Explain why each of following aqueous mixtures could or could not produce a buffer. In each case where the solution is a buffer, name the common ion and calculate the pH. (Use the Ka and Kb values)
a) 100 mL solution containing 0.20 M NH4Cl and 0.20 M NH3
b) 100 mL solution containing 0.20 M KOH and H2O
c) 100 mL solution containing 0.10 M H2SO3 and 0.15 M NaHSO
Answer :-
To be a buffer solution, it should have weak acid or base and its sal with strong base or acid. So a and c will give buffer solution while b will not give the buffer.
The answer is given in the image,
Explain why each of following aqueous mixtures could or could not produce a buffer. In each...
Calculate the pH of the solution that results from each of the following mixtures. A) 55.0 mL of 0.15 molL−1 HCOOH (Ka=1.8×10−4) with 80.0 mL of 0.13 molL−1 HCOONa. B) 135.0 mL of 0.13 molL−1 NH3 (Kb=1.76×10−5) with 240.0 mL of 0.13 molL−1 NH4Cl
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