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Question
Final the ΔpH ( initial pH - final pH ) when 100 ml of 0.01 M HCI is added in solution containing 0.1 m moles of NaHCO3 solution of negligible volume (initial pH=9,Ka1=10−7,Ka2=10−11 for H2CO3):
Final the ΔpH ( initial pH - final pH ) when 100 ml of 0.01 M HCI is added in solution containing 0.1 m moles of NaHCO3 solution of negligible volume (initial pH=9,Ka1=10−7,Ka2=10−11 for H2CO3):
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Solution
The correct option is B 6 + 2 log 3
The initial pH is the pH of the NaHCO3 solution. It is 9.
The reaction between HCl and NaHCO3 can be represented as, H++HCO−3→H2CO3.
The number of mmoles of HCl remaining unreacted is =1−0.1=0.9mmol.
The expression for the final pH of the solution is pH=−log(9×10−3)=−2 log 3+3.
The change in pH is (initial pH−final pH)=9−(−2 log 3+3)=6+2 log 3.
Option A is correct.
The initial pH is the pH of the NaHCO3 solution. It is 9.
The reaction between HCl and NaHCO3 can be represented as, H++HCO−3→H2CO3.
The number of mmoles of HCl remaining unreacted is =1−0.1=0.9mmol.
The expression for the final pH of the solution is pH=−log(9×10−3)=−2 log 3+3.
The change in pH is (initial pH−final pH)=9−(−2 log 3+3)=6+2 log 3.
Option A is correct.
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