Question

A solution contains 1 LaTeX: \times\:×10−4 M OH– ions. Calculate the solution pH value, and determine if the solution is acidic, basic, or neutral. Helpful math formulas: LaTeX: pH=-\log\left[H_3O^+\right]p H = − log ⁡ [ H 3 O + ] LaTeX: pOH=-\log\left[OH^-\right]p O H = − log ⁡ [ O H − ] LaTeX: pH+pOH=14.00p H + p O H = 14.00 LaTeX: \left[H_3O^+\right]\left[OH^-\right]=1.0\times10^{-14}

Answer 1

Answer: The pH value of the solution is 10 and the solution is basic in nature.

Explanation:

To calculate the pH of the solution, we need to determine pOH of the solution. To calculate pOH of the solution, we use the equation:

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

We are given:

$[OH^-]=1\times 10^{-4}M$

Putting values in above equation, we get:

$pOH=-\log(1\times 10^{-4})\\\\pOH=4$

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

$pH+pOH=14\\pH=14-4=10$

There are three types of solution: acidic, basic and neutral

To determine the type of solution, we look at the pH values.

• The pH range of acidic solution is 0 to 6.9
• The pH range of basic solution is 7.1 to 14
• The pH of neutral solution is 7.

As, the pH of the solution is 10 and is lying in the range of basic solution, so the solution is basic in nature.