# Question #cb24c

##### 1 Answer

#### Explanation:

Your strategy here is to use an **ICE table** to find the equilibrium concentration of the hydronium ions, *formic acid* (methanoic acid),

To get the *acid dissociation constant*,

#K_a = 10^(-pK_a)#

#K_a = 10^(-3.75) = 0.00017778 = 1.78 * 10^(-4)#

So, use an ICE table to get the equilibrium concentration of the hydronium ions

#"CHCO"_2"H"_text((aq]) + "H"_2"O"_text((l]) rightleftharpoons "CHCO"_text(2(aq])^(-) " "+" " "H"_3"O"_text((aq])^(+)#

By definition, the acid dissociation constant will be

#K_a = (["H"_3"O"^(+)] * ["CHO"_2^(-)])/(["CHO"_2"H"])#

#K_a = (x * x)/(0.05 - x) = 1.78 * 10^(-4)#

Since the initial concentration of the acid is relatively small, you cannot use the approximation

#0.05 - x ~~ 0.05#

This means that will have to solve for

#x^2 = 1.78 * 10^(-4) * (0.05 - x)#

#x^2 = 8.9 * 10^(-6) - 1.78 * 10^(-4)x#

#x^2 + 1.78 * 10^(-4)x - 8.9 * 10^(-6) = 0#

This quadratic equation will produce two solutions, one positive and one negative. Since *concentration*, the only solution that will have chemical and physical significance will be the positive one

#x = 0.0028956#

This means that the concentration of hydronium ions will be

#["H"_3"O"^(+)] = x = "0.0028956 M"#

The pH of the solution will be

#"pH" = - log( ["H"_3"O"^(+)])#

#"pH" = - log(0.0028956) = color(green)(2.54)#

**SIDE NOTE** *You can try to solve by using the approximation*

#0.05 - x ~~ 0.05#

*the pH of the solution will be similar, but the approximation error will be greater than 5%, which indicates that the approximation is not justified.*

#0.05 - 0.002983 = 0.04702#

*The error is*

#|0.04702 - 0.05|/0.05 xx 100 = 5.96%#