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At 25ºC, the pH of 0.0050 M Ba(OH)₂, is A - VCE - SSCE Chemistry - Question 3 - 2003 - Paper 1

Question 3

At 25ºC, the pH of 0.0050 M Ba(OH)₂, is A. 2.0 B. 2.3 C. 11.7 D. 12.0

Worked Solution & Example Answer:At 25ºC, the pH of 0.0050 M Ba(OH)₂, is A - VCE - SSCE Chemistry - Question 3 - 2003 - Paper 1

Step 1

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Answer

Barium hydroxide, Ba(OH)₂, dissociates in water to release two hydroxide ions (OH⁻) for each formula unit:

$\text{Ba(OH)}_2 \rightarrow \text{Ba}^{2+} + 2\text{OH}^-$

For a 0.0050 M solution of Ba(OH)₂, the concentration of OH⁻ ions is:

$\text{[OH}^-\text{]} = 2 \times 0.0050 \, \text{M} = 0.0100 \, \text{M}$

Step 2

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Answer

To find the pOH, we use the formula:

$\text{pOH} = -\log{\text{[OH}^-\text{]}}$

Substituting in the concentration we found:

$\text{pOH} = -\log{(0.0100)} \approx 2.0$

Step 3

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Answer

The relationship between pH and pOH at 25ºC is given by the equation:

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

Thus, we can find the pH:

$\text{pH} = 14 - \text{pOH} = 14 - 2.0 = 12.0$

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