Question

A monobasic acid have dissociation constant equal to 1.8* 10^-5 at 25°C Calculate the degree of dissociation when molar concentration is equal to 0.20 M at the same temperature what is the concentration of H+ .​

Answer 1

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Answer 2

Concept:

Monobasic acid is an acid that can donate only one H+ ion during an acid-base reaction.

Eg: HA---- H+ + A-

Given:

Ka = 1.8×10^-⁵

Initially, HA------- H+   +      A-  

          0.20           0            0

Final

  0.20-0.20x      0.20x      0.20x

To find: Degree of dissociation and H+ concentration

Solution:  

As we know that

Ka= CX²/1-X = 0.2x²/1-x

1.8 × 10^-⁵ = 0.2x²/1-x

x² = 1.8 × 10^-⁵ × (1-x)/ 0.2

x²= 9 × 10^-⁵

x = √9 × 10^-⁵

x = 3 × 0.0031

x = 0.0093

Hence, the degree of dissociation  = 9.3 × 10^-³

Now, the concentration of H+ = 0.2x = 0.2 × 9.3 × 10^-³ = 1.86 × 10^-³ M

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