Question

An Amine RHN2 has a PKb of 4.20. What is the pH of a 0.20M solution of the base? (need complete solution step wise) ​

Answer 1

Answer:

https://eanswersin.com/chemistry/question526845096

Answer 2

Answer:

The pH of a 0.20M solution of the base is 11.2.

Explanation:

• If its a weak monoacidic base like ammonia and amines then,

                        [OH-] = √Kb × molarity of base

                   ⇒   [OH-] = √ (6.3×$10^{-5}$) × .2  

                                         [Pkb = -log(kb) ⇒ 4.2 = -log(kb) ⇒ kb = 6.3×$10^{-5}$]

                   ⇒    [OH-] = 1.5 × $10^{-3}$

• So, pOH will be -log(1.5 × $10^{-3}$) = 2.8
• pH = 14 - pOH ⇒ pH = 14 - 2.8 ⇒ pH = 11.2

To learn more about base:

https://brainly.in/question/395570

To learn more about amines:

https://brainly.in/question/6278646

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