If the concentration of $[Ag^{+}]$ in a solution is $1 \times 10^{-6} \ M$,what is the concentration of $[Br^{-}]$? Given that the $K_{sp}$ for $AgBr$ is $4.0 \times 10^{-13}$.
- A$4.0 \times 10^{-7} \ M$
- B$4.0 \times 10^{-6} \ M$
- C$2.0 \times 10^{-7} \ M$
- D$1.0 \times 10^{-7} \ M$
Explore More
Similar Questions
The solubility of sparingly soluble salt $AB_2$ is $1.0 \times 10^{-4} \ mol \ dm^{-3}$. What is its solubility product?
An ionic compound is dissolved simultaneously in heavy water and simple water. Its solubility is
Easy
View SolutionThe solubility product of $PbCl_2$ at $298 \ K$ is $1 \times 10^{-6}$. Its solubility in $mol/L$ is:
Medium
View SolutionThe $K_{sp}$ of $AgI$ is $1.5 \times 10^{-16}$. Which of the following mixtures of equal volumes will result in precipitation?
Difficult
View SolutionThe solubility of $CaF_2$ in a solution of $0.1 \ M \ Ca(NO_3)_2$ is.
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