The molarity of an aqueous solution of hydrochloric acid, HCl, is determined by titration with a 3.34 x 10-2 M barium hydroxide, Ba(OH)2, solution. 2HCI + Ba(OH)2 → BaCl2 + 2H2O If 32.6 mL of barium hydroxide are required to neutralize 12.5 mL of the acid, what is the molarity of the hydrochloric acid solution?

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**Determining the Molarity of Hydrochloric Acid Solution**

The molarity of an aqueous solution of hydrochloric acid (HCl) is determined by titration with a 3.34 × 10⁻² M barium hydroxide (Ba(OH)₂) solution.

The balanced chemical equation for the reaction is:
\[ 2HCl + Ba(OH)_2 \rightarrow BaCl_2 + 2H_2O \]

**Problem Statement:**
If 32.6 mL of barium hydroxide are required to neutralize 12.5 mL of the acid, what is the molarity of the hydrochloric acid solution?

**Given:**
- Volume of Ba(OH)₂ solution = 32.6 mL
- Molarity of Ba(OH)₂ solution = 3.34 × 10⁻² M
- Volume of HCl solution = 12.5 mL

**Task:**
Calculate the molarity of the hydrochloric acid (HCl) solution.

\[ \text{Molarity} = \_\_\_\_\_\_ \text{ M} \]
Transcribed Image Text:**Determining the Molarity of Hydrochloric Acid Solution** The molarity of an aqueous solution of hydrochloric acid (HCl) is determined by titration with a 3.34 × 10⁻² M barium hydroxide (Ba(OH)₂) solution. The balanced chemical equation for the reaction is: \[ 2HCl + Ba(OH)_2 \rightarrow BaCl_2 + 2H_2O \] **Problem Statement:** If 32.6 mL of barium hydroxide are required to neutralize 12.5 mL of the acid, what is the molarity of the hydrochloric acid solution? **Given:** - Volume of Ba(OH)₂ solution = 32.6 mL - Molarity of Ba(OH)₂ solution = 3.34 × 10⁻² M - Volume of HCl solution = 12.5 mL **Task:** Calculate the molarity of the hydrochloric acid (HCl) solution. \[ \text{Molarity} = \_\_\_\_\_\_ \text{ M} \]
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