The solubility product of `AgCl` is `10^(-10)M^(2)`. The minimum volume ( in `m^(3))` of water required to dissolve `14.35 mg` of `AgCl` is approximately `:`
K_(sp) of AgCl is 1xx10^(-10) . Its solubility in 0.1 M KNO_(3) will be :
Find the product : - 2/9 × 10/3
Calculate approximate pH of 10^(-10) M NaOH at 25^(@)C.
Solubility of Ag_(2)CrO_(4) is 8 xx 10^(-5) mol L^(-1) . Calculate the solubility product.
The solubility of silver chloride (AgCl) in water at 25^(@)C ia 1.06 xx 10^(-5) mol L^(-1) . Calculate the solubility product of AgCl at this temperature.
The solubility of electrolytes MX_(1),MX_(2) and MX_(3) is 1xx10^(-3) moles per litre. Hence their respective solubility products are :
1L of pond water contains 20mg of Ca^(2+) and 12mg of mg^(2+) ions. What is the volume of a 2N Na_2 CO_3 solution required to soften 5000L of pond water ?
The value of the ion product constant for water, (K_(w)) at 60^(@) C is 9.6xx10^(-14) M^(2) what is the [H_(3)O^(+)] of a neutral aqueous solutoin at 60^(@) C and an aqueous solution with a pH=7.0 at 60 ^(@) C are respectively?
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
