Predict the feasibility of the given reactions in aqueous solution:
$(i)$ $Be(OH)_2 + 2 OH^{-} \longrightarrow [Be(OH)_4]^{2-}$
$(ii)$ $Be(OH)_2 + 2 H^{+} \longrightarrow Be^{2+} + 2 H_2O$
$(i)$ $Be(OH)_2 + 2 OH^{-} \longrightarrow [Be(OH)_4]^{2-}$
$(ii)$ $Be(OH)_2 + 2 H^{+} \longrightarrow Be^{2+} + 2 H_2O$
- AOnly $(i)$ is feasible
- BOnly $(ii)$ is feasible
- C$(i)$ and $(ii)$ are feasible
- D$(i)$ and $(ii)$ are not feasible
Explore More
Similar Questions
Identify correct statements from the following:
$i$. Beryllium oxide is an amphoteric oxide.
$ii$. Group $II$ elements dissolve in liquid ammonia to form deep blue-black solutions.
$iii$. The hydration enthalpy of group $II$ ions decreases from $Be^{2+}$ to $Ba^{2+}$.
$i$. Beryllium oxide is an amphoteric oxide.
$ii$. Group $II$ elements dissolve in liquid ammonia to form deep blue-black solutions.
$iii$. The hydration enthalpy of group $II$ ions decreases from $Be^{2+}$ to $Ba^{2+}$.
$MgO$ is used as a refractory material because
Medium
View SolutionThe solubility of sulfates in water decreases down the group for $Be$ to $Ba$. The correct order is $BeSO_4 > MgSO_4 > CaSO_4 > SrSO_4 > BaSO_4$. The reason for this is:
Medium
View SolutionDiscuss the general characteristics and gradation in properties of alkaline earth metals.
Difficult
View SolutionAssertion $(A):- MgSO_{4}$ is readily soluble in water.
Reason $(R):-$ The greater hydration enthalpy of $Mg^{2+}$ ions overcomes its lattice enthalpy.
Reason $(R):-$ The greater hydration enthalpy of $Mg^{2+}$ ions overcomes its lattice enthalpy.
Vedclass 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