Question 32
mmol HCN = concentration Volume = 0.20 M 25.0 ml = 5.0 mmol
mmol KOH = concentration Volume = 0.25 M 20.0 ml = 5.0 mmol
Consider reaction, HCN (aq) + KOH (aq) 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 Volume = 0.10 M 50.0 ml =5.0 mmol
mmol KOH = concentration Volume = 0.10 M 10.0 ml =1.0 mmol
Consider reaction, HCN (aq) + KOH (aq) 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 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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