A bufer solution was prepared by dissolving 0.05 mol formic acid & 0.06 mol sodium formate in enough water to make 1.0 L of solution. Ka for formic acid is `1.80 xx 10^(-4)`
Calculate the pH of the solution.

A bufer solution was prepared by dissolving 0.05 mol formic acid & 0.06 mol sodium formate in enough water to make 1.0 L of solution. Ka for formic acid is 1.80 xx 10^(-4) If this solution were diluted to 10 times its volume, what would be the pH ?

A solution was prepared by dissolving 0.63g of nitric acid in 10 L of the solution. Calculate its pH.

What is the pH of a 0.05 M solution of formic acid? (K_(a)=1.8xx10^(-4))

What is the pH of a buffer solution prepared by dissolving 0.1 mole of sodium acetate and 0.2 mole of acetic acid in enough water to make a dm^(3) of solution? ( K_(a) of acetic acid = 1.8xx10^(-5) ).

Calculate the pH of buffer solution prepared by dissolving 0.20 mol of sodium cyanate (NaCNO) and 1.0 mol of cynic acid (HCNO)in enough water to make 1.0 litre of solution . K_a(HCNO)=2.0 xx10^(-4)

Calculate the pH of buffer solution prepared by dissolving 0.20 mol of sodium cyanate (NaCNO) and 1.0 mol of cynic acid (HCNO)in enough water to make 1.0 litre of solution . K_a(HCNO)=2.0 xx10^(-4)

If K_(a) for formic acid is 2.0 xx 10^(-4) mol L^(-1) then K_(h) for HCOO^(-) is

Formic acid is 4.6% dissociated in a 0.1 N solution at 20^@C . The ionisation constant of formic acid is :