Question

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,

Answer 1

Option (B) is the right answer.

Hydronium ion ($H_{3}O^{+}$) concentration decreases by the factor of 100, if the pH of a solution increases from 2.0 to 4.0.

What is pH?

The hydrogen ion concentration in water is expressed by pH. Specific to aqueous solutions, pH is the negative logarithm of the hydrogen ion (H+) concentration (mol/L) : $pH = -log_{10}[H_{3}O^{+} ]$

Acidic solutions are those with a pH under 7, and basic solutions are those with a pH over 7. At this temperature, solutions with a pH of 7 are neutral (e.g. pure water). The pH neutrality relies on temperature, falling below 7 if the temperature rises above 25 °C.

Given:

pH1( initial pH) = 2.0

pH2( initial pH) = 4.0

[H3O+] =  initial hydronium concentration

[H3O+]* = final hydronium concentration

Formula used :

$pH = -log_{10}[H_{3}O^{+}]$

Solution:

$pH = - log_{10}[H_{3}O^{+}] \\\\= > 10^{-pH} = [H_{3}O^{+}] \\\\similarly, \\\\10^{-pH} = [H_{3}O^{+}]*\\\\ = > 10^{-4} = [H_{3}O^{+}]*\\\\Now, \frac{[H_{3}O^{+}]*}{[H_{3}O^{+}]} = 10^{-2}$

Thus , the concentration of hydronium ion decreases by 100.

To learn more about pH :

brainly.com/question/15289741

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