The solubility product of $AgBr$ is $4.9 \times 10^{-13}$ at a certain temperature. Calculate the solubility.
- A$4 \times 10^{-6} \ mol \ dm^{-3}$
- B$4 \times 10^{-7} \ mol \ dm^{-3}$
- C$7 \times 10^{-7} \ mol \ dm^{-3}$
- D$3 \times 10^{-8} \ mol \ dm^{-3}$
Explore More
Similar Questions
The $K_{sp}$ for $AgBr$ at $25 \, ^\circ C$ is $4.9 \times 10^{-13}$. How much $AgBr$ (in grams) will dissolve in $20 \, L$ of its saturated solution? (Molecular weight of $AgBr = 188$)
Medium
View SolutionAt $298 \ K$,the solubility of $PbCl_2$ is $2 \times 10^{-2} \ mol/L$. Calculate the $K_{sp}$.
Medium
View SolutionIf the concentration of sodium ions in a saturated solution of $Na_2SO_4$ is $10^{-5} \ mol/L$,find the solubility product $(K_{sp})$.
Medium
View SolutionThe $K_{sp}$ of $AgI$ is $1.5 \times 10^{-16}$. Precipitation will occur upon mixing equal volumes of which of the following solutions?
Medium
View SolutionWhat is the molarity of $F^{-}$ in a saturated solution of $InF_3$? $(K_{sp} = 7.9 \times 10^{-10})$
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