The pH of 10M HCl aqueous solution is

Options

A. less than 0
B. zero
C. 2
D. 1

Explanation

To find the pH of a 10 M HCl aqueous solution, we can follow these steps:

### Step 1: Understand the nature of HCl
HCl is a strong acid, which means it completely dissociates in water. Therefore, the concentration of hydrogen ions \([H^+]\) in the solution will be equal to the concentration of HCl.

### Step 2: Determine the concentration of hydrogen ions
Given that the concentration of HCl is 10 M, we can conclude:
\[ [H^+] = 10 \, \text{M} \]

### Step 3: Use the pH formula
The pH of a solution is calculated using the formula:
\[ \text{pH} = -\log_{10} [H^+] \]
Substituting the concentration of hydrogen ions into the formula:
\[ \text{pH} = -\log_{10} (10) \]

### Step 4: Calculate the logarithm
The logarithm of 10 to the base 10 is 1:
\[ \text{pH} = -1 \]

### Step 5: Interpret the result
While we calculated a pH of -1, it is important to note that pH values are typically considered within the range of 0 to 14. In very concentrated solutions, the behavior of acids can deviate from ideal conditions. Therefore, while the theoretical pH is -1, the actual pH may be higher due to activity coefficients and incomplete dissociation at high concentrations.

### Final Answer
The pH of a 10 M HCl aqueous solution is approximately -1, but practically it may be higher due to non-ideal behavior.

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