11. If the pH of a solution increases from 2.0 to 4.0, the H3O^+ ion

concentration

O

a decreases by a factor of 2.

b. decreases by a factor of 100.

c. increases by a factor of 3.

O

d. increases by a factor of 1000,

On increasing the pH of the solution from 2 to 4, the Hydronium ion concentration has been decreased by a factor of 100. Thus, option B is correct.

The log of hydronium ion concentration has been calculated as the pH.

pH = -log [Hydronium ion concentration]

Hydronium ion concentration at pH 2:

2 = -log []

[] = antilog (-2)

[] = 1 M

Hydronium ion concentration at pH 4:

4= -log []

[] = antilog (-4)

[] = 1 M

The relationship in the hydronium ion at pH 2 and pH 4:

pH 2 = 100 pH 4.

Thus on increasing the pH of the solution from 2 to 4, the Hydronium ion concentration has been decreased by a factor of 100. Thus, option B is correct.

For more information about the hydronium ion concentration, refer to the link:

link

Option B. decreases by a factor of 100

Explanation:

To obtain the right answer to the question, let us calculate the concentration of the hydronium ion, [H3O+] in both cases.

For pH = 2,

pH = – Log [H3O+]

2 = – Log [H3O+]

–2 = Log [H3O+]

[H3O+] = antilog (–2)

[H3O+] = 1x10^–2M

For pH = 4,

pH = – Log [H3O+]

4 = – Log [H3O+]

–4 = Log [H3O+]

[H3O+] = antilog (–4)

[H3O+] = 1x10^–4M

Now, we shall determine the ratio of [H3O+] in pH 4 to that of pH 2. This is illustrated below:

[H3O+] in pH 4 : [H3O+] in pH 2 => 1x10^–4 / 1x10^–2 = 0.01 = 1x10^–2

From the above, we can thus say that:

[H3O+] in pH 4 = 1/100 [H3O+] in pH 2

Therefore, the [H3O+] decrease by 100

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

the answer would be c