The percentage deprotonation of a 0.115 M solution of benzoic acid (a weak, monoprotic acid) is 2.1%. What is the pH of the solution

The pH value of the solution is  : 2.6

Given data:

percentage deprotonation = 2.1%

concentration of solution ( c )  = 0.115 M

Determine the pH of the solution

Applying dissociation constant ;  K =       ( HA ---> H⁺A⁻ )

∝ = = 0.021

[ H⁺ ] = c * ∝ = 0.115 * 0.021 = 0.0024

Given that

pH = -log [ H⁺ ]

pH = - log [ 0.0024 ]

∴ pH of the solution = 2.6

Hence we can conclude that the pH of the solution is 2.6

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 pH of the solution is 2.6

Explanation:

 cM              0             0

So dissociation constant will be:

Give c= 0.115 M and =

Also

Thus pH of the solution is 2.6

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.