Muscles produce lactic acid, CH 3 CH ( OH ) COOH ( aq ) , during exercise. Calculate the percent ionization (deprotonation), pH, and pOH of a 0.1051 M solution of lactic acid. The acid‑dissociation (or ionization) constant, K a , of this acid is 8.40 × 10 − 4 .

The degree of ionization = 8.56%; pH = 1.4264; pOH = 12.5736.

Explanation:

The balanced equilibrium reaction for the dissociation of lactic acid is given below;

CH3CH(OH)COOH ( aq ) + H2O <> CH3CH(OH)COO^-(aq) + H3O^+.

(It must be noted that CH3CH(OH)COOH is a weak and monoprotic acid).

==> The initial concentration of CH3CH(OH)COOH = 0.1051 M and the initial concentration of H3O^+ and CH3CH(OH)COO^- = 0 M respectively.

==> At equilibrium, the concentration of CH3CH(OH)COOH = 0.1051 - x M and the concentration of CH3CH(OH)COOH is x M and the concentration of H3O^+ = x M.

Hence, the formula relating the ka value and the concentration of the species in the Reaction is given below;

Ka = [H3O^+] [CH3CH(OH)COO^-] / [CH3CH(OH)COOH].

8.40 × 10^-4 = (x^2)/ 0.1051 - x.

x^2 = (8.40 × 10^-4 × 0.1051) - 8.40 × 10^-4 x.

x^2 + 8.40 × 10^-4 - 0.000088284.

Therefore, solving the quadratic equation for the equation above, the value of x= 0.0089851262617787( we are ignoring the x value that has negative sign attached to it)

x= 0.009 M

(1). The degree of ionization= [concentration of ionized molecules/ Initial concentration of the acid] × 100.

The degree of ionization = (0.009/ 0.1051) × 100.

= 8.56%.

(2). In order to calculate the value of pH we make use of Henderson-Hasselbalch Equation which is given below;

pH = pKa + log ( [ CH3CH(OH)COO^-] / [CH3CH(OH)COOH] ).

pH= 3.1 + log ( 0.009/ 0.1051).

pH= 3.1 + log 0.08563273073.

pH = 3.1 + (-1.0673602066).

pH= 3.1 - 1.6736.

pH = 1.4264.

(Recall that pKa = - log ka).

(3). pH + pOH = 14.

pOH = 14 - pH.

pOH = 12.5736.

b

explanation:

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line graphs show patterns in data with variables that change over time; whereas, circle graphs show data as parts out of a whole (such as out of 100%).