Home
Class 12
CHEMISTRY
Calculate the degree of dissociation (io...

Calculate the degree of dissociation (ionization) of `0.05` M acetic acid if its `pK_(a) " is " 4.74`.

Text Solution

AI Generated Solution

To calculate the degree of dissociation (ionization) of 0.05 M acetic acid given its pKa of 4.74, we can follow these steps: ### Step 1: Convert pKa to Ka We know that: \[ pK_a = -\log(K_a) \] Given \( pK_a = 4.74 \), we can find \( K_a \) using the formula: \[ K_a = 10^{-pK_a} \] Substituting the value: ...
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise Illustration - 8|1 Videos

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise Illustration - 9|1 Videos

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise Illustration - 6|1 Videos

  • INTRODUCTION TO ORGANIC CHEMISTRY

    VMC MODULES ENGLISH|Exercise JEE ADVANCED ARCHIVE|81 Videos

  • JEE MAIN - 5

    VMC MODULES ENGLISH|Exercise PART II : CHEMISTRY (SECTION - 2)|5 Videos

Similar Questions

Explore conceptually related problems

Calculate the degree of ionisation of 0.05 M acetic acid if its pK_a , value is 4.74. How is the degree of dissociation affected when its solution also contains (a) 0.01 M (b) 0.1 M in HCl ?

The degree of dissociation (extent of ionization ) increases

Calculate the degree of dissociation (alpha) of acetic acid if its molar conductivity (^^_(m)) is 39.05 S cm^(2) mol^(-1) Given lamda^(@) (H^(+)) = 349.6 cm^(2) mol^(-1) and lamda^(2) (CH_(3)COO^(-)) = 40.9 S cm^(2) mol^(-1)

The degree of dissociation of 0.1 M acetic acid is 1.4 xx 10^(-2) . Find out the pKa?

The ionization constant of acetic acid 1.74xx10^(-5) . Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH .

The ionization constant of propionic acid is 1.32xx10^(-5) . Calculate the degree of ionization of the acid in its 0.05 M solution and also its pH. What will be its degree of ionization in the solution of 0.01N HCI ?

Calculate the percentage ionization of 0.01 M acetic acid in 0.1 M HCI. K_a of acetic acid is 1.8 xx 10^(-5)

If degree of dissociation is 0.01 of decimolar solution of weak acid HA then pK_(a) of acid is :

What will be the degree of dissociation of 0.005M NH_(4)OH solution. If pK_(b) for NH_(4)OH is 4.7

Degree of dissociation of 0.1 molar acetic acid at 25^(@)C (K_(a) = 1.0 xx 10^(-5)) is