Assuming complete dissociation, what is the ph of a 4.02 mg/l ba(oh)2 solution?

The pH of the solution is 9.68

Explanation:

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

We are given:

Mass of solute (barium hydroxide) = 4.02 mg = 0.00402 g   (Conversion factor:  1 g = 1000 mg)

Molar mass of barium hydroxide = 171.34 g/mol

Volume of solution = 1 L

Putting values in above equation, we get:

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:

On complete dissociation, 1 mole of barium hydroxide produces 2 moles of hydroxide ions

We are given:

Putting values in above equation, we get:

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

Hence, the pH of the solution is 9.68

the temperature of the gas, in k, not celsius.