0.63 g sample of CaO is dissolved in enough water tomake 1529 mL of solution. Ca
ID: 676558 • Letter: 0
Question
0.63 g sample of CaO is dissolved in enough water tomake 1529 mL of solution. Calculate the pH of the solution.I got the molarity being0.63/56.08=0.0112mols 0.0112 mols/1.529L=0.00735M
I am confused on how to go aboutthis. I tried taking the log of this and got 2.13 which was wrongas the pH. Then I figured CaO + H2O-->Ca(OH)2 I am confusing myself and makingit more complicated that it probably is. Any help?
I got the molarity being0.63/56.08=0.0112mols 0.0112 mols/1.529L=0.00735M
I am confused on how to go aboutthis. I tried taking the log of this and got 2.13 which was wrongas the pH. Then I figured CaO + H2O-->Ca(OH)2 I am confusing myself and makingit more complicated that it probably is. Any help?
Explanation / Answer
CaO + H2O ==> Ca(OH)2 molar mass of CaO = 56 g/mol 0.63g/56g/mol =.01125 moles .01125 mol/1.529 L = 0.00736 M = [Ca(OH)2] [OH] = 2 x 0.00736M = .0147 M [OH] 1.0e-14 / .0147 = 6.8e-13 [H3O+] pH = -log[H3O+] = -log (6.8e-13) = 12.18
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