4. \( \boxed{\text{HI} (aq) + \text{LiOH} (aq) \rightarrow \text{LiI} (aq) + \text{H}_2\text{O} (l)} \)
5. \( \boxed{2\text{HBr} (aq) + \text{Ba(OH)}_2 (aq) \rightarrow \text{BaBr}_2 (aq) + 2\text{H}_2\text{O} (l)} \)
6. \( \boxed{(\text{NH}_4)_2\text{CO}_3 (aq) + \text{MgCl}_2 (aq) \rightarrow \text{MgCO}_3 (s) + 2\text{NH}_4\text{Cl} (aq)} \)
7. \( \boxed{\text{CuCl}_2 (aq) + \text{KNO}_3 (aq) \rightarrow \text{No Reaction}} \)
8. \( \boxed{\text{MgBr}_2 (aq) + \text{Pb(NO}_3\text{)}_2 (aq) \rightarrow \text{PbBr}_2 (s) + \text{Mg(NO}_3\text{)}_2 (aq)} \)
9. \( \boxed{\text{H}_2\text{SO}_4 (aq) + 2\text{KOH} (aq) \rightarrow \text{K}_2\text{SO}_4 (aq) + 2\text{H}_2\text{O} (l)} \)
10. \( \boxed{2\text{Na}_3\text{PO}_4 (aq) + 3\text{MgCl}_2 (aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2 (s) + 6\text{NaCl} (aq)} \)
11. \( \boxed{\text{HCl} (aq) + \text{KOH} (aq) \rightarrow \text{KCl} (aq) + \text{H}_2\text{O} (l)} \)
12. \( \boxed{\text{Pb(NO}_3\text{)}_2 (aq) + 2\text{AlCl}_3 (aq) \rightarrow 2\text{PbCl}_2 (s) + 2\text{Al(NO}_3\text{)}_3 (aq)} \)
13. \( \boxed{\text{H}_3\text{PO}_4 (aq) + 3\text{NaOH} (aq) \rightarrow \text{Na}_3\text{PO}_4 (aq) + 3\text{H}_2\text{O} (l)} \)