The `pH` of a solution increased from `3` to `6`. Its `[H^(o+)]` will be

Options

A. Reduced by `1000` times
B. Increased to `1000` times
C. Doubled
D. Reduced to half

Explanation

To solve the problem of how the hydrogen ion concentration changes when the pH of a solution increases from 3 to 6, we can follow these steps:

### Step 1: Understand the relationship between pH and hydrogen ion concentration
The pH of a solution is defined as:
\[ \text{pH} = -\log[H^+] \]
where \([H^+]\) is the concentration of hydrogen ions in moles per liter.

### Step 2: Calculate the initial hydrogen ion concentration at pH 3
Given that the initial pH is 3, we can calculate the hydrogen ion concentration:
\[ \text{pH} = 3 \implies [H^+] = 10^{-3} \text{ moles per liter} \]
This means:
\[ [H^+] = 0.001 \text{ moles per liter} \]

### Step 3: Calculate the hydrogen ion concentration at pH 6
Now, when the pH increases to 6, we again use the formula:
\[ \text{pH} = 6 \implies [H^+] = 10^{-6} \text{ moles per liter} \]
This means:
\[ [H^+] = 0.000001 \text{ moles per liter} \]

### Step 4: Compare the two concentrations
Now we can compare the initial and final concentrations:
- Initial concentration at pH 3: \(0.001 \text{ moles per liter}\)
- Final concentration at pH 6: \(0.000001 \text{ moles per liter}\)

### Step 5: Calculate the change in concentration
To find out how the concentration has changed, we can divide the initial concentration by the final concentration:
\[ \text{Change factor} = \frac{0.001}{0.000001} = 1000 \]
This indicates that the hydrogen ion concentration has decreased by a factor of 1000.

### Conclusion
Thus, the hydrogen ion concentration decreased by 1000 times when the pH increased from 3 to 6.

### Final Answer
The correct option is that the hydrogen ion concentration is reduced by 1000 times.

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