Consider separate solutions of 0.500 , M , C_ | vedclass

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(A) The osmotic pressure $\pi$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas c

Vedclass · Accepted Answer

They all have the same osmotic pressure.

Vedclass · Answer

(A) The osmotic pressure $\pi$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature.For $C_2H_5OH$ (non-electrolyte): $i = 1$,$\pi = 1 	imes 0.500 	imes RT = 0.500 RT$.For $Mg_3(PO_4)_2$ (dissociates into $3Mg^{2+} + 2PO_4^{3-}$,so $i = 5$): $\pi = 5 	imes 0.100 	imes RT = 0.500 RT$.For $KBr$ (dissociates into $K^+ + Br^-$,so $i = 2$): $\pi = 2 	imes 0.250 	imes RT = 0.500 RT$.For $Na_3PO_4$ (dissociates into $3Na^+ + PO_4^{3-}$,so $i = 4$): $\pi = 4 	imes 0.125 	imes RT = 0.500 RT$.Since the osmotic pressure of all the given solutions is equal,they are isotonic.

Consider separate solutions of $0.500 \, M \, C_2H_5OH \, (aq)$,$0.100 \, M \, Mg_3(PO_4)_2 \, (aq)$,$0.250 \, M \, KBr \, (aq)$ and $0.125 \, M \, Na_3PO_4 \, (aq)$ at $25 ^\circ C$. Which statement is true about these solutions,assuming all salts to be strong electrolytes?

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