What is the concentration of $Ba^{2+}$ when $BaF_2$ $(K_{sp} = 1.0 \times 10^{-6})$ begins to precipitate from a solution that is $0.30 \, M \ F^{-}$?
- A$9.0 \times 10^{-7} \, M$
- B$3.3 \times 10^{-5} \, M$
- C$1.1 \times 10^{-5} \, M$
- D$3.0 \times 10^{-7} \, M$
Explore More
Similar Questions
$PbCl_2$ has a maximum concentration of $1.0 \times 10^{-3} \ M$ in its saturated aqueous solution at $25 \ ^oC$. Its solubility in a $0.1 \ M \ NaCl$ solution will be:
Medium
View SolutionThe solubility product of $PbI_{2}$ is $8.0 \times 10^{-9}$. The solubility of lead iodide in $0.1 \ M$ solution of lead nitrate is $x \times 10^{-6} \ mol/L$. The value of $x$ is ....... .(Rounded off to the nearest integer)
$[$Given: $\sqrt{2}=1.41]$
$[$Given: $\sqrt{2}=1.41]$
The solubility product of $AgCl$ is $4.0 \times 10^{-10}$ at $298 \ K$. The solubility of $AgCl$ in $0.04 \ m \ CaCl_2$ will be
Medium
View SolutionThe molar solubility of $Cd(OH)_2$ is $1.84 \times 10^{-5} \ M$ in water. The expected solubility of $Cd(OH)_2$ in a buffer solution of $pH = 12$ is
DifficultJEE MAIN 2019
View Solution$MX$ is a salt formed by neutralization of a strong base,$MOH$,and a weak acid,$HX$. If the dissociation constant of $HX$ is $K_a$ and the solubility product of $MX$ is $K_{sp}$,then the solubility of $MX$ in an aqueous acidic solution is given by:
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