$1 \ dm^{3}$ solution containing $10^{-5} \ mol$ each of $Cl^{-}$ ions and $CrO_{4}^{2-}$ ions is treated with $10^{-4} \ mol$ of silver nitrate. Which one of the following observations is made?
$[K_{sp} \ Ag_{2}CrO_{4} = 4 \times 10^{-12}]$
$[K_{sp} \ AgCl = 1 \times 10^{-10}]$
$[K_{sp} \ Ag_{2}CrO_{4} = 4 \times 10^{-12}]$
$[K_{sp} \ AgCl = 1 \times 10^{-10}]$
- APrecipitation does not occur
- BSilver chromate gets precipitated first
- CSilver chloride gets precipitated first
- DBoth silver chromate and silver chloride start precipitating simultaneously
Explore More
Similar Questions
Calculate the solubility of sparingly soluble salt $BA$ in $mol \ dm^{-3}$ at $300 \ K$ if its solubility product is $4.9 \times 10^{-9}$ at same temperature.
An acidified solution of $0.05 \ M \ Zn^{2+}$ is saturated with $0.1 \ M \ H_2S$. What is the minimum molar concentration $(M)$ of $H^{+}$ required to prevent the precipitation of $ZnS$? Use $K_{sp}(ZnS) = 1.25 \times 10^{-22}$ and overall dissociation constant of $H_2S$,$K_{NET} = K_1 K_2 = 1 \times 10^{-21}$.
What is the solubility of $PbSO_4$ in centinormal $(0.01 \ N)$ $H_2SO_4$ solution? The solubility product $(K_{sp})$ of $PbSO_4$ at a given temperature is $1 \times 10^{-8} \ (mol/L)^2$.
Difficult
View SolutionThe $K_{sp}$ of $AgCl$ at $18\, ^oC$ is $1.8 \times 10^{-10}$. If the concentration of $Ag^{+}$ is $4 \times 10^{-3}\ mol/L$,what is the minimum concentration of $Cl^{-}$ required for $AgCl$ precipitation?
Medium
View Solution$A$ precipitate of $CaF_2$ $(K_{sp} = 1.7 \times 10^{-10})$ will be obtained when equal volumes of the following are mixed:
Medium
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo