Question

question 11 (5 points) what is the ph of a 0.01 m solution of hcl? a) 0.01 b) 1 c) -2 d) none of these choices

Explanation:

Step1: Determine $[H^+]$ from HCl

HCl is a strong acid, so it dissociates completely: $HCl
ightarrow H^+ + Cl^-$. Thus, $[H^+] = 0.01\ M = 1\times10^{-2}\ M$.

Step2: Calculate pH using formula

The pH formula is $pH = -\log_{10}[H^+]$. Substitute $[H^+] = 1\times10^{-2}$:
$pH = -\log_{10}(1\times10^{-2}) = -(-2) = 2$? Wait, no—wait, $0.01\ M$ is $10^{-2}\ M$, so $-\log(10^{-2}) = 2$? Wait, no, wait the options: wait, maybe I made a mistake. Wait, $0.01\ M$ HCl: $[H^+] = 0.01 = 10^{-2}\ M$. Then $pH = -\log(10^{-2}) = 2$. But the options are a) 0.01, b)1, c)-2, d) none. Wait, so the correct pH is 2, which is not in a, b, c. So the answer is d. Wait, let's recheck:

Wait, $0.01\ M$ HCl: $[H^+] = 0.01\ mol/L = 1\times10^{-2}\ M$.
$pH = -\log_{10}(1\times10^{-2}) = 2$. Since 2 is not among a (0.01), b (1), c (-2), the answer is d.

Answer:

d) none of these choices