Chemistry

Question

The hydronium ion concentration of lemon juice is 5 x 10^ –3.

A sample of lemon juice will have [OH–] value of ___i___ mol/L and pH value of ___ii___. The statement given above is completed by the information in row:

Row i ii
A 5 x 10^–12 4.2
B. 3 x 10^–12 3.1
C. 2 x 10^–12 2.3
D. 2 x 10^–11 1.2
E. 4 x 10^–12 2.7

a) A
b) B
c) C
d) D
e) E

Answer 1

The concentration of hydroxide ions ([OH-]) can be calculated using the formula Kw = [H3O+][OH-], where Kw is the ion product of water (1 x 10^-14 mol^2/L^2). Rearranging the equation, [OH-] = Kw / [H3O+].

Given that the hydronium ion concentration of lemon juice (H3O+) is 5 x 10^-3 mol/L, we can calculate the value of [OH-]:

[OH-] = (1 x 10^-14 mol^2/L^2) / (5 x 10^-3 mol/L)
[OH-] = 2 x 10^-12 mol/L

Therefore, the value of [OH-] is 2 x 10^-12 mol/L.

To calculate the pH value, we can use the formula pH = -log[H3O+]. Substituting the given value of hydronium ion concentration, we get:

pH = -log(5 x 10^-3)
pH = 2.3

Therefore, the pH value of the lemon juice sample is 2.3.

From the information provided, we can conclude that the completed statement is given by option C: C. 2 x 10^–12 (i) and 2.3 (ii).

Answer 2

are you sure?

Answer 3

Apologies for the mistake in my previous response. Let me recalculate and provide you with the correct answer.

Given that the hydronium ion concentration of lemon juice (H3O+) is 5 x 10^-3 mol/L, we can calculate the value of [OH-]:

[OH-] = (1 x 10^-14 mol^2/L^2) / (5 x 10^-3 mol/L)
[OH-] = 2 x 10^-12 mol/L

Therefore, the value of [OH-] is 2 x 10^-12 mol/L.

To calculate the pH value, we can use the formula pH = -log[H3O+]. Substituting the given value of hydronium ion concentration, we get:

pH = -log(5 x 10^-3)
pH ≈ 2.3

Therefore, the pH value of the lemon juice sample is approximately 2.3.

Upon reconsideration, the correct completed statement is given by option C: C. 2 x 10^–12 (i) and 2.3 (ii).