The solubility (S) of a solute in water varies with temperature as given by S=Ae- Δ H / R T,Δ H being the enthalpy of solution. For a given solute, variation of lnS with temperature is as shown in figure. The solute is expected to be

Question

The solubility (S) of a solute in water varies with temperature as given by S=Ae- Δ H / R T,Δ H being the enthalpy of solution. For a given solute, variation of lnS with temperature is as shown in figure. The solute is expected to be <img class="img-fluid question-image" alt="Question" src="https://cdn.tardigrade.in/q/nta/c-aa1tfheqlkl5eain.jpg" /> (A)  textCaO (B) MgSO4 (C) CuSO4 (D) CuSO4.5H2O

Tardigrade Admin · Accepted Answer

textlnS text= textlnA - ( textÎH/ textRT) textSlope text= (- textÎH/ textRT) textlnS textvs ( text1/ textT) graph with negative slope. So, Δ H>0 Salts with water of crystallisation. i.e., CuSO4.5H2O .

Q. The solubility (S) of a solute in water varies with temperature as given by $S = A e^{- Δ H / RT}, Δ H$ being the enthalpy of solution. For a given solute, variation of lnS with temperature is as shown in figure. The solute is expected to be

$CaO$

$M g S O_{4}$

$C u S O_{4}$

$C u S O_{4} .5 H_{2} O$

$lnS = lnA - \frac{ΔH}{RT}$
$Slope = \frac{- ΔH}{RT}$
$lnS vs \frac{1}{T}$ graph with negative slope.
So, $Δ H > 0$
Salts with water of crystallisation.
i.e., $C u S O_{4} .5 H_{2} O$ .

Q. The solubility (S) of a solute in water varies with temperature as given by S=Ae−ΔH/RT,ΔH being the enthalpy of solution. For a given solute, variation of lnS with temperature is as shown in figure. The solute is expected to be

CaO

MgSO4​

CuSO4​

CuSO4​.5H2​O