Home
Class 12
CHEMISTRY
The solubility of AgCl(s) with solubilit...

The solubility of AgCl(s) with solubility product `1.6 xx 10^(-10)` ini 0.1 M NaCl solution would be -

A

zero

B

`1.26 xx 10^(-5)` M

C

`1.6 xx 10^(-9)` M

D

`1.6 xx 10^(-11)` M

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Topper's Solved these Questions

  • PREVIOUS YEAR QUESTION PAPER 2016

    CHHAYA PUBLICATION|Exercise NEET 2016 [ Phase- I]|13 Videos

  • PREVIOUS YEAR QUESTION PAPER 2019

    CHHAYA PUBLICATION|Exercise WBJEE 2019|18 Videos

  • PREVIOUS YEAR QUESTION PAPER 2017

    CHHAYA PUBLICATION|Exercise NEET 2017|13 Videos

Similar Questions

Explore conceptually related problems

The solubility of AgCl(s) with solubility product 1.6xx10^(-10) in 0.1 (M) NaCl solution would be-

If the solubility of Ca_3(PO_4)_2 in water be y mol L^(-1) , the solubility product of the salt will be -

Calculate the molar solubility of Ni(OH)_2 in 0.10 M NaOH. The solubility product of Ni(OH)_2 is 2.0 xx 10^(-15) .

Determine the pH of a solution which is obtained by mixing equal volume (50ml) of the solutions with pH 1 and 2. Given that the solubility product of BaSO_4 is 1.49xx10^(-9) . Determine its solubility in 0.1 M BaCl_2 solution.

Determine the simultaneous solutbiltiy of AgCN (K_(sp)=2.2xx10^-16) and AgCl(K_(sp)=1.6xx10^-10) in 1.0 M ammonia solution. K_f[Ag(NH_3)_2^+]=1.5xx10^7

An aqueous solution contains an unknown concentration of Ba^(2+) . When 50 mL of 1 M solution of Na_(2)SO_(4) is added , BaSO_(4) just begins to precipitate . The final volume is 500 mL . The solubility product of BaSO_(4) is 1 xx 10^(-10) . what is the original concentration of Ba^(2+) ?

Given the solubility product of Pb_3(PO_4)_2 is 1.5xx10^(-32) Determine the solubility in g/litre

The solubility product of a binary weak electrolyte is 4xx10^-10 at 298K. Its solubility in mol dm^(-3) at the same temperature is