What is the kb of a 0.0200 m (at equilibrium) solution of methylamine, ch3nh2, that has a ph = 11.40? a.8.61 b. 7.92 × 10−22 c. 1.26 × 10−7 d. 3.15 × 10−4

The answer is D. 3.15 × 10−4

Now the dissolution of methylamine can be represented as follows:

CH3NH2 + H2O → CH3NH3OH  

The product formed dissociates and it is represented as given below

CH3NH3OH ↔ CH3CH3+ + OH-  

Now pH = 11.4 ,

Then pOH = 2.6  

[OH-] = 10^-2.6  

[OH-] = 2.51*10^-3  

Considering the below equation again

CH3NH3OH ↔ CH3CH3+ + OH-  

We can calculate Kb = [CH3NH3] [ OH-] / [CH3NH3OH]  

where Kb is the equilibrium constant.

Now [CH3NH3] = [OH-] = 2.51 × 10^-3

and [CH3NH3OH] = 0.020M (given)

Substituting these values we get  

Kb = ( 2.51 × 10^-3)² / 0.02  

Kb = 6.31 × 10^-6 / 0.02  

Kb = 3.15 × 10^-4

they are both synthetic elements

explanation:

d

c (diamond),

sio2 (quartz)