Q1)pKa of acid = -log Ka = -log 7.94x10-5 = 4.1
At equivalence
mmoles of acid = mmoles of base
48.7mL x 0.39M = V x 0.70M
Thus volume of base at equivlaence = 27.13 mL
At equivalence
HA + KOH ----------------------------> KA + H2O
48.7x0.39 27.13x0.70 0 0 initial mmoles
0 0 18.993 --- equilibrium
The concentration of KA = [KA] = mmoles/total volume = 18.993/(48.7+27.13)=0.25 0M
The solution now has only the salt of weak acid with strong base and hence is basic in aquous solution due to anionic hydrolysis.
The pH of such salt is given by
pH = 1/2[pKw +pKa + log C]
= 1/2[14+4.1 + log 0.250]
= 8.749
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