Asolution is made by adding 0.350 g ca(oh)2(s), 45.0 ml of 1.00 m hno3, and enough water to make a final volume of 75.0 ml. assuming that all of the solid dissolves, what is the ph of the final solution?

0.323

Explanation:

number of moles of Ca(OH)2(s) = mass given / molar mass = 0.350 g / 74.093 g/mol = 0.00472 mol

number of mole of HNO3 = Molarity × volume in Liters = 1.0  × (45 / 1000) = 0.045 M

Ca(OH)2(s) + 2 HNO3(aq) → Ca(NO₃)₂(aq) + 2 H₂O(I)

1 mole of calcium hydroxide react with 2 mole of trioxonitrate(V)

0.00472 mole will require 0.00945 mole

but we have 0.045 mole of the acid

net mole = 0.045 - 0.00945 = 0.0356 mole

Molarity of the net mole = 0.0356 / (75/1000) = 0.475 M

pH = - log (0.475) = 0.323

12 is it do you think so