Equal volumes of `0.002M` solutions of sodium iodate and cupric chlorate are mixed together. Will it lead to precipitation of copper iodate ? (For cupric iodate `K_(sp)=7.4xx10^(-8)`).

What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipition of iron sulphide ? (For iron sulphide , K_(sp)=6.3xx10^(-18) ).

100 ml of 0.1 M HCl and 100 ml of 0.1 M HOCN are mixed . What is the concentration of .. OCN ^(-).. , and pH of the solution ? (K_a=1.2 xx 10^(-6) )

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 BaSO_(4) , in 0.1 M BaCl_(2) , solution is (K_(sp) , of BaSO_(4), = 1.5 xx 10^(-9))

A sample of hard water contains 0.005 moles of calcium chloride per litre.What is the minimum concentration of sodium sulphate which must be added for removing the Ca^(2+) ions from this water sample ? K_(sp) " of " CaSO_4= 2.4 xx 10^(-5)

A solution of 0.01 MCd^(2+) contains 0.01M NH_4OH. What conc. Of NH_4^(+) from NH_4Cl is necessary to prevent precipitation of Cd( OH)_2? K_(sp) " of " (OH)_2 =2.0 xx 10^(-14) ,K_b " of " NH_4 OH = 1.8 xx 10^(-5) if answer is 1.272 xx 10^(-x) mol/litre then x=________?