Question

Calculate the pH of a solution made by adding 2. 60 g of lithium oxide (Li2O) to enough water to make 1. 700 L of solution

Answer 1

To solve this problem, let's write out the equation of reaction

$Li_2O + H_2O \to 2LiOH$

pH of a Solution

The pH of a solution indicates it's level of acidity. But in this question, lithium oxide dissolves in water to produce lithium hydroxide.

We can calculate the acidity of the solution by;

The numbers of moles is

$n = \frac{mass}{molar mass}\\n = \frac{2.6}{30}\\n = 0.086 moles$

1 mole of Li2O produce 2 moles LiOH

0.086 moles of H2O will give

$2 * 0.086 moles = 0.173 moles of LiOH$

The molarity of LiOH

$n = \frac{moles}{volume} = \frac{0.173}{1.70} = 0.102M$

Since we have the pOH of the solution, let's calculate the pH of the solution

$pH + pOH = 14\\pH = 14 - pOH\\pOH = 0.99\\pH = 14 - 0.99 = 13.009$

The pH of the solution is equal to 13.0

Learn more on pH of a solution here;

https://brainly.com/question/13557815