Defining and Calculating pOH (HSC SSCE Chemistry): Quizzes

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Defining and Calculating pOH
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What is the formula for calculating pOH from hydroxide ion concentration?

pOH=−log⁡10[OH−]\text{pOH} = -\log_{10}[\text{OH}^-]

What is the pOH when [OH−]=1.5×10−4[\text{OH}^-] = 1.5 \times 10^{-4} mol L−1^{-1}?

3.82

What is [OH−][\text{OH}^-] when pOH = 5.8?

1.6×10−61.6 \times 10^{-6} mol L−1^{-1}

For NaOH, what is the relationship between [NaOH][\text{NaOH}] and [OH−][\text{OH}^-]?

[NaOH]=[OH−][\text{NaOH}] = [\text{OH}^-]

For Ba(OH)2_2, what is the relationship between [Ba(OH)2][\text{Ba(OH)}_2] and [OH−][\text{OH}^-]?

[Ba(OH)2]=12[OH−][\text{Ba(OH)}_2] = \frac{1}{2}[\text{OH}^-]

What is the relationship between pH and pOH at 25°C?

pH+pOH=14\text{pH} + \text{pOH} = 14

If pOH = 3.9, what is the pH at 25°C?

10.1

If HF with pH = 3 is diluted by a factor of 100, what is the final pH?

5

What is the value of KwK_w at 25°C?

1.0×10−141.0 \times 10^{-14}

What happens to pOH when a basic solution evaporates?

pOH decreases

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