Question
An aqueous solution contains the amino acid glycine $\left(\mathrm{NH}_2 \mathrm{CH}_2 \mathrm{COOH}\right)$. Assuming that the acid does not ionize in water, calculate the molality of the solution if it freezes at $-1.1^{\circ} \mathrm{C}$.
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An aqueous solution contains the amino acid glycine $\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{COOH}\right) .$ Assuming that the acid does not ionize in water, calculate the molality of the solution if it freezes at $-1.1^{\circ} \mathrm{C}$.
An aqueous solution contains the amino acid glycine $\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{COOH}\right) .$ Assuming that the acid does not ionize in water, calculate the molality of the solution if it freezes at $-1.1^{\circ} \mathrm{C}$
An aqueous solution contains the amino acid glycine $\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{COOH}\right)$. Assuming no ionization of the acid, calculate the molality of the solution if it freezes at $-1.1^{\circ} \mathrm{C}$.
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