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veena
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Homework Statement
Solid Magnesium sulphate exists only as a mono hydrate . Calculate the mass of this solute in 500 mL of the stock MnSo4 used in this experiment.
Homework Equations
Plz help
To calculate the mass of magnesium sulphate in a 500 mL stock solution of MnSo4, you will need to know the concentration of the stock solution and the molar mass of magnesium sulphate. The formula for calculating mass is: mass = concentration (mol/L) x volume (L) x molar mass (g/mol). Simply plug in the values and calculate the mass.
The molar mass of magnesium sulphate is 120.37 g/mol. This can be found by adding the atomic masses of each element in the compound (Mg = 24.31 g/mol, S = 32.06 g/mol, O = 16.00 g/mol) multiplied by their respective subscripts in the chemical formula (MgSO4).
To convert mL to L, you simply divide the volume in mL by 1000. In this case, the volume is 500 mL, so the calculation would be 500 mL / 1000 = 0.5 L.
Calculating the mass of a compound in a stock solution is important because it allows you to know the exact amount of the compound that is present. This is crucial in experiments and chemical reactions, as the amount of a compound can greatly affect the outcome. It also helps in ensuring the correct concentration of the solution is being used.
Yes, the mass of magnesium sulphate in a 500 mL stock solution of MnSo4 can vary depending on the concentration of the stock solution. The higher the concentration, the greater the mass will be. Additionally, human error in measuring and calculating can also affect the final mass. It is important to use accurate measurements and calculations to minimize variation in the mass.