A monoprotic weak acid when dissolved in water is 0.66% dissociated and produces a solution with a pH of 3.04. Calculate the Ka
1 answer:
Answer:
Ka = 6.02x10⁻⁶
Explanation:
The equilibrium that takes place is:
- HA ⇄ H⁺ + A⁻
- Ka = [H⁺][A⁻]/[HA]
We <u>calculate [H⁺] from the pH</u>:
- pH = -log[H⁺]
- [H⁺] =
- [H⁺] = 9.12x10⁻⁴ M
Keep in mind that [H⁺]=[A⁻].
As for [HA], we know the acid is 0.66% dissociated, in other words:
- [HA] * 0.66/100 = [H⁺]
We <u>calculate [HA]</u>:
- [HA] = 0.138 M
Finally we <u>calculate the Ka</u>:
- Ka =
= 6.02x10⁻⁶
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=
= 9 L =
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),
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or, W =
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W =
=
= 1823.85 Nm
or, = 1823.85 J
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= Q - W
= 800 J - 1823.85 J
= -1023.85 J
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