Enter your answer in the provided box. Sodium stearate (C17H35COONa) is a major component of bar soap. The Ka of the stearic acid is 1.3 × 10−5. What is the pH of 10.0 mL of a solution containing 3.96 g of sodium stearate?

11.61 is the pH of 10.0 mL of a solution containing 3.96 g of sodium stearate.

Explanation:

Concentration of sodium stearate acid : c

Moles of sodium stearate =

Volume of the solution = 10.0 mL = 0.010 L

initially c

c           0    0

At equilibrium

(c-x)       x    x

Dissociation constant of an acid =

Expression of a dissociation constant of an acid is given by:  

Solving for x;

x = 0.0041 M

The pOH of the solution:

pH = 14 -pOH

pH = 14 - 2.39 = 11.61

11.61 is the pH of 10.0 mL of a solution containing 3.96 g of sodium stearate.

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer