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What is the pH of a solution with a concentration of 4.2 x 10−5 M H3O+? (4 points)

Select one:
a. 2.31
b. 4.38
c. 5.62
d. 6.87

What is the pH of a solution with a 4.60 x 10−4 M hydroxide ion concentration? (4 points)

Select one:
a. 0.663
b. 3.33
c. 10.1
d. 10.7

Respuesta :

maacastrobr

Answer:

1) b. 4.38

2)  d. 10.7

Explanation:

1) The problem tells us that [H₃O⁺] = 4.2x10⁻⁵ M, and keeping in mind that [H₃O⁺]= [H⁺], we can calculate the pH of the solution:

  • pH = -log[H⁺] = 4.38

2) First we calculate the pOH of the solution:

  • pOH = -log[OH⁻] = -log(4.6x10⁻⁴) = 3.33

Then we calculate the pH using the following formula:

  • pH = 14 - pOH = 14 - 3.33
  • pH = 10.7

The pH of a solution with a concentration of 4.2x10⁻⁵ M H₃O⁺ ion is 4.38 and of a solution with a concentration of 4.6x10⁻⁴ OH⁻ ion is 10.7.

What is pH and pOH?

pH of any solution is define as the negative log of the concentration of H⁺ ions and pOH is define as the negative log of the concentration of OH⁻ ions.

Given that concentration of H⁺ ions in solution = 4.2x10⁻⁵ M

pH for this solution is calculated as:
pH = -log(4.2x10⁻⁵) = 4.38

Also given that concentration of OH⁻ ions in solution = 4.6x10⁻⁴

pOH = -log(4.6x10⁻⁴) = 3.33

We know that, pH + pOH = 14.

pH = 14 - 3.33 = 10.7

Hence, value of pH & pOH is 4.38 and 10.7 respectively.

To know more about pH & pOH, visit the below link:
https://brainly.com/question/24595796

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