Calculate the pH of a 0.100M NaCH3COO solution. Ka for acetic acid, HC2H3O2 is 1.8x10-5

Calculate the pH of a 0.100M NaCH₃COO solution. Ka for acetic acid, HC₂H₃O₂ is 1.8x10^-5

Expert Solution

Let a be the dissociation of the weak acid
HA <---> H ⁺ + A^-

initial conc. c 0 0

change -ca +ca +ca

Equb. conc. c(1-a) ca ca

Dissociation constant , K_a = ca x ca / ( c(1-a)

= c a² / (1-a)

In the case of weak acids a is very small so 1-a is taken as 1

So K_a = ca²

==> a = √ ( K_a / c )

Given K_a = 1.8x10^-5

c = concentration = 0.100 M

Plug the values we get a = 0.0134

[H⁺] = ca = 0.100 x 0.0134 M

= 1.34x10^-3 M

pH = -log[H⁺]

= - log ( 1.34x10^-3)

= 2.87

Therefore the pH of the solution is 2.87

queen_honey_blossom answered 2 years ago

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