The pH for the mixture of 0.01 M HCI and 0.01 M NaOH will be

Options

A. 7
B. 0
C. 14
D. 1

Answer

To determine the pH of a mixture of 0.01 M HCl and 0.01 M NaOH, we can follow these steps:

### Step 1: Identify the substances involved
We have hydrochloric acid (HCl), which is a strong acid, and sodium hydroxide (NaOH), which is a strong base. Both are completely dissociated in solution.

### Step 2: Calculate the moles of HCl and NaOH
Assuming we have 1 liter of each solution:
- Moles of HCl = Molarity × Volume = 0.01 M × 1 L = 0.01 moles
- Moles of NaOH = Molarity × Volume = 0.01 M × 1 L = 0.01 moles

### Step 3: Determine the reaction between HCl and NaOH
The reaction between HCl and NaOH can be represented as:
\[ \text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} \]

### Step 4: Analyze the stoichiometry of the reaction
Since both HCl and NaOH are present in equal amounts (0.01 moles each), they will completely neutralize each other. There are no excess reactants left after the reaction.

### Step 5: Determine the resulting solution
The products of the neutralization reaction are sodium chloride (NaCl) and water (H2O). The resulting solution will be neutral because it contains only the salt and water.

### Step 6: Conclude the pH of the solution
For a neutral solution at 25°C, the pH is 7. Therefore, the pH of the mixture of 0.01 M HCl and 0.01 M NaOH will be:
\[ \text{pH} = 7 \]

### Final Answer
The pH for the mixture of 0.01 M HCl and 0.01 M NaOH is 7.

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