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Answer :
To find the pOH of a solution, we can use the concentration of hydroxide ions [tex]\([OH^-]\)[/tex]. The formula to calculate pOH from the hydroxide ion concentration is:
[tex]\[ \text{pOH} = -\log_{10} \left[ \text{OH}^- \right] \][/tex]
Given that the concentration of hydroxide ions in the solution is [tex]\([OH^-] = 2.0 \times 10^{-2}\)[/tex], we can substitute this value into the formula:
1. Substitute the [tex]\([OH^-]\)[/tex] value into the formula:
[tex]\[ \text{pOH} = -\log_{10} (2.0 \times 10^{-2}) \][/tex]
2. Calculate the logarithm:
[tex]\[ \log_{10} (2.0 \times 10^{-2}) \approx -1.69897 \][/tex]
3. Apply the negative sign:
[tex]\[ \text{pOH} = -(-1.69897) = 1.69897 \][/tex]
After rounding the result to two decimal places, we find that the pOH is approximately 1.70.
So, the correct answer is option C: 1.70.
[tex]\[ \text{pOH} = -\log_{10} \left[ \text{OH}^- \right] \][/tex]
Given that the concentration of hydroxide ions in the solution is [tex]\([OH^-] = 2.0 \times 10^{-2}\)[/tex], we can substitute this value into the formula:
1. Substitute the [tex]\([OH^-]\)[/tex] value into the formula:
[tex]\[ \text{pOH} = -\log_{10} (2.0 \times 10^{-2}) \][/tex]
2. Calculate the logarithm:
[tex]\[ \log_{10} (2.0 \times 10^{-2}) \approx -1.69897 \][/tex]
3. Apply the negative sign:
[tex]\[ \text{pOH} = -(-1.69897) = 1.69897 \][/tex]
After rounding the result to two decimal places, we find that the pOH is approximately 1.70.
So, the correct answer is option C: 1.70.
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