The solubility of sulphates in water decreases down the group. The magnitude of the lattic enthalpy remains almost constant as the sulphate ion is so big that small increases in size of cation from $\mathrm{Be}$ to $\mathrm{Ba}$ does not make any difference, The hydration enthalpy decreases from $\mathrm{Be}^{2+}$ to $\mathrm{Ba}^{2+}$ as the size of the cation increases down the group. Hence, the solubility of sulphates of alkaline earth metal decreases down the group mainly due to decreasing hydration enthalpy from $\mathrm{Be}^{2+}$ to $\mathrm{Ba}^{2+}$. The decreasing order of solubility would be ${ }^{-}$ $\mathrm{BeSO}_4>\mathrm{MgSO}_4>\mathrm{CaSO}_4>\mathrm{SrSO}_4>\mathrm{BaSO}_4$
WB- JEE-2016
Ionic Equilibrium
229478
Solubility of which among the following solids in water changes slightly with temperature?
1 $\mathrm{KNO}_3$
2 $\mathrm{NaNO}_3$
3 $\mathrm{KBr}$
4 $\mathrm{NaBr}$
Explanation:
The solubility of $\mathrm{NaBr}$ changes slightly with temperature.
MHT CET-2017
Ionic Equilibrium
229359
The ionic product of water $\left[\mathrm{H}^{+}\right][\mathrm{OH}]$ is
1 $10^{-11}$
2 $10^{-12}$
3 $10^{-5}$
4 $10^{-14}$
Explanation:
The product of concentration of $\mathrm{H}^{+}$and $\mathrm{OH}^{-}$ ions in water at a particular temperature is known as ionic product of water. The ionic product of water is $10^{-14}$.
AIMMS- 25.05.2019
Ionic Equilibrium
229364
Among the following, which is water insoluble?
1 Sodium fluoride
2 Potassium fluoride
3 Beryllium fluoride
4 Magnesium fluoride
Explanation:
The solubility of the fluorides is based on the lattice energy released when there is more attraction and more is the charge density. Magnesium fluoride $\left(\mathrm{MgF}_2\right)$ is water insoluble because of the fluorides of alkaline earth metal are insoluble in water and beryllium fluoride is slightly soluble in water.
The solubility of sulphates in water decreases down the group. The magnitude of the lattic enthalpy remains almost constant as the sulphate ion is so big that small increases in size of cation from $\mathrm{Be}$ to $\mathrm{Ba}$ does not make any difference, The hydration enthalpy decreases from $\mathrm{Be}^{2+}$ to $\mathrm{Ba}^{2+}$ as the size of the cation increases down the group. Hence, the solubility of sulphates of alkaline earth metal decreases down the group mainly due to decreasing hydration enthalpy from $\mathrm{Be}^{2+}$ to $\mathrm{Ba}^{2+}$. The decreasing order of solubility would be ${ }^{-}$ $\mathrm{BeSO}_4>\mathrm{MgSO}_4>\mathrm{CaSO}_4>\mathrm{SrSO}_4>\mathrm{BaSO}_4$
WB- JEE-2016
Ionic Equilibrium
229478
Solubility of which among the following solids in water changes slightly with temperature?
1 $\mathrm{KNO}_3$
2 $\mathrm{NaNO}_3$
3 $\mathrm{KBr}$
4 $\mathrm{NaBr}$
Explanation:
The solubility of $\mathrm{NaBr}$ changes slightly with temperature.
MHT CET-2017
Ionic Equilibrium
229359
The ionic product of water $\left[\mathrm{H}^{+}\right][\mathrm{OH}]$ is
1 $10^{-11}$
2 $10^{-12}$
3 $10^{-5}$
4 $10^{-14}$
Explanation:
The product of concentration of $\mathrm{H}^{+}$and $\mathrm{OH}^{-}$ ions in water at a particular temperature is known as ionic product of water. The ionic product of water is $10^{-14}$.
AIMMS- 25.05.2019
Ionic Equilibrium
229364
Among the following, which is water insoluble?
1 Sodium fluoride
2 Potassium fluoride
3 Beryllium fluoride
4 Magnesium fluoride
Explanation:
The solubility of the fluorides is based on the lattice energy released when there is more attraction and more is the charge density. Magnesium fluoride $\left(\mathrm{MgF}_2\right)$ is water insoluble because of the fluorides of alkaline earth metal are insoluble in water and beryllium fluoride is slightly soluble in water.
The solubility of sulphates in water decreases down the group. The magnitude of the lattic enthalpy remains almost constant as the sulphate ion is so big that small increases in size of cation from $\mathrm{Be}$ to $\mathrm{Ba}$ does not make any difference, The hydration enthalpy decreases from $\mathrm{Be}^{2+}$ to $\mathrm{Ba}^{2+}$ as the size of the cation increases down the group. Hence, the solubility of sulphates of alkaline earth metal decreases down the group mainly due to decreasing hydration enthalpy from $\mathrm{Be}^{2+}$ to $\mathrm{Ba}^{2+}$. The decreasing order of solubility would be ${ }^{-}$ $\mathrm{BeSO}_4>\mathrm{MgSO}_4>\mathrm{CaSO}_4>\mathrm{SrSO}_4>\mathrm{BaSO}_4$
WB- JEE-2016
Ionic Equilibrium
229478
Solubility of which among the following solids in water changes slightly with temperature?
1 $\mathrm{KNO}_3$
2 $\mathrm{NaNO}_3$
3 $\mathrm{KBr}$
4 $\mathrm{NaBr}$
Explanation:
The solubility of $\mathrm{NaBr}$ changes slightly with temperature.
MHT CET-2017
Ionic Equilibrium
229359
The ionic product of water $\left[\mathrm{H}^{+}\right][\mathrm{OH}]$ is
1 $10^{-11}$
2 $10^{-12}$
3 $10^{-5}$
4 $10^{-14}$
Explanation:
The product of concentration of $\mathrm{H}^{+}$and $\mathrm{OH}^{-}$ ions in water at a particular temperature is known as ionic product of water. The ionic product of water is $10^{-14}$.
AIMMS- 25.05.2019
Ionic Equilibrium
229364
Among the following, which is water insoluble?
1 Sodium fluoride
2 Potassium fluoride
3 Beryllium fluoride
4 Magnesium fluoride
Explanation:
The solubility of the fluorides is based on the lattice energy released when there is more attraction and more is the charge density. Magnesium fluoride $\left(\mathrm{MgF}_2\right)$ is water insoluble because of the fluorides of alkaline earth metal are insoluble in water and beryllium fluoride is slightly soluble in water.
The solubility of sulphates in water decreases down the group. The magnitude of the lattic enthalpy remains almost constant as the sulphate ion is so big that small increases in size of cation from $\mathrm{Be}$ to $\mathrm{Ba}$ does not make any difference, The hydration enthalpy decreases from $\mathrm{Be}^{2+}$ to $\mathrm{Ba}^{2+}$ as the size of the cation increases down the group. Hence, the solubility of sulphates of alkaline earth metal decreases down the group mainly due to decreasing hydration enthalpy from $\mathrm{Be}^{2+}$ to $\mathrm{Ba}^{2+}$. The decreasing order of solubility would be ${ }^{-}$ $\mathrm{BeSO}_4>\mathrm{MgSO}_4>\mathrm{CaSO}_4>\mathrm{SrSO}_4>\mathrm{BaSO}_4$
WB- JEE-2016
Ionic Equilibrium
229478
Solubility of which among the following solids in water changes slightly with temperature?
1 $\mathrm{KNO}_3$
2 $\mathrm{NaNO}_3$
3 $\mathrm{KBr}$
4 $\mathrm{NaBr}$
Explanation:
The solubility of $\mathrm{NaBr}$ changes slightly with temperature.
MHT CET-2017
Ionic Equilibrium
229359
The ionic product of water $\left[\mathrm{H}^{+}\right][\mathrm{OH}]$ is
1 $10^{-11}$
2 $10^{-12}$
3 $10^{-5}$
4 $10^{-14}$
Explanation:
The product of concentration of $\mathrm{H}^{+}$and $\mathrm{OH}^{-}$ ions in water at a particular temperature is known as ionic product of water. The ionic product of water is $10^{-14}$.
AIMMS- 25.05.2019
Ionic Equilibrium
229364
Among the following, which is water insoluble?
1 Sodium fluoride
2 Potassium fluoride
3 Beryllium fluoride
4 Magnesium fluoride
Explanation:
The solubility of the fluorides is based on the lattice energy released when there is more attraction and more is the charge density. Magnesium fluoride $\left(\mathrm{MgF}_2\right)$ is water insoluble because of the fluorides of alkaline earth metal are insoluble in water and beryllium fluoride is slightly soluble in water.
