Question

A solution is made by dissolving 17.3 g of magnesium nitrate in water to a final volume of 475 mL solution. What is the wight?

Answer 1

The mass percent of MgSO4 in the mixture can be determined by calculating the moles of precipitated BaSO4, finding the corresponding mass of MgSO4, and then dividing by the total mass of the mixture to get the percentage.

Step-by-step explanation:

To determine the mass percent of MgSO4 in the given mixture, we must relate the mass of the precipitated BaSO4 back to the original MgSO4. We can do this because the stoichiometry of the reaction dictates that one mole of MgSO4 will produce one mole of BaSO4. First, calculate the number of moles of BaSO4 from its mass using its molar mass, then using this information, find the mass of MgSO4 that would have been present to form that amount of BaSO4. The mass percent of MgSO4 is then found by taking the calculated mass of MgSO4 and dividing it by the total mass of the mixture, then multiplying by 100 to get a percentage.

Answer 2

The solution weighs 17.775 grams.

This weight is determined by considering the mass of magnesium nitrate (the solute) dissolved in a specific amount of water (the solvent).

To find this weight, we look at the mass of magnesium nitrate, given as 17.3 grams, and the final volume of the solution, which is 475 milliliters.

To calculate the solution's weight, we convert the volume from milliliters to grams using the density of water (1 g/mL).

First, we convert 475 mL to liters, resulting in 0.475 L. Then, by using the density, we find the mass of the water to be 0.475 grams.

Finally, we determine the total weight of the solution by adding the mass of magnesium nitrate to the mass of the water: 17.3 g + 0.475 g, which equals the overall weight of the solution as 17.775 grams.