7. Determine the volume of 1.5 M KI solution required for the reaction of 10.00 grams lead(II) nitrate. Pb(NO3)2 2KI Pbl2 + 2KNO3

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### Chemistry Problems

#### 6. Dilution and Molarity
**Problem:**
What is the final molarity that would result if you diluted 180.0 mL of a 1.55 M HCl solution to a final volume of 500.0 mL?

**Solution Approach:**
Use the dilution formula: 
\[ M_1V_1 = M_2V_2 \]

Where:
- \( M_1 \) = initial molarity
- \( V_1 \) = initial volume
- \( M_2 \) = final molarity
- \( V_2 \) = final volume

#### 7. Reaction Stoichiometry
**Problem:**
Determine the volume of 1.5 M KI solution required for the reaction of 10.00 grams of lead(II) nitrate.

**Reaction:**
\[ \text{Pb(NO}_3\text{)}_2 + 2\text{KI} \rightarrow \text{PbI}_2 + 2\text{KNO}_3 \]

**Solution Approach:**
1. Calculate moles of lead(II) nitrate using its molar mass.
2. Use the stoichiometry of the balanced equation to find moles of KI needed.
3. Use molarity (\( M = \text{moles/volume} \)) to find the required volume of KI solution.

#### 8. Mass from Molarity
**Problem:**
How many grams of KNO\(_3\) are contained in 245 mL of 3.00 M KNO\(_3\) solution?

**Solution Approach:**
1. Convert volume to liters.
2. Use molarity to find moles of KNO\(_3\).
3. Calculate mass using the molar mass of KNO\(_3\).

#### 9. Percent Yield
**Problem:**
If the combustion of 4.00 grams of magnesium results in the actual yield of 5.00 grams of magnesium oxide, what is the percent yield of the reaction?

**Reaction:**
\[ 2\text{Mg(s)} + \text{O}_2\text{(g)} \rightarrow 2\text{MgO(s)} \]

**Solution Approach:**
1. Calculate the theoretical yield of MgO using stoichiometry based on starting mass of magnesium.
2. Use the formula for
Transcribed Image Text:### Chemistry Problems #### 6. Dilution and Molarity **Problem:** What is the final molarity that would result if you diluted 180.0 mL of a 1.55 M HCl solution to a final volume of 500.0 mL? **Solution Approach:** Use the dilution formula: \[ M_1V_1 = M_2V_2 \] Where: - \( M_1 \) = initial molarity - \( V_1 \) = initial volume - \( M_2 \) = final molarity - \( V_2 \) = final volume #### 7. Reaction Stoichiometry **Problem:** Determine the volume of 1.5 M KI solution required for the reaction of 10.00 grams of lead(II) nitrate. **Reaction:** \[ \text{Pb(NO}_3\text{)}_2 + 2\text{KI} \rightarrow \text{PbI}_2 + 2\text{KNO}_3 \] **Solution Approach:** 1. Calculate moles of lead(II) nitrate using its molar mass. 2. Use the stoichiometry of the balanced equation to find moles of KI needed. 3. Use molarity (\( M = \text{moles/volume} \)) to find the required volume of KI solution. #### 8. Mass from Molarity **Problem:** How many grams of KNO\(_3\) are contained in 245 mL of 3.00 M KNO\(_3\) solution? **Solution Approach:** 1. Convert volume to liters. 2. Use molarity to find moles of KNO\(_3\). 3. Calculate mass using the molar mass of KNO\(_3\). #### 9. Percent Yield **Problem:** If the combustion of 4.00 grams of magnesium results in the actual yield of 5.00 grams of magnesium oxide, what is the percent yield of the reaction? **Reaction:** \[ 2\text{Mg(s)} + \text{O}_2\text{(g)} \rightarrow 2\text{MgO(s)} \] **Solution Approach:** 1. Calculate the theoretical yield of MgO using stoichiometry based on starting mass of magnesium. 2. Use the formula for
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