Browse by Stream
QnA
Home
QnA
Go To Your Study Dashboard

Get Answers to all your Questions

header-bg qa
  • Home
  • NCERT
  • The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.

7.60     The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.

Answers (1)

best_answer

We have,
Concentration of cyanic acid = 0.1 M
p^H=-\log [H^+] = 2.34

Therefore, the concentration of [H^+] = antilog (-2.34)
                                                            = 4.5 \times 10^{-3}

It is known that,
[H^+] =C.\alpha  = 4.5 \times 10^{-3}
 \alpha = \frac{4.5\times 10^{-3}}{0.1} = 4.5\times 10^{-2}

Then Ionization constant (K_a) =C.\alpha^2 = 
                                                   =(0.1)(4.5\times10^{-2})^2
                                                     =2.02\times 10^{-4}

Posted by

manish

View full answer

Crack CUET with india's "Best Teachers"

  • HD Video Lectures
  • Unlimited Mock Tests
  • Faculty Support
cuet_ads

Similar Questions

Trending Articles/News

anam-khan

CBSE Date Sheet 2025 (Out) Live: Class 10, 12 board exam time table at cbse.gov.in; syllabus, sample papers
anam-khan

CBSE Class 12 board exam date sheet 2025 out; exams from February 15 to April 4
anam-khan

When will CBSE Board exam 2025 date sheet be released for Class 10, 12?

Latest Question