What is the hydronium ion concentration of a 0.25 M HA solution `(K_(a)=4xx10^(-8))`

What is the ionization constant of an acid if the hydronium ion concentration of a 0.40 M solution is 1.40xx10^(-4) M?

What is the ionization constant of an acid if the hydronium ion concentration of a 0.40 M solution is 1.40xx10^(-4) M?

What is the ionization constant of an acid if the hydronium ion concentration of a 0.40 M solution is 1.40xx10^(-4) M? (a) 1.96xx10^(-8) (b) 1.22xx10^(-9) (c) 4.90xx10^(-8) (d) 1.40xx10^(-6)

Explain the terms molecularity and order of a reaction. Give one example from each of first and second order reactions. A 0.1 M HCN solution contained 0.2 moles of KCN per litre of the solution. What was the hydronium ion concentration of the solution. (K_(a) for HCN = 7.2 xx 10^(-10) )

What is the approximate OH^(-) ion concentration of a 0.150M NH_(3) solution? (K_(b)=1.75xx10^(-5))

What is the approximate OH^(-) ion concentration of a 0.150M NH_(3) solution? (K_(b)=1.75xx10^(-5))

The hydrogen ion concentration of a 0.006 M benzoic acid solution is (K_(a) = 6 xx 10^(-5))

The hydrogen ion concentration of a 0.006 M benzoic acid solution is (K_(a) = 6 xx 10^(-5))

An acid HA is 40% dissociated in an aqueous solution. The hydronium ion concentration of its 0.2M solution would be