The concentration of acetic acid `(K_(a)=1.8 xx 10^(-5))` required to give `3.5 xx 10^(-4) ` moles `//` litres of `H_(3)O^(+)` ions is

The concentration of acetic acid required to get 3.5 xx 10^(-4) mole/lit of H^(+) ion is [K_(a) = 1.8 xx 10^(-5) ]

The concentration of fluroacetic acid (K_(a)of acid =2.6xx10^(-3)) , which is required to get [H^(+)]=1.50xx10^(-3)M is:

The degree of ionization of 0.4 M acetic acid will be ( K _ a = 1.8 xx 10 ^( -5 ))

What concentration of dichloroacetic acid gives [H^(+)]=8.5xx10^(-3)M ? ("Given": K_(a)"of acid" = 5.0xx10^(-2)) .

The values of ionisation constants for some pairs of acids and bases are given which of them is stronger ? (a) Acetic acid (K_(a) =1.8 xx 10^(5)), boric acid (K_(a) =5,8 xx 10^(-10)) (b) Hydrofluoric acid (K_(a)= 6.7 xx 10^(-4)), benzoic acid (K_(a) =6.3 xx 10^(-5)) (c) Ammonium hydroxide (K_(b) =1.8 xx 10^(-5)) Magensium hydroxide (K_(b) =8.1 xx 10^(-3))

A mixture of weak acid is 0.1M in HCOOH (K_(a) = 1.8 xx 10^(-4)) and 0.1M in HOCN (K_(a) = 3.1 xx 10^(-4)) . Hence, [H_(3)O^(o+)] is

A mixture of weak acid is 0.1M in HCOOH (K_(a) = 1.8 xx 10^(-4)) and 0.1M in HOCN (K_(a) = 3.1 xx 10^(-4)) . Hence, [H_(3)O^(o+)] is

What concentration of acetic acid is needed to give a hudrogen ion concentration of 3.5xx10^(-4) M ? (K_(a)=1.8xx10^(-5)) ?

The dissociation constant of acetic acid is 1.8 xx 10^(-5) at 298 K. Calculate its degree of dissociation and H_3O^(+) ion concentration in its 0.1 M solution.