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The density of a solution of 3.69g KBr in 21.70g H2O is 1.11g/mL. Calculate the molarity...

The density of a solution of 3.69g KBr in 21.70g H2O is 1.11g/mL. Calculate the molarity of KBr in the solution 0.94 M 1.49 M 1.10 M 0.99 M 1.56 M 1.36 M

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Answer #1

The density of solution of 3.69g KBt in 21.70g of H2O = 1.11g / mL

The mass of KBr = 3.69 grams

Molecular weight of KBr = 119g / mole

Moles of KBr = MAss / Molecular weight = 3.69 / 119 = 0.0310 moles

Total mass of solution = Mass of KBr + mass of Water = 3.69 + 21.70 = 25.39 grams

Volume of solution = Mass of solution / Density = 25.39 / 1.11 = 22.87 mL = 0.02287 L

Molarity of solution = Moles of solute / Volume of solution in litres = Moles of KBr / Volume

Molarity of solution = 0.0310 / 0.02287 = 1.355 M = 1.36 M


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