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A solution has a hydronium concentration of [tex]\(4.7 \times 10^{-11}\)[/tex]. What is the [tex]\(pH\)[/tex] of the solution?

The [tex]\(pH\)[/tex] of the solution is [tex]\(\boxed{\quad}\)[/tex]

Sagot :

GinnyAnswer
To find the pH of a solution given its hydronium ion concentration, we use the formula:

[tex]\[ \text{pH} = -\log_{10} [\text{H}_3\text{O}^+] \][/tex]

Here, the hydronium ion concentration [tex]\([\text{H}_3\text{O}^+]\)[/tex] is [tex]\(4.7 \times 10^{-11}\)[/tex].

Now, let's calculate the pH:

1. First, take the common logarithm (base 10) of the hydronium ion concentration:

[tex]\[ \log_{10} (4.7 \times 10^{-11}) \approx -10.327902142064282 \][/tex]

2. Then, multiply this value by -1 to find the pH:

[tex]\[ \text{pH} = -(-10.327902142064282) = 10.327902142064282 \][/tex]

3. Lastly, round this value to the nearest hundredth:

[tex]\[ \text{pH} \approx 10.33 \][/tex]

Therefore, the pH of the solution is approximately:

[tex]\[ \boxed{10.33} \][/tex]
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