Home
Class 12
CHEMISTRY
Solubility of calcium phosphate (molecul...

Solubility of calcium phosphate (molecular mass, `M`) in water is `W g` per `100 mL` at `25^(@)C`. Its solubility product at `25^(@)C` will be approximately

A

`10^(9)((W)/(M))^(5)`

B

`10^(7)((W)/(M))^(5)`

C

`10^(5)((W)/(M))^(5)`

D

`10^(3)((W)/(M))^(5)`

Text Solution

Verified by Experts

The correct Answer is:
B
Promotional Banner

Similar Questions

Explore conceptually related problems

The solubility of an insoluble phosphate, M_(3)(PO_(4))_(2) of molecular weight w in water is x grams per litre, its solubility product is proportional to

The ionic product of water at 25^@C is 10^(-14) its ionic product at 90^@C will be

The solubility product of barium sulphate is 1.5 xx 10^(-9) at 18^(@)C . Its solubility in water at 18^(@)C is

Calculate solubility of AgCl in 0.1 M NaCl at 25^(@)C if its solubility product at same temperature is 2.0xx10^(10)

The solubility of a sparingly soluble salt A_xB_y in water at 25^@C=1.5xx10^(-4)M .The solubility product is 1.1xx10^(-11) The possibilities are

The solubility of CaF_2 in water at 298 K is 1.7 xx 10 ^(-3) grams per 100 cm ^(3) .Calculate the solubility product of CaF_2 at 298 K.

The solubility product of AgCl is 1.5625xx10^(-10) at 25^(@)C . Its solubility in g per litre will be :-

The solubility of AgCl in water at 298 K is 1.06xx10^(-5) mle per litre. Calculate its solubility product at this temperature.

A solution which remains in equilibrium with undissolved solute is said to be saturated. The concentration of a saturated solution at a given temperature is called solubility. The product of concentration of ions in a saturated solution of an electrolyte at a given temperature, is called solubility product (K_(sp)) . For the electrolyte, A_(x),B_(y),:A_(x),B_(y(s)) rarr xA^(y+)+ y^(Bx-) , with solubility S, the solubility product (K_(sp)) =x^(x)xxy^(y) xx s^(x+y) . While calculating the solubility of a sparingly soluble salt in the presence of some strong electrolyte containing a common ion, the common ion concentration is practically equal to that of strong electrolyte. If in a solution, the ionic product of an clectrolyte exceeds its K_(sp) , value at a particular temperature, then precipitation occurs. The solubility of PbSO_(4) , in water is 0.303 g/l at 25^(@) C, its solubility product at that temperature is

Calculate solubility of AgCI in 0.1 M NaCI at 25^@C if its solubility product at same temperature is 2.0 xx 10^(-10) .