In a solution, the concentration of hydroxide ions is 8 x 10^11 M. What is the pH of the solution? To find the pH, we first need to find the pOH using the concentration of hydroxide ions (OH^): pOH = log[OH^] Substitute the given concentration into the formula: pOH = log(8 x 10^11) We can express this as: pOH = log(8)  log(10^11) Using the properties of logarithms, we get: pOH = log(8) + 11 We know that (log(8) ≈ 0.903): pOH = 0.903 + 11 Therefore, the pOH is: pOH ≈ 10.097 To find the pH, we use the relationship between pH and pOH: pH + pOH = 14 Substitute the value of pOH into this equation: pH + 10.097 = 14 Solving for pH: pH = 14  10.097 pH ≈ 3.903 Therefore, the correct option is: C. 3.9
Question
In a solution, the concentration of hydroxide ions is $$ 8 \times 10^{11} \mathrm{M} $$. What is the pH of the solution?
To find the pH, we first need to find the pOH using the concentration of hydroxide ions (( \mathrm{OH}^ )):
$$ \text{pOH} = \log[ \mathrm{OH}^] $$
Substitute the given concentration into the formula:
$$ \text{pOH} = \log(8 \times 10^{11}) $$
We can express this as:
$$ \text{pOH} = \log(8)  \log(10^{11}) $$
Using the properties of logarithms, we get:
$$ \text{pOH} = \log(8) + 11 $$
We know that ( \log(8) \approx 0.903 ):
$$ \text{pOH} = 0.903 + 11 $$
Therefore, the pOH is:
$$ \text{pOH} \approx 10.097 $$
To find the pH, we use the relationship between pH and pOH:
$$ \text{pH} + \text{pOH} = 14 $$
Substitute the value of pOH into this equation:
$$ \text{pH} + 10.097 = 14 $$
Solving for pH:
$$ \text{pH} = 14  10.097 $$
$$ \text{pH} \approx 3.903 $$
Therefore, the correct option is:
C. 3.9
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Answer
To determine the $\text{pH}$ of an alcohol solution with a hydroxide ion concentration of $8 \times 10^{11} , \text{M}$, follow these steps:

Find the pOH using the formula: $$ \text{pOH} = \log [\text{OH}^] $$
Given that $[\text{OH}^] = 8 \times 10^{11} , \text{M}$, $$ \text{pOH} = \log (8 \times 10^{11}) $$ Approximating, we get: $$ \text{pOH} \approx 10.1 $$

Convert pOH to pH: Using the relation $\text{pH} + \text{pOH} = 14$, $$ \text{pH} = 14  \text{pOH} $$
Substituting the computed pOH value, $$ \text{pH} = 14  10.1 = 3.9 $$
Hence, the $\text{pH}$ of the alcohol solution is $\textbf{3.9}$. Thus, the correct option is:
C. 3.9
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