CHEMISTRY MIDDLE SCHOOL

What is the [H3O+] in a solution with [OH-] = 2.5 x 10-2 M?a.) 4.0 x 10-^12
b.) 4.0 x 10-^2
c.) 2.5 x 10-^2
d.) 4.0 x 10-^13

Answers

Answer 1

Answer:

Answer: The $[H_3O^+]$ in a solution is $4.0* 10^(-13)$

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

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

$pOH=-\log[OH^-]$

We are given:

$OH^-=2.5* 10^(-2)$

Putting values in above equation, we get:

$pOH=-\log[2.5* 10^(-2)]=1.60$

$pH+pOH=14$

$pH=14-1.60=12.4$

$12.4=-\log[H_3O^+]$

$[H_3O^+]=4.0* 10^(-13)$

The $[H_3O^+]$ in a solution is $4.0* 10^(-13)$

Answer 2

Answer:

Final answer:

The concentration of H3O+ in a solution with OH− concentration of 2.5 x 10-2 M is 4.0 x 10^-13 M, based on the relationship between H3O+ and OH− in acid-base chemistry.

Explanation:

The question asks for the concentration of hydronium ion ([H3O+]) in a solution with a hydroxide ion concentration ([OH−]) of 2.5 x 10-2 M. This falls under the topic of acid-base chemistry, where the product of [H3O+] and [OH−] is always equal to Kw, the ionic product of water.

In this case, the formula we use is [H3O+] = Kw / [OH–]. Assuming Kw is 1.0 x 10-14 (which is true at 25 degree Celsius), the calculation is [H3O+] = (1.0 x 10^-14) / (2.5 x 10^-2). The answer will be: 4.0 x 10^-13 M.

Therefore, the concentration of [H3O+] in the given solution is 4.0 x 10^-13 M, which matches option d.) 4.0 x 10^-13.

Learn more about Acid-Base Chemistry here:

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