HCOOH(aq)+H2O(l)⇌HCOO(aq)−+H3O(aq)+
Using the ICE table;
Initial: 1.15M + --- ⇌ 0M + 0M
Change:. -xM + --- ⇌ +xM + +xM
Equilibrium: (1.15-x)M + --- ⇌ xM + xM
Ka=[HCOOH][HCOO−][H3O+] =[1.15−x]x2
Since Ka is small compared with the initial concentration of the acid, you can approximate (1.15−x) with 1.15. This will give;
1.8×10−4=1.15x2
x=1.8×10−4×1.15=0.0144
since [x]=[H3O]=0.0144
pH = −log[H3O]=1.84
Therefore, the pH of the 1.15 M solution of methanoic acid is 1.84
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