What is the pH value of `1 M H_(2)SO_(4)`

Options

A. 0
B. `-0.213`
C. `-2`
D. `-0.3010`

Explanation

To find the pH value of a 1 M solution of sulfuric acid (H₂SO₄), we can follow these steps:

### Step 1: Understand the nature of H₂SO₄
H₂SO₄ is a strong acid, which means it completely dissociates in water.

### Step 2: Write the dissociation reaction
The dissociation of sulfuric acid in water can be represented as follows:
\[ \text{H}_2\text{SO}_4 \rightarrow 2 \text{H}^+ + \text{SO}_4^{2-} \]

### Step 3: Determine the concentration of H⁺ ions
Since 1 mole of H₂SO₄ produces 2 moles of H⁺ ions upon complete dissociation, the concentration of H⁺ ions in a 1 M solution of H₂SO₄ will be:
\[ [\text{H}^+] = 2 \times 1 \, \text{M} = 2 \, \text{M} \]

### Step 4: Calculate the pH
The pH is calculated using the formula:
\[ \text{pH} = -\log[\text{H}^+] \]
Substituting the concentration of H⁺ ions:
\[ \text{pH} = -\log(2) \]

### Step 5: Calculate the logarithm
Using a calculator or logarithm table, we find:
\[ -\log(2) \approx -0.3010 \]

### Step 6: Final pH value
Thus, the pH of a 1 M solution of H₂SO₄ is:
\[ \text{pH} \approx -0.3010 \]

### Summary
The pH value of 1 M H₂SO₄ is approximately -0.3010.

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