1. Titration of 331 mL of 0.501 M carbonic acid (H 2 CO 3 ) (K a1 = 4.3 x 10 -7

Question

1. Titration of 331 mL of 0.501 M carbonic acid (H2CO3) (Ka1= 4.3 x 10-7, Ka2= 5.6 x 10-11) with 1.5 M KOH.

b) What will the pH of the solution be when 0.1913 L of 1.5 M KOH are added to the 331 mL of 0.501 M carbonic acid?

((I have the answers to this one but I have no idea how to do the questions))

2. Titration of 521 mL of 0.501 M carbonic acid (H2CO3) (Ka1= 4.3 x 10-7, Ka2= 5.6 x 10-11) with 1.9 M KOH.

b) What will the pH of the solution be when 0.2432 L of 1.9 M KOH are added to the 521 mL of 0.501 M carbonic acid?

Explanation / Answer

1)b) A buffer solution will be formed.so,

pH=pKa+log(salt/acid)

also,

pKa=pKa2

=10.25

so,

pH=10.25+log((80.746*1.5/(331*0.501-80.746*1.5))

=10.68

2b)a similar problem like the one solved above.so,

pH=pKa+log(salt/acid)

also,

pKa=pKa2

=10.25

so,

pH=10.25+log((105.82*1.9/(521*0.501-105.82*1.9))

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