5) The density of a 2.45 M aqueous solution of methanol (CH3OH) is 0.976 g/mL. What is the molality of the solution? The molar mass of methanol is 32.04 g. 6) Calculate the molality of a 35.4 percent (by mass) aqueous solution of phosphoric acid (H3PO4 ). The molar mass of phosphoric acid is 97.99 g 7) A solution containing 53 g of sodium carbonate (mol mass = 106) in 1 Kg water at 20°C. The density of the solution at this temperature is 1.1 g/ml. Determine for the solution. 1) the mole fraction of each component 1) the mass percent 2) the molarity 3) the molality 4) the normality

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5) The density of a 2.45 M aqueous solution
of methanol (CH3OH) is 0.976 g/mL. What
is the molality of the solution? The molar
mass of methanol is 32.04 g. 6) Calculate
the molality of a 35.4 percent (by mass)
aqueous solution of phosphoric acid
(H3PO4 ). The molar mass of phosphoric
acid is 97.99 g 7) A solution containing 53 g
of sodium carbonate (mol mass = 106) in 1
Kg water at 20°C. The density of the
solution at this temperature is 1.1 g/ml.
Determine for the solution. 1) the mole
fraction of each component 1) the mass
percent 2) the molarity 3) the molality 4) the
normality
Transcribed Image Text:5) The density of a 2.45 M aqueous solution of methanol (CH3OH) is 0.976 g/mL. What is the molality of the solution? The molar mass of methanol is 32.04 g. 6) Calculate the molality of a 35.4 percent (by mass) aqueous solution of phosphoric acid (H3PO4 ). The molar mass of phosphoric acid is 97.99 g 7) A solution containing 53 g of sodium carbonate (mol mass = 106) in 1 Kg water at 20°C. The density of the solution at this temperature is 1.1 g/ml. Determine for the solution. 1) the mole fraction of each component 1) the mass percent 2) the molarity 3) the molality 4) the normality
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