Home
Class 11
CHEMISTRY
Calculate [H^(+) ] in a 0.1 M solution ...

Calculate `[H^(+) ]` in a 0.1 M solution of dichloroacetic acid `(K_a =5 xx 10 ^(-2) ) ` that also contains 0.1 M sodium dichloroacetae. Neglect hydrolysis of sodium salt. If `[H^(+) ]= yxx 10 ^(-2) ` then what is the value of y ?

Text Solution

Verified by Experts

The correct Answer is:
5
` pH= pKa+log ""(S)/(A) =2- log 5 +log ""(0.1)/(0.1) `
` pH =2 -log 5 rArr [H^(+)] =5 xx 10 ^(-2) `
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    AAKASH SERIES|Exercise PRACTICE SHEET (EXERCISE -IV LEVEL -I (MAIN) (Straight Objective Type Questions))|24 Videos

  • IONIC EQUILIBRIUM

    AAKASH SERIES|Exercise PRACTICE SHEET (EXERCISE -IV LEVEL -I (ADVANCED) (Straight Objective Type Questions))|20 Videos

  • IONIC EQUILIBRIUM

    AAKASH SERIES|Exercise PRACTICE SHEET (EXERCISE -III LEVEL -II (ADVANCED) (Matrix Matching Type Questions))|4 Videos

  • HYDROGEN AND ITS COMPOUNDS

    AAKASH SERIES|Exercise QUESTIONS FOR DESCRIPTIVE ANSWERS|20 Videos

  • ISOMERISM

    AAKASH SERIES|Exercise ADDITIONAL PRACTICE EXERCISE ( PRACTICE SHEET (ADVANCED) INTEGER TYPE QUESTIONS)|10 Videos

Similar Questions

Explore conceptually related problems

Calculate pH of a 1.0xx10^(-8) M solution of HCl.

5L of 0.1 M solution of sodium Carbonate contains

The nature of 0.1 M solution of sodium bisulphate is

The ionization constant of chloroacetic acid is 1.65xx10^(-3) . What will be the pH of 0.1M acid and its 0.1M sodium salt solution ?

What [NH_4^(+) ] in a solution that contains 0.02M NH_3 (K_b =1.8 xx 10^(-5) ) and 0.01 M KOH ?

Solubility of silver chloride in pure water is 1 xx 10^(-5) M. What is its solubility in 0.001M sodium chloride solution ?

Calculate pH of 0.1 M acetic acid having K_(a)=1.8xx10^(-5)