A) An aqueous solution contains 0.376 M
KHCO3 and 0.224 M
H2CO3.
The pH of this solution is____
B) An aqueous solution contains 0.183 M
KHCO3 and 0.300 M
H2CO3.
The pH of this solution is ______
C) An aqueous solution contains 0.313 M
NaHCO3 and
7.12×10-2 M
H2CO3.
The pH of this solution is _________
Solution :-
Using the Henderson Hassel Balch equation we can find the pH of the buffer solution.
HCO3^- and H2CO3 makes the buffer solution.
pKa of the H2CO3 is 6.35
part a) solution containing 0.376 M KHCO3 and 0.224 M H2CO3
pH= pka + log [base]/[acid]
pH= 6.35+ log [HCO3^-]/[H2CO3]
pH= 6.35 + log [0.376]/[0.224]
pH= 6.57
part b) solution containing 0.183 M KHCO3 and 0.300 M H2CO3
pH= pka + log [base]/[acid]
pH= 6.35+ log [HCO3^-]/[H2CO3]
pH= 6.35 + log [0.183]/[0.300]
pH= 6.14
part c) solution containing 0.313 M NaHCO3 and 7.12*10^-2 M H2CO3
pH= pka + log [base]/[acid]
pH= 6.35+ log [HCO3^-]/[H2CO3]
pH= 6.35 + log [0.313]/[0.0712]
pH= 6.99
Get Answers For Free
Most questions answered within 1 hours.