The correct increasing order of solubility of the sulphates in water is

Question

The correct increasing order of solubility of the sulphates in water is (A)  textBeS textO text4> text MgS textO text4> text CaS textO text4> text textSrS textO text4 > text BaS textO text4  (B)  textBaS textO text4 text > text SrS textO text4 text > text CaS textO text4 text > text MgS textO text4 text > text BeS textO text4  (C)  textBaS textO text4 text > text CaS textO text4 text > text SrS textO text4 text > text BeS textO text4 text > text MgS textO text4  (D)  textBaS textO text4 text > text SrS textO4> text MgSO text4 text > textCaS textO text4 text ~ text > text BeS textO4

Tardigrade Admin · Accepted Answer

The solubility of the sulphates in water decreases down the group
The high solubilities of

BeS O_{4}

and

MgS O_{4}

are due to the high enthalpy of hydration of the smaller

B e^{2 +}

and

M g^{2 +}

ions, which overcomes the lattice energy factor.

Q. The correct increasing order of solubility of the sulphates in water is

$BeS O_{4} > MgS O_{4} > CaS O_{4} >$ $SrS O_{4}$ $> BaS O_{4}$

$BaS O_{4} > SrS O_{4} > CaS O_{4} > MgS O_{4}$ $> BeS O_{4}$

$BaS O_{4} > CaS O_{4} > SrS O_{4} > BeS O_{4}$ $> MgS O_{4}$

$BaS O_{4} > SrS O_{4} > MgS O_{4} >$ $CaS O_{4}$ $> BeS O_{4}$

The solubility of the sulphates in water decreases down the group
The high solubilities of $BeS O_{4}$ and $MgS O_{4}$ are due to the high enthalpy of hydration of the smaller $B e^{2 +}$ and $M g^{2 +}$ ions, which overcomes the lattice energy factor.

Q. The correct increasing order of solubility of the sulphates in water is

BeSO4​> MgSO4​> CaSO4​> SrSO4​ > BaSO4​

BaSO4​> SrSO4​> CaSO4​> MgSO4​ > BeSO4​

BaSO4​> CaSO4​> SrSO4​> BeSO4​ > MgSO4​

BaSO4​> SrSO4​> MgSO4​> CaSO4​ > BeSO4​

The solubility of the sulphates in water decreases down the group The high solubilities of BeSO4​ and MgSO4​ are due to the high enthalpy of hydration of the smaller Be2+ and Mg2+ ions, which overcomes the lattice energy factor.

$BeS O_{4} > MgS O_{4} > CaS O_{4} >$ $SrS O_{4}$ $> BaS O_{4}$

$BaS O_{4} > SrS O_{4} > CaS O_{4} > MgS O_{4}$ $> BeS O_{4}$

$BaS O_{4} > CaS O_{4} > SrS O_{4} > BeS O_{4}$ $> MgS O_{4}$

$BaS O_{4} > SrS O_{4} > MgS O_{4} >$ $CaS O_{4}$ $> BeS O_{4}$

The solubility of the sulphates in water decreases down the group
The high solubilities of $BeS O_{4}$ and $MgS O_{4}$ are due to the high enthalpy of hydration of the smaller $B e^{2 +}$ and $M g^{2 +}$ ions, which overcomes the lattice energy factor.