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)` fo atomic acid is `3.8` and `pK_(a)` of ammonia is `4.8)`.

Text Solution

Verified by Experts

`6.5`
Promotional Banner

Similar Questions

Explore conceptually related problems

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 )

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 degree of dissociation (ionization) of 0.05 M acetic acid if its pK_(a) " is " 4.74 .

What is the pH of a 0.50M aqueous NaCN solution ? (pK_(b)of CN^(-)=4.70)

If degree of dissociation is 0.01 of decimolar solution of weak acid HA then pK_(a) of acid is :

Calcuate the pOH of 0.74g//L aqueous solution of propane - 1,2 -diamine .Given : pK_(b_(1))& pK_(b_(2)) for base is 4.18&7.39 respectively.

Calculate the pH of 0.01 M Solution of CH_3 COOH . The dissociation constant of the acid is 1.8 xx 10 ^(-5)

50 mL of 0.1 M solution of sodium acetate and 50 mL of 0.01 M acetic acid mixed. The pK_(a) of acetic acid is 4.76. The P^(H) of the buffer solution is