At 30°C 0.1M acetic acid ionizes to the extent of 1%. The `P^H` of 0.1M acetic acid at 30°C is
(a) 1
(b) 3
(c) 4
(d) 2

The addition of NH_(4)Cl to 0.1 M acetic acid will cause

Calculate the H^+ ion concentration in 0.10 M acetic acid solution- Given that the dissociation constant of acetic acid in water is 1.8 xx 10^(-6) .

Calculate t the H^(+) ion concentration in 0.10 M acetic acid solution. Given that the dissociation constant of acetic acid in water is 1.8xx10^(-5)

Degree of dissociation of 0.1 molar acetic acid at 25^(@)C (K_(a) = 1.0 xx 10^(-5)) is

20 mL of 0.1 M acetic acid is mixed with 50 mL of potassium acetate. K_(a) of acetic acid = 1.8 xx 10^(-5) at 27^(circ)C . Calculate concentration of potassium acetate if pH of the mixture is 4.8.

Acetic acid is a weak acid. The molar conductances of 0.05 M acetic acid at 25^@C is 7.36 S " cm"^(2) "mol"^(-1) . If its ^^^_m^(oo) is 390.72 S cm^(2)"mol"^(-1) . The value of equilibrium constant is

The P^(H) of 10^(-3) M mono acidic base, if it is 1% ionised is

Degree of dissociation of decinormal acetic acid is 3.66% at 25^@C .If the equivalent conductance at infinite dilution of acetic acid at 25^@C is 390.7 "ohm"^(-1) ,calculate the equivalent conductance at given concentration.

What is pH of 7.0 xx 10^(-8)M acetic acid. What is the concentration of un-ionsed acetic acid. K_(a) of CH_(3)COOH = 1.8 xx 10^(-5) .

Calculate the percentage ionization of 0.01 M acetic acid in 0.1 M HCI. K_a of acetic acid is 1.8 xx 10^(-5)