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I know the answers to these but can you explain/work out the problems here. I am not sure how to calculate these.
I know the answers to these but can you explain/work out the problems here. I am not sure how to calculate these.
What is the pH of a 0.20 M aqueous solution of CH3NH2 at 25oC? Kb for CH3NH2 = 4.4 x 10-4 and Ka for CH3NH3+ = 2.3 x 10-11
A) 0.70
B) 2.03
C) 7.00
D) 11.97
E) 13.30
2. What concentration of an aqueous solution of HBrO2 is required to result in the same pH as a 0.050 M solution of HCl? Ka for HBrO2 = 3.7 x 10-4 and Ka for HCl = 1 x 108
A) 0.0043 M
B) 0.050 M
C) 0.054 M
D) 5.00 M
E) 6.81 M
1. Determine the Kb value for HAsO42- at 25oC given that for H3AsO4:
Ka1 = 5.0 x 10-3
Ka2 = 8.0 x 10-8
Ka3 = 6.0 x 10-10
A) 1.7 x 10-5
B) 1.3 x 10-7
C) 4.0 x 10-10
D) 6.0 x 10-10
E) 2.0 x 10-12
Calculate the pH of 1.00 L of solution consisting of 0.50 M CH3COOH and 0.35 M LiCH3COO after 0.150 mol of solid NaOH have been added (assume no change in volume). The Ka of CH3COOH is 1.8x10-5 and the Kb for NaOH is 1 x 107
A) 4.23
B) 4.59
C) 4.74
D) 4.90
E) 5.26
A diprotic acid, H2A, has the following acid dissociation constants: Ka1 = 1.1 x 10-3 and Ka2 = 2.5 x 10-6. Which combination of species would you use to make a buffer solution whose pH is 3.25?
A) NaHA / H2A
B) Na2A / NaHA
C) H2A / NaHA / Na2A
D) H2A / Na2A
E) H2A and its conjugates cannot be used to form a buffer of pH = 3.25
