What volume of 0.6 M HCl has enough hydrochloric acid to react exactly with 25 mL of aqueous NaOH having concentration of 0.5 M ?

Explanation

To solve the problem, we need to determine the volume of 0.6 M HCl required to react with 25 mL of 0.5 M NaOH. Here’s a step-by-step solution:

### Step 1: Write the balanced chemical equation
The reaction between NaOH and HCl can be represented as:
\[ \text{NaOH (aq)} + \text{HCl (aq)} \rightarrow \text{NaCl (aq)} + \text{H}_2\text{O (l)} \]

### Step 2: Calculate the moles of NaOH
We know the concentration (molarity) and volume of NaOH:
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