SATHEE: Chemical and Ionic Equilibrium 2 Question 62

Chemical and Ionic Equilibrium 2 Question 62

62. Calculate the $pH$ of an aqueous solution of $1.0 M$ ammonium formate assuming complete dissociation.

$(p K_{a}$ of formic acid $= 3.8$ and $p K_{b}$ of ammonia $= 4.8)$

(1995, 2M)

Show Answer

Solution:

For salts of weak acid and weak base .

$pH = 7 + \frac{1}{2} (p K_{a} - p K_{b}) = 7 + \frac{1}{2} (3.8 - 4.8) = 6.50$

Play Store

App Store

Ask SATHEE

Welcome to SATHEE !
Select from 'Menu' to explore our services, or ask SATHEE to get started. Let's embark on this journey of growth together! 🌐📚🚀🎓

I'm relatively new and can sometimes make mistakes.
If you notice any error, such as an incorrect solution, please use the thumbs down icon to aid my learning.
To begin your journey now, click on "I understand".

Chemical and Ionic Equilibrium 2 Question 62

62. Calculate the pH of an aqueous solution of 1.0M ammonium formate assuming complete dissociation.

Solution:

Engineering Preparation

Medical Preparation

NCERT Books & Solutions

Important Resources

Other Resources

Syllabus

Test Platform

Sample Mock Test

Mentorship

Menu

62. Calculate the $pH$ of an aqueous solution of $1.0 M$ ammonium formate assuming complete dissociation.