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26.03.2020 •
Chemistry
A chemist titrates 100.0mL of a 0.3444M hydrocyanic acid HCN solution with 0.8414M KOH solution at 25°C . Calculate the pH at equivalence. The pKa of hydrocyanic acid is 9.21 . Round your answer to 2 decimal places.
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Ответ:
Answer : The pH at equivalence is, 11.30
Explanation : Given,
Concentration of = 0.3444 M
Volume of = 100.0 mL = 0.1 L (1 L = 1000 mL)
First we have to calculate the moles of
As we known that at equivalent point, the moles of HCN and KOH are equal.
So, Moles of KOH = Moles of HCN = 0.03444 mol
Now we have to calculate the volume of KOH.
Total volume of solution = 0.1 L + 0.0409 L = 0.1409 L
Now we have to calculate the concentration of KCN.
The balanced equilibrium reaction will be:
Moles of KCN = 0.03444 mol
At equivalent point,
Given:
Now put all the given values in the above expression, we get:
Therefore, the pH at equivalence is, 11.30
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