The pH of a solution containing 49.0 mL of 0.10 M KOH and 50.0 mL of 0.10 M of HBr is:
a. 5.0 b. 3.0 d. 7.0 e. 4.0
answer : b ) 3.0
solution:
millimoles of KOH = 49.0 x 0.10 = 4.90
millimoles of HBr = 50 x 0.1 = 5
millimoles of acid > millimoles of base
after reaction millimoles of acid remains = 5- 4.9 = 0.1
molarity of [H+] = 0.1 / total volume
= 0.1 / (49 +50)
= 1.0 x 10^-3 M
pH = -log [H+]
pH = -log (1.0 x 10^-3)
pH = 3.0
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