A solution of acetic acid that has a concentration of 0.10 moles per liter has a pH of 2.87. What is the likely pH of a 0.10 mole per liter solution of the conjugate base sodium acetate? A. 8.97
B. 1.00
C. 2.87
D. 4.74
E. 13.00

The correct option is A) 8.97

Explanation:

To calculate the of a reaction, we use the equation:

where,

= acid dissociation constant of acetic acid =

= base dissociation constant

Putting values in above equation, we get:

To calculate the hydroxide ion concentration of conjugate base, we use the equation:

where,

[Conjugate base] = 0.10 M

Putting values in above equation, we get:

To calculate the pOH of the solution, we use the equation:

To calculate the pH of the solution, we use the equation:

pH + pOH = 14

pH + 5.03 = 14

pH = (14 - 5.03) = 8.97

Hence, the correct option is A) 8.97

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.