A solution has 0.05MMg2+ and 0.05MNH3. The concentration of NH4Cl required to prevent the formation of Mg(OH)2 in solution is: Ksp of Mg(OH)2=9.0×10−12 and Kb of NH3=1.8×10−5.
0.062M
0.067M
0.075M
0.070M
A
0.067M
B
0.075M
C
0.070M
D
0.062M
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Q1
A solution has 0.05MMg2+ and 0.05MNH3. The concentration of NH4Cl required to prevent the formation of Mg(OH)2 in solution is: Ksp of Mg(OH)2=9.0×10−12 and Kb of NH3=1.8×10−5.
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Q2
A solution has 0.05MMg2+ and 0.05MNH3. Calculate the concentration of NH4Cl required to prevent the formation of Mg(OH)2 in this solution. Ksp of Mg(OH)2=9.0×10−12 and ionisation constant of NH3=1.8×10−5
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Q3
A solution has 0.05M−Mg+2 and 0.05M−NH3. Calculate the minimum concentration of NH4Cl required to prevent only precipitation of Mg as Mg(OH)2⋅Ksp of Mg(OH)2=9×10−12 and Kb of NH3=1.8×10−5.
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Q4
A solution has 0.05MMg2+ and 0.05MNH3. Calculate the concentration of NH4Cl required to prevent the formation of Mg(OH)2 in this solution. KspofMg(OH)2=9.0×10−12 and ionization constant of NH3=1.8×10−5
(Given, √1.8=1.34)
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Q5
A solution has $$0.05$$M $$Mg^{2+}$$ and $$0.05$$ M $$NH_3$$. Calculate the concentration of $$NH_4Cl$$ requried to prevent the formation of $$Mg(OH)_2$$ in the solution. $$K_{sp}(Mg(OH)_2)=9.0\times 10^{-12}$$ and $$K_b(NH_3)=1.8\times 10^{-5}$$.