The concentration of `OH^(-)` in a solution is `1.0xx10^(-10)M`. The solution is

Options

A. acidic
B. basic
C. neutral
D. None of these

Explanation

To determine whether the solution is acidic, basic, or neutral based on the concentration of hydroxide ions (OH⁻), follow these steps:

### Step 1: Given Information
We are given the concentration of OH⁻ ions in the solution, which is \(1.0 \times 10^{-10} \, M\).

### Step 2: Calculate pOH
To find the pOH of the solution, we use the formula:
\[ \text{pOH} = -\log[\text{OH}^-] \]
Substituting the given concentration:
\[ \text{pOH} = -\log(1.0 \times 10^{-10}) = 10 \]

### Step 3: Calculate pH
Using the relationship between pH and pOH, we can find the pH:
\[ \text{pH} + \text{pOH} = 14 \]
Substituting the value of pOH:
\[ \text{pH} = 14 - 10 = 4 \]

### Step 4: Determine H⁺ Concentration
Next, we need to find the concentration of hydrogen ions (H⁺) using the pH:
\[ [\text{H}^+] = 10^{-\text{pH}} = 10^{-4} \, M \]

### Step 5: Compare H⁺ and OH⁻ Concentrations
Now, we compare the concentrations of H⁺ and OH⁻:
- Concentration of H⁺: \(10^{-4} \, M\)
- Concentration of OH⁻: \(10^{-10} \, M\)

Since \(10^{-4} > 10^{-10}\), the solution has a higher concentration of H⁺ ions than OH⁻ ions.

### Step 6: Conclusion
Since the concentration of H⁺ ions is greater than that of OH⁻ ions, we conclude that the solution is **acidic**.

### Final Answer
The solution is **acidic**.

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