An aqueous solution contains the amino acid glycine (NH2CH2COOH). Assuming that the acid does not ionize in water, calculate the molality, in molal, of the solution if it freezes at - 4.13 °C. (Cryoscopic constant of water: 1.86 °C/molal; Atomic Weight: N = 14.01 g/mol; H = 1.008 g/mol; C = 12.01 g/mol; O = 16.00 g/mol; density of water = 1.00 g/mL). Express your answer in three decimal places only. Do not put the units.
An aqueous solution contains the amino acid glycine (NH2CH2COOH). Assuming that the acid does not ionize in water, calculate the molality, in molal, of the solution if it freezes at - 4.13 °C. (Cryoscopic constant of water: 1.86 °C/molal; Atomic Weight: N = 14.01 g/mol; H = 1.008 g/mol; C = 12.01 g/mol; O = 16.00 g/mol; density of water = 1.00 g/mL). Express your answer in three decimal places only. Do not put the units.
Chemistry & Chemical Reactivity
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ISBN:9781337399074
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Chapter13: Solutions And Their Behavior
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Problem 12PS: Silver ion has an average concentration of 28 ppb (parts per billion) in U.S. water supplies. (a)...
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An aqueous solution contains the amino acid glycine (NH2CH2COOH). Assuming that the acid does not ionize in water, calculate the molality, in molal, of the solution if it freezes at - 4.13 °C. (Cryoscopic constant of water: 1.86 °C/molal; Atomic Weight: N = 14.01 g/mol; H = 1.008 g/mol; C = 12.01 g/mol; O = 16.00 g/mol; density of water = 1.00 g/mL). Express your answer in three decimal places only. Do not put the units.
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