Home
Class 12
CHEMISTRY
Calculate the change in pH of 1 litre bu...

Calculate the change in pH of 1 litre buffer solution containing `0.1` mole each of `NH_(3)` and `NH_(4)CI` upon addition of:
(i) `0.02` mole of dissolved gasous HCI.
(ii) `0.02` mole of dissolved of NaOH.
Assume no change in volume. `K_(NH_(3))=1.8xx10^(-5)`

Text Solution

Verified by Experts

The correct Answer is:
(i) ` Delta pH = 0.1761 ` unit
(ii) ` Delta pH = 0.1761 ` unit
Promotional Banner

Topper's Solved these Questions

  • EQUILIBRIUM

    AAKASH INSTITUTE|Exercise Assignment (SECTION-J) (AAKASH CHALLENGERS QUESTIONS)|6 Videos

  • EQUILIBRIUM

    AAKASH INSTITUTE|Exercise EXERCISE|50 Videos

  • EQUILIBRIUM

    AAKASH INSTITUTE|Exercise Assignment (SECTION-H) (MULTIPLE TRUE-FALSE TYPE QUESTIONS)|4 Videos

  • ENVIRONMENTAL CHEMISTRY

    AAKASH INSTITUTE|Exercise ASSIGNMENT (SECTION-D) (Assertion - Reason Type Questions)|5 Videos

  • GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF ELEMENTS

    AAKASH INSTITUTE|Exercise Assignment (Section-D) Assertion-Reason Type Question|15 Videos

Similar Questions

Explore conceptually related problems

Calculate the pH of a buffer solution containing 0.2 mole of NH_4Cl and 0.1 mole of NH_4OH per litre. K_b for NH_4OH=1.85xx10^(-5) .

Calculate pH of the buffer solution containing 0.15 mole of NH_(4)OH " and " 0.25 mole of NH_(4)Cl. K_(b) " for " NH_(4)OH " is " 1.98 xx 10^(-5) .

1 lit of buffer solution contains 0.1 mole each of NH_(4)OH and NH_(4)Cl . What will be the P^(H) of the solution when 0.01 mole of HCl is added to it [ P^(Kb) of NH_(4)OH = 4.74 ]

Calculate pH of a buffer solution that contains 0.1M NH_(4)OH(K_(b)=10^(-5)) and 0.1 M NH_(4)Cl.

Calculate the pH of a buffer by mixing 0.15 mole of NH_(4)OH and 0.25 mole of NH_(4)CI in a 1000mL solution K_(b) for NH_(4)OH = 2.0 xx 10^(-5)

Calculate the pH of a buffer solution containing 0.1 mole of acetic acid and 0.15 mole of sodium acetate. K_(c) for acetic acid is 1.75 xx 10^(-5) .

To 1.0L solution containing 0.1mol each of NH_(3) and NH_(4)C1,0.05mol NaOH is added. The change in pH will be (pK_(a) for CH_(3)COOH = 4.74)

Volume of 2 M HCl required to neutralise the solution containing 1"mole" of NH_(4)Cl and 1 "mole" of NaOH is: