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(B) The molar concentration of $CH_3COOH$ is $C_1 = \frac{6.00 \ g \ L^{-1}}{60 \ g \ mol^{-1}} = 0.1 \ M$.The molar concentration of $KCl$ is $C_2 =

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$\pi_1 < \pi_2$

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(B) The molar concentration of $CH_3COOH$ is $C_1 = \frac{6.00 \ g \ L^{-1}}{60 \ g \ mol^{-1}} = 0.1 \ M$.The molar concentration of $KCl$ is $C_2 = \frac{7.45 \ g \ L^{-1}}{74.5 \ g \ mol^{-1}} = 0.1 \ M$.The osmotic pressure is given by $\pi = iCRT$,where $i$ is the van't Hoff factor.For $CH_3COOH$ (a weak electrolyte),$i_1 = 1 + \alpha_1$,where $\alpha_1$ is small.For $KCl$ (a strong electrolyte),$i_2 \approx 2$ (since it dissociates into $K^+$ and $Cl^-$).Since $C_1 = C_2$ and $i_2 > i_1$,it follows that $\pi_2 > \pi_1$ or $\pi_1 < \pi_2$.

What is the relationship between the osmotic pressures of $6.00 \ g \ L^{-1}$ $CH_3COOH$ $(\pi_1)$ and $7.45 \ g \ L^{-1}$ $KCl$ $(\pi_2)$ solutions?

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