What is the `K_b` of a weak base that produces one `OH^-` per molecule if a 0.050 M solution is 2.5% ionized ?

A 0.010 M solution of a weak acid that produces one OH^- pe molecule of a 0.050 M solution is 2.5% ionized ?

What is the K_(b) of weak base that produce one OH-ion if a 0.05 M solution is 2.5% ionised ?

What is the K_(b) of weak base that produce one OH-ion if a 0.05 M solution is 2.5% ionised ?

The concentration of OH^(-) ions in a 0.050 M HNO_(3) solution is

What is the pH of a 0.010 M solution of a weak acid HA that is 4.0 % ionized ?

What is dissociation constant of a weak base (K_(b)) .

The pH of an aqueous solution of a 0.1 M solution of weak monoprotic acid, which is 1 % ionized is

1.0 M solution of a weak base , BOH is only 0.5 % ionized . If 2 mL 1 M solution of BOH is mixed with 30 mL water , the degree of dissociation of the base in the resulting solution and H^(+) ion concentration of the solution will bee respectively

1.0 M solution of a weak base , BOH is only 0.5 % ionized . If 2 mL 1 M solution of BOH is mixed with 30 mL water , the degree of dissociation of the base in the resulting solution and H^(+) ion concentration of the solution will bee respectively

A 0.5 molal aqueous solution of a weak acid (HX) is 20 percent ionized. The lowering in freezing point of this solution is ( K_f = 1.86 K/m for water)