A 0.10 M solution of C6H5NH2 has a pH of 9.82. What is the equilibrium constant, Kb, for this base?
Answer

2.1 x 10-4

4.3 x 10-8

8.8 x 10-8

6.6 x 10-4

2.0 x 10-5

Question

A 0.10 M solution of C6H5NH2 has a pH of 9.82. What is the equilibrium constant, Kb, for this base?
Answer
		
2.1 x 10-4
		
4.3 x 10-8
		
8.8 x 10-8
		
6.6 x 10-4
		
2.0 x 10-5

anonymous · Answer

The pH of a 0.010 M aqueous solution of calcium hydroxide is ___.
Answer
		
12.30
		
12.00
		
11.70
		
12.60
		
1.70

anonymous · Answer

help please i have 4 mins

nottim · Answer

well. i had this a while ago, but i cant remember much.
see....
n=0.10mol
pH=9.82
kb=?
ka= A constant; something like 1.7x10*-1 or something.

paxpolaris · Answer

i'm not sure i'm doing this right, but:

the pOH of 0.01M $Ca(OH)_2$ would be: $\Large -\log(0.02)$

to get pH you do 14 minus that