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Rashid [163]
4 years ago
14

If the kb of a weak base is 3.3 Ã 10-6, what is the ph of a 0.17 m solution of this base?

Chemistry
1 answer:
Nana76 [90]4 years ago
8 0

The relation between base equilibrium constant and degree of dissociation is

C x^2 = Kb

x is degree of dissociation

C x^2 = 3.3 * 10^-6

(0.17) x^2 = 3.3 * 10^-6

x = 4.24 * 10^-3

Concentration of hydroxyl ion is

[OH-] = c x = 0.17 * 4.24 * 10^-3 = 0.72 * 10^-3 M

PoH = - log [OH-] = 2.85

PH = 14 - pOH = 11.15

Hence, pH of solution is 11.15

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If I have 21,000 mL of gas at a temperature of 870C and a pressure of 101 atm, what will be the pressure of the gas if I raise t
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Answer:

We  have,

Initial volume is V  

1

​  

 

Initial temprature is T  

1

​  

=75  

0

C

Initial pressure is P  

1

​  

 

So, final temprature is T  

2

​  

=273+75=348K

V  

2

​  

=V  

1

​  

−  

100

15

​  

V  

1

​  

 

=  

100

85V  

1

​  

 

​  

 

Applying the gas formula,

T  

1

​  

 

P  

1

​  

V  

1

​  

 

​  

=  

T  

2

​  

 

P  

2

​  

V  

2

​  

 

​  

 

348

P  

1

​  

V  

1

​  

 

​  

=  

T  

2

​  

×100

2P  

1

​  

×85V  

1

​  

 

​  

 

T  

2

​  

=  

100

2×85×348

​  

 

T  

2

​  

=591.6K

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3 years ago
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