How many times more acidic is solution A with a pH of 2.2 than solution B with a pH of 9.2 ?

Question

UpStudy AI · Accepted Answer

Let the concentration of hydrogen ions be represented by $$[H^+]$$. The pH of a solution is defined as

$$
\text{pH} = -\log [H^+]
$$

For solution A with $$\text{pH} = 2.2$$:

$$
[H^+]_A = 10^{-2.2}
$$

For solution B with $$\text{pH} = 9.2$$:

$$
[H^+]_B = 10^{-9.2}
$$

To find how many times more acidic solution A is than solution B, we compute the ratio of their hydrogen ion concentrations:

$$
\frac{[H^+]_A}{[H^+]_B} = \frac{10^{-2.2}}{10^{-9.2}} = 10^{-2.2 - (-9.2)} = 10^{7.0}
$$

Therefore, solution A is

$$
10^7
$$

times more acidic than solution B.
Solution A is $$10^7$$ times more acidic than solution B.

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