The pH of the given 400 ml of 0.10 M solution is.
Further explanation:
Molarity:
The molarity of the solution can be defined as the concentration of the solution and is equal to the number of moles of the solute dissolved in 1 liter of the solution.
The expression of molarity (M), volume (V), and a number of moles (n) is as follows:
…… (1)
Here, V is a volume of solution in liters and n is a number of moles of solute.
Rearrange the above equation to calculate the number of moles from molarity.
…… (2)
The balanced dissociation reaction of barium hydroxide is,
Since barium hydroxide is a strong electrolyte. Therefore, according to the balanced equation,1 mole of barium hydroxide completely dissociates into 1 mole of barium ion and 2 moles of hydroxide ion in aqueous solution.
Given molarity of is 0.10 M and volume is 400.0 mL. Substitute these value in equation (2) to calculate the number of moles of .
Since 1 mole of produces 2 moles of hydroxide ion, therefore, 0.04 moles of will produce,
Hence, concentration of ions in the solution is calculated as follows:
The formula to calculate the pH of the solution is,
This expression can be elaborate as,
…… (3)
Substitute for in equation (3)
Therefore, the pH of the given solution is 13.3.
Learn more:
1. Equilibrium constant of pure water at 25°c: brainly.com/question/3467841
2. The difference between heat and temperature.: brainly.com/question/914750
Answer details:
Grade: Senior school
Subject: Chemistry
Chapter: Acid, bases and salts
Keywords: pH, 0.10 M baoh2, solution of barium hydroxide, pH 13.3, 2 mole oh- ions.