Home
Class 12
CHEMISTRY
A 0.02M solution of pyridinium hydrochlo...

A 0.02M solution of pyridinium hydrochloride has pH = 3.44. Calculate the ionization constant of pyridine.

Text Solution

Verified by Experts

The aqueous solution of pyridium hydrochloride is an acidic solution due to hydrolysis. Observe that it is a salt of strong acid, HCl and weak base, Pyridine.
`C_(5)H_(5)N^(+)HCl^(-) + H_(2)O to C_(6)H_(5)N^(+)HOH^(-) + HCl`
Using standard result of pH :`pH=7- (pK_(b))/2 – (logC)/2 implies 3.44=7- (pK_(b))/2 – (log0.02)/2`
On solving and substituting values, `K_(b)=1.5xx10^(-9)`
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise LEVEL 1|75 Videos

  • IONIC EQUILIBRIUM

    VMC MODULES ENGLISH|Exercise LEVEL 2|50 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

A 0.02 M solution of pyridinium hydrochloride has pH=3.44 . Calculate the ionization constant of pyridine.

(i) Predict if the aqueous solutions of the following salts are neutral acidic or basic, NaCl,KBr,NaCN,NH_(4)NO_(3),NaNO_(3) and KF .Explain. (ii) A 0.02M solution of pyridinium hystochloride has pH=3.44 calcuate ionization constant of pyridine (antiolog 0.18=1.5 ) (iii) The ionization constant of nitrous acid is 4.5xx10^(-4) .Calculate the pH of 0.04M solution nitrite solution and also its degree of hydrolysis (log 4.5=0.65,log4=0.6)

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

It has been found that the pH of a 0.01 M solution of an organic acid is 4.15 . Calculate the concentration of the anion, the ionization constant of the acid and its pK_(a) .

Calculate [OH^(-)]and % dissociation of 0.01 M solution of ammonium hydroxide solution. The ionization constant for NH_(4)OH(K_(b))=1.8xx10^(-5)

A 0.25M solution of pyridinium chloride (C_(5)H_(5)overset(o+)NHCl^(Theta)) has pH of 2.89 . Calculate pK_(b) for pyridine (C_(5)H_(5)N) .

What is the pH of 0.001 M aniline solution? The ionization constant of aniline 4.27xx10^(-10) . Calculate the degree of ionization of aniline in the solution. Also calculate the ionization constant of the conjustant acid of aniline.

What is the pH of a solution of 0.28 M acid and 0.84 M of its conjugate base if the ionization constant of acid is 4xx10^(-4) ?

Determine the degree if ionization and pH of 0.05 M of ammonia solution. The ionization constant of ammonia can be taken from Table 7.7. Also calculate the ionization constant of the conjugate acid of ammonia.

A 0.20 M solution of methanoic acid has degree of ionization of 0.032. Its dissociation constant would be