Test tubes $A$ and $B$ contain solutions of $NH_4Cl$ and $NaCl$ respectively. What happens if $Mg(OH)_2$ solution is added to both test tubes?
- APrecipitates will be formed in both $A$ and $B$.
- BThe solution in $A$ will remain clear,and precipitation will occur in $B$.
- CThe solution will remain clear in both $A$ and $B$.
- DNone of the above.
Explore More
Similar Questions
When $HCl$ gas is passed through a saturated solution of $BaCl_2$,a white precipitate is obtained. This is due to:
Difficult
View SolutionThe solubility of $BaSO_4$ in pure water is $10^{-5} \ M$ at $298 \ K$. The solubility of $BaSO_4$ in $0.1 \ M \ K_2SO_4$ (aq.) solution is: (Molar mass of $BaSO_4 = 233 \ g \ mol^{-1}$)
Medium
View SolutionIn the precipitation of the iron group in qualitative analysis,ammonium chloride is added before adding ammonium hydroxide to:
DifficultAIIMS 1980
View SolutionAssertion : $Sb_2S_3$ is not soluble in yellow ammonium sulphide. Reason : The common ion effect due to $S^{2-}$ ions reduces the solubility of $Sb_2S_3$.
MediumAIIMS 2006
View SolutionWhen $H_2S$ gas is passed through a solution containing $HCl$ during qualitative analysis,cations of the second group are precipitated,but cations of the fourth group are not precipitated because:
Easy
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