When 741g of solid CaOH2 Molar mass = 7409gmole Ksp = 502×10-6 is dissolved into 100L of water assume there is no change in volume the pH of the solution is closest to

To find the pH of the solution, we need to determine the concentration of hydroxide ions (OH-) in the solution.

First, we need to find the number of moles of Ca(OH)2 in the solution: Number of moles = mass / molar mass Number of moles = 7.41g / 74.09g/mol = 0.1 mol

Since Ca(OH)2 dissociates into 2 moles of OH- for every 1 mole of Ca(OH)2, the concentration of OH- ions in the solution is: Concentration of OH- = 2 * 0.1 mol / 1.00L = 0.2 M

Now, we can use the following relationship to find the pOH of the solution: pOH = -log[OH-] pOH = -log(0.2) pOH ≈ 0.70

Finally, we can find the pH of the solution using the equation: pH = 14 - pOH pH = 14 - 0.70 pH ≈ 13.30

Therefore, the pH of the solution is closest to 13.30