An aqueous solution of barium hydroxide is standardized by titration with a 0.179 M solution of hydrochloric acid. If 28.4 mL of base are required to neutralize 24.5 mL of the acid, what is the molarity of the barium hydroxide solution? M barium hydroxide Submit Answer Retry Entire Group 9 more group attempts remaining

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**Titration Problem: Determining the Molarity of Barium Hydroxide Solution**

An aqueous solution of **barium hydroxide** is standardized by titration with a **0.179 M solution of hydrochloric acid**.

**Question:**
If **28.4 mL of base** are required to neutralize **24.5 mL of the acid**, what is the molarity of the **barium hydroxide** solution?

[Input field for molarity]

**Buttons:**
- **Submit Answer**
- **Retry Entire Group**
   
(Note: You have **9 more group attempts remaining**)

---

### Explanation:

To solve this titration problem, follow these steps:

1. **Write the balanced chemical equation** for the reaction between barium hydroxide (Ba(OH)₂) and hydrochloric acid (HCl):

   \[
   \text{Ba(OH)}_{\text{2}}(aq) + 2\text{HCl}(aq) \rightarrow \text{BaCl}_{\text{2}}(aq) + 2\text{H}_{\text{2}}\text{O}(l)
   \]

2. **Determine the moles of HCl used**:

   \[
   \text{Moles of HCl} = \text{Molarity of HCl} \times \text{Volume of HCl in liters}
   \]
   \[
   \text{Moles of HCl} = 0.179 \, \text{M} \times 0.0245 \, \text{L} = 4.3855 \times 10^{-3} \, \text{mol}
   \]

3. **Use the stoichiometry of the reaction** to find the moles of Ba(OH)₂. According to the balanced equation, 1 mole of Ba(OH)₂ reacts with 2 moles of HCl:

   \[
   \text{Moles of Ba(OH)}_{\text{2}} = \frac{\text{Moles of HCl}}{2} = \frac{4.3855 \times 10^{-3}}{2} = 2.19275 \times 10^{-3} \, \text{mol}
   \]

4. **Determine the molarity of the barium hydroxide solution**:

   \[
Transcribed Image Text:**Titration Problem: Determining the Molarity of Barium Hydroxide Solution** An aqueous solution of **barium hydroxide** is standardized by titration with a **0.179 M solution of hydrochloric acid**. **Question:** If **28.4 mL of base** are required to neutralize **24.5 mL of the acid**, what is the molarity of the **barium hydroxide** solution? [Input field for molarity] **Buttons:** - **Submit Answer** - **Retry Entire Group** (Note: You have **9 more group attempts remaining**) --- ### Explanation: To solve this titration problem, follow these steps: 1. **Write the balanced chemical equation** for the reaction between barium hydroxide (Ba(OH)₂) and hydrochloric acid (HCl): \[ \text{Ba(OH)}_{\text{2}}(aq) + 2\text{HCl}(aq) \rightarrow \text{BaCl}_{\text{2}}(aq) + 2\text{H}_{\text{2}}\text{O}(l) \] 2. **Determine the moles of HCl used**: \[ \text{Moles of HCl} = \text{Molarity of HCl} \times \text{Volume of HCl in liters} \] \[ \text{Moles of HCl} = 0.179 \, \text{M} \times 0.0245 \, \text{L} = 4.3855 \times 10^{-3} \, \text{mol} \] 3. **Use the stoichiometry of the reaction** to find the moles of Ba(OH)₂. According to the balanced equation, 1 mole of Ba(OH)₂ reacts with 2 moles of HCl: \[ \text{Moles of Ba(OH)}_{\text{2}} = \frac{\text{Moles of HCl}}{2} = \frac{4.3855 \times 10^{-3}}{2} = 2.19275 \times 10^{-3} \, \text{mol} \] 4. **Determine the molarity of the barium hydroxide solution**: \[
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