when 0.102 g of an unknown compound was dissolved in 100 ml of water on osmotic

Question

when 0.102 g of an unknown compound was dissolved in 100 ml of water on osmotic pressure of 28.1 torr was measured at 20 Celsius. calculate molar mass of the compound when 0.102 g of an unknown compound was dissolved in 100 ml of water on osmotic pressure of 28.1 torr was measured at 20 Celsius. calculate molar mass of the compound when 0.102 g of an unknown compound was dissolved in 100 ml of water on osmotic pressure of 28.1 torr was measured at 20 Celsius. calculate molar mass of the compound

Explanation / Answer

we have to use the formula    = i M R T

i is the van 't Hoff factor

M is the molarity

R= 62.36367 LmmHgK1mol1 is the gas constant

T is the thermodynamic (absolute) temperature = 20+273 = 293K

from the above the equation

M = /iRT

M = 28.1/1x62.363x293

M = 0.00153784 moles/liter

we also have 0.102 g in 100 mL or

0.102 g / .1000 L = 1.02 g per liter

we in 1 liter have 1.02 g of solute = 0.001466 moles

mass of 1 mole = 1.02 g / 0.001537842 mol = 663g / mole .. molar mass of the compound

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