For example: What is the pH of a 0.010 M NaOH solution? What is the pH of a 0.00
ID: 1040629 • Letter: F
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For example: What is the pH of a 0.010 M NaOH solution? What is the pH of a 0.0010 M HNO3 solution? What is the pH of a 0.035 M Ca(OH), solution? What is the pH of 0.15 M solution of H.SO,? This last one is not as straight forward. There are two acidic protons with only the loss of the first one being strong. The loss of the second acidic hydrogen is weak. What would be the maximum and minimum pH value? The formula HA can be used to represent a general weak acid. HA(aq) + H2O(1) H30"(aq) + A-(aq) H30* A HA KaExplanation / Answer
0.01 M NaOH : NaOH + H2O - - - - > OH- +H3O+
[OH-] = 0.01 M
pOH = -log[OH-] = -log(0.01) = 2
PH = 14-pOH =14-2=10
0.001 M HNO3 : HNO3 + H2O - - - - > H3O+ + NO3-
pH = -log(H3O+) = - log(H+) = - log(0.001)= 3
0.035M Ca(OH)2: Ca(OH)2 + H2O - - - - > 2 OH- + Ca+2
[OH-] = 2x 0.035= 0.070 M
pOH = -log(OH-)=-log(0.070)= 1.15
PH = 14-1.15 =12.85
0.15 M H2SO4 : H2SO4 - - - - > 2 H+ +SO42-
[H+] = 2x 0.15= 0.30 M
pH =-log(0.30)= 0.52
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