In pure liquid of `HCOOH`, concentration of `HCOO^(-)=10^(-3) M` at `27^(@)C`. What is the self- ionisation constant `(K=[HCOOH^(2+)][HCOO^(-)])`

For the self-ionisation (protonation) process liquid formic acid at 20^(@) C. HCOOH+HCOOHto HCOOH_(2)^(+)+HCOO^(-) the equilibrium constant, K=([HCOOH_(2)^(+)][HCOO^(-)])/([HCOOH]^(2))=10^(-10) At 20^(@) C, the density of liquid formic acid is 0.92 gm/mL. The ionic prodcut of formic acid, K=[HCOOH_(2)^(+)][HCOO^(-)] is :

For the self-ionisation (protonation) process liquid formic acid at 20^(@) C. HCOOH+HCOOHto HCOOH_(2)^(+)+HCOO^(-) the equilibrium constant, K=([HCOOH_(2)^(+)][HCOO^(-)])/([HCOOH]^(2))=10^(-10) At 20^(@) C, the density of liquid formic acid is 0.92 gm/mL. How many formate ions (HCOO^(-)) are present in each 5ml of liq.formic acid at 20^(@) C? (N_(A)=6xx10^(23))

For the self-ionisation (protonation) process liquid formic acid at 20^(@) C. HCOOH+HCOOHto HCOOH_(2)^(+)+HCOO^(-) the equilibrium constant, K=([HCOOH_(2)^(+)][HCOO^(-)])/([HCOOH]^(2))=10^(-10) At 20^(@) C, the density of liquid formic acid is 0.92 gm/mL. What percentage of formic acid molecules are self ionised?

Refer to an aqueous solution of formic acid, HCOOH , which has a K_(a) value of 1.9 xx 10^(-4) at 25^(@)C . What is the percent ionization of a 0.10 M solution of formic acid at 25^(@)C

What concentration of HCOO^(-) is present in a solution of weak of 0.01 M HCOOH (K_(a)=1.8xx10^(-4) and 0.01 M HCl?

What concentration of HCOO^(-) is present in a solution of weak of 0.01 M HCOOH (K_(a)=1.8xx10^(-4) and 0.01 M HCl?

What concentration of HCOO^(-) is present in a solution of weak of 0.01 M HCOOH (K_(a)=1.8xx10^(-4) and 0.01 M HCl?

Calculate the ratio of concentration of HCOO^(-) & OCN^(-) ions in a solution containing 0.1M HCOOH (K_(a)=1.8xx10^(-4)) and 0.1M HOCN(K_(a_(1))=4xx10^(-4)) .if simplest ratio is a:b reprot your answer as (a+b) .

Neutralisation constant of HCOOH with a strong bse is 10^(8) . What is the pH of 0.01 M HCOOK solution at 25^(0)C ?

Liquid ammonia ionises to a slight extent. At -50^(@)C , its self ionisation constant, K_(NH_(3))=[NH_(4)^(+)][NH_(2)^(-)]=10^(-30) . How many amide ions are present per cm^(3) of pure liquid ammonia ? ("Assume" N=6.0xx10^(23))