`Ph` of an aqueous solution of `HCl` is 5. If `1 c.c.` of this solution is dilution to 1000 times. The pH will become

Options

A. 8
B. 5
C. 6.9
D. None

Explanation

To solve the problem, we need to follow these steps:

### Step 1: Understand the initial pH of the solution
The initial pH of the HCl solution is given as 5. Recall that pH is defined as:
\[ \text{pH} = -\log[H^+] \]
From this, we can find the concentration of hydrogen ions \([H^+]\) in the solution.

### Step 2: Calculate the concentration of \([H^+]\)
Using the pH value:
\[ 5 = -\log[H^+] \]
To find \([H^+]\), we take the antilogarithm:
\[ [H^+] = 10^{-5} \, \text{M} \]

### Step 3: Determine the dilution of the solution
The problem states that 1 c.c. of this solution is diluted to 1000 times. This means that the final volume after dilution will be:
\[ \text{Final Volume} = 1 \, \text{c.c.} \times 1000 = 1000 \, \text{c.c.} \]

### Step 4: Calculate the new concentration after dilution
When a solution is diluted, the concentration of the solute decreases. The dilution factor is 1000, so the new concentration of \([H^+]\) after dilution will be:
\[ \text{New Concentration} = \frac{[H^+]}{\text{Dilution Factor}} = \frac{10^{-5}}{1000} = 10^{-5} \times 10^{-3} = 10^{-8} \, \text{M} \]

### Step 5: Calculate the new pH
Now we can find the new pH using the new concentration of hydrogen ions:
\[ \text{pH} = -\log[H^+] = -\log(10^{-8}) = 8 \]

### Final Answer
The pH of the diluted solution will be **8**.

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