Answer to Question #56387 in General Chemistry for kelly

Question #56387
What is the pH and pOH of a solution prepared by dissolving 1.50 g of Ca(OH)2 in water to make 965 mL of solution? Part A What is the pH of a solution? Express your answer using two decimal places. pH = ??? Part B What is the pOH of a solution? Express your answer using two decimal places. pOH = ???
Solution:
Part A)
Calcium hydroxide dissociates in the solution to produce hydroxyl anions, which create the basic pH of the solution.
Ca(OH)2 = Ca2+ + 2OH-
From the given mass we can calculate the concentration of the hydroxyl groups:
n(Ca(OH)2)=m(Ca(OH)2)/M(Ca(OH)2)=1.5/74=0.02 mol
n(OH−)=2*n(Ca(OH)2)=2*0.02=0.04 mol
Because V = 965 mL = 0.965 L :
[OH−]=c(OH−)=n(OH−)/V=0.04/0.965=0.042 M
And we can estimate the pH from the calculating pOH with the help of the formulas:
pOH = - log [OH-] from this, pOH = -log (0.042) = 1.38
pOH + pH = 14 from this, pH = 14 - pOH
pH = 14-1.38 = 12.62

Part B)
[OH−] = 0.042 M
pOH = - log [OH-] from this, pOH = -log (0.042) = 1.38

Part A) pH = 12.62
Part B) pOH = 1.38

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