A sample of barium nitrate is placed into a jar containing water. The mass of the barium nitrate sample is 27g. Assume the water
2 answers:
<u>Answer:</u> The mass of water present in the jar is 297.7 grams.
<u>Explanation:</u>
We are given:
Mass of barium nitrate sample = 27 g
Solubility is defined as the maximum amount of solute that can be dissolved in a solvent at equilibrium.
The solubility of barium nitrate at 20°C is 9.02 g per 100 g of water
To calculate the mass of solution in which given amount of barium nitrate is dissolved, we apply unitary method:
9.02 g of barium nitrate is dissolved in 100 g of water
So, 27 g of barium nitrate will be dissolved in of water
Hence, the mass of water present in the jar is 297.7 grams.
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<u>Answer:</u> The freezing point of solution is -117.54°C and the boiling point of solution is 80.48°C
<u>Explanation:</u>
To calculate the mass of ethanol, we use the equation:
Density of ethanol = 0.789 g/mL
Volume of ethanol = 96.3 mL
Putting values in above equation, we get:
- <u>Calculating the freezing point:</u>
Depression in freezing point is defined as the difference in the freezing point of pure solution and freezing point of solution.
The equation used to calculate depression in freezing point follows:
To calculate the depression in freezing point, we use the equation:
Or,
where,
Freezing point of pure solution = -114.1 °C
i = Vant hoff factor = 1 (For non-electrolytes)
= molal freezing point elevation constant = 1.99°C/m
= Given mass of solute (ethylene glycol) = 8.15 g
= Molar mass of solute (ethylene glycol) = 62 g/mol
= Mass of solvent (ethanol) = 75.98 g
Putting values in above equation, we get:
Hence, the freezing point of solution is -117.54°C
- <u>Calculating the boiling point:</u>
Elevation in boiling point is defined as the difference in the boiling point of solution and freezing point of pure solution.
The equation used to calculate elevation in boiling point follows:
To calculate the elevation in boiling point, we use the equation:
Or,
where,
Boiling point of pure solution = 78.4°C
i = Vant hoff factor = 1 (For non-electrolytes)
= molal boiling point elevation constant = 1.20°C/m.g
= Given mass of solute (ethylene glycol) = 8.15 g
= Molar mass of solute (ethylene glycol) = 62 g/mol
= Mass of solvent (ethanol) = 75.98 g
Putting values in above equation, we get:
Hence, the boiling point of solution is 80.48°C