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.

a is the answer

explanation:

which statement about trans-fatty acids is false?

a. the conversion of cis-fatty acids to trans-fatty acids is inhibited by the presence of antioxidants.

hope this

r just means there's a number of carbon in teh chain. for example rcooh means that after x number of carbon, the chain ends with cooh.

explanation: