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32. What substances are present in an aquesous solution that results from mixing 25.0 ml of 0.20 M HCN with 20.0 mL of 0.25 M

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Question 32

mmol HCN = concentration \times Volume = 0.20 M \times 25.0 ml = 5.0 mmol

mmol KOH = concentration \times Volume = 0.25 M \times 20.0 ml = 5.0 mmol

Consider reaction, HCN (aq) + KOH (aq) \rightarrow KCN (aq) + H2O (l)

According to reaction, 1 mol HCN reacts with 1 mol KOH and produces 1 mol KCN and 1 mol H2O.

Therefore, 5.0 mmol HCN will react with 5.0 mmol KOH and produce 5.0 mmol KCN and 5.0 mmol  H2O.

In this case, all HCN is consumed by added KOH.

After completion of reaction, solution contain only KCN and Water.

ANSWER : D) KCN and water.

Question 33

mmol HCN = concentration \times Volume = 0.10 M \times 50.0 ml =5.0 mmol

mmol KOH = concentration \times Volume = 0.10 M \times 10.0 ml =1.0 mmol

Consider reaction, HCN (aq) + KOH (aq) \rightarrow KCN (aq) + H2O (l)

According to reaction, 1 mol HCN reacts with 1 mol KOH and produces 1 mol KCN and 1 mol H2O.

From above calculations, it is clear that HCN is excess reactant and KOH is limiting reactant.

Excess mmol HCN = 5.0 mmol - 1.0 mmol = 4.0 mmol

mmol KCN produced = mmol of KOH added = 1.0 mmol

Volume of solution after addition of KOH = 50.0 + 10.0 = 60.0 ml

Let's calculate [ HCN ] and [ KCN ]

[ HCN ] = 4.0 mmol / 60.0 ml = 0.0667 M

[ KCN ] = 1.0 mmol / 60.0 ml = 0.0167 M

After reaction solution contain weak acid HCN and its salt KCN . This solution acts as a buffer solution.

We can calculate pH of buffer solution by using Henderson's equation, pH = pKa + log [ Salt ]/ [ Acid ]

pH = - log Ka + log [ KCN ] / [ HCN ]

pH = - log ( 4.9 \times 10 -10 ) + log 0.0167 / 0.0667

pH = 9.31 + log 0.0167 / 0.0667

pH = 9.31 - 0.601

pH = 8.71

ANSWER : B) 8.71

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