Home
Class 12
CHEMISTRY
Find "K"("b"), the ionization constant o...

Find `"K"_("b")`, the ionization constant of tartaric acid if a 0.100 molal aqueous solution of tartaric acid freezes at `-0.205^(@)"C"`. Assume that only the first ionization is of importance and that `0.1"m"=0.1"M". " K"_("f")=1.86 "kg mol"^(-1)"K".`

Promotional Banner

Similar Questions

Explore conceptually related problems

The cryoscopic constant of water is 1.86 K "mol"^(-1) kg. An aqueous solution of cane sugar freezes at -0.372^(@)C . Calculate the molality of the solution.

A 0.075 molal solution of monobasic acid has a freezing point of -0.18^(@)C . Calculate K_(a) for the acid , (k_(f)=1.86)

If the freezing point of a 0.01 molal aqueous solution of a cobalt chloride ammonia complex is -0.0558^@C , the number of chloride in the coordination sphere of the complex is [K_f of water =1.86K kg mol^-1]

0.2m aqueous solution of KCl freezes at -0.68^(@)C calculate van't Hoff factor. K _(f) for water is 1.86 K kg mol ^(-1).

A 0.1 molal aqueous solution of a weak acid is 30% ionized. If K_(f) for water is 1.86^(@)C//m , the freezing point of the solution will be.

A 0.1 molal aqueous solution of a weak acid is 30% ionized. If K_(f) for water is 1.86^(@)C//m , the freezing point of the solution will be.

0.01 m aqueous solution of K_(3)[Fe(CN)_(6)] freezes at -0.062^(@)C . What is the apparent percentage of dissociation ? ( K_(f) for water = 1.86" K kg mol"^(-1) )