Home
Class 12
CHEMISTRY
Calculate the pH of an aqueous solution ...

Calculate the pH of an aqueous solution of `1.0M` ammonium formate assuming complete dissociation. `(pK_(a)` of formic acid `= 3.8 and pK_(b)` of ammonia `= 4.8`)

Text Solution

Verified by Experts

`6.5`
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (SUBJECTIVE ) LEVEL -II|13 Videos

  • IONIC EQUILIBRIUM

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE ) LEVEL - I|42 Videos

  • IONIC EQUILIBRIUM

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (SUBJECTIVE ) FILL IN THE BLANKS|7 Videos

  • HYDROCARBONS

    FIITJEE|Exercise SINGLE INTEGER ANSWER TYPE QUESTION|9 Videos

  • LIQUID SOLUTION

    FIITJEE|Exercise Single Integer Answer Type Question|10 Videos

Similar Questions

Explore conceptually related problems

What will be the pH of an aqueous solution of 1.0 M ammonium formate? Given : pK_(a)=3.8 and pK_(b)=4.8

The pH of aqueous solution of ammonium formate is (pK_(a) of HCOOH =3.7 and NH_(3)=4.8)

Calculate the pH of 0.05M sodium acetate solution, if the pK_(a) of acetic acid is 4.74 .

Calculate the pH of a 0.1 M aqueous ammonium cyanide solution. Given pK_a =9.02 and pK_b =4.76