The `OH^-` concentration of a solution is 1.0 `xx 10^(-10)` M. The solution is

Options

A. acidic
B. basic
C. neutral
D. amphoteric

Answer

To determine the nature of the solution with an `OH^-` concentration of 1.0 x 10^(-10) M, we will follow these steps:

### Step 1: Calculate pOH
To find the pOH of the solution, we can use the formula:
\[ \text{pOH} = -\log[\text{OH}^-] \]

Given that the concentration of `OH^-` is 1.0 x 10^(-10) M, we can substitute this value into the formula:
\[ \text{pOH} = -\log(1.0 \times 10^{-10}) \]

### Step 2: Solve for pOH
Using the logarithmic property:
\[ \log(1.0 \times 10^{-10}) = -10 \]
Thus,
\[ \text{pOH} = -(-10) = 10 \]

### Step 3: Calculate pH
Next, we can use the relationship between pH and pOH at 25°C, which is given by the equation:
\[ \text{pH} + \text{pOH} = 14 \]

We already calculated pOH to be 10, so we can find pH:
\[ \text{pH} = 14 - \text{pOH} \]
\[ \text{pH} = 14 - 10 = 4 \]

### Step 4: Determine the nature of the solution
Now that we have the pH value, we can determine the nature of the solution:
- If pH < 7, the solution is acidic.
- If pH = 7, the solution is neutral.
- If pH > 7, the solution is basic.

Since we found that pH = 4, which is less than 7, we conclude that the solution is acidic.

### Final Answer
The solution is acidic.

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