Question

Exactly 400.0 ml of 0.650 M magnesium sulfate solution is mixed with exactly 400.0 mL of 0.350 M barium chloride solution. The precipitate forms a compound that has negligible solubility (insoluble). This means that this reaction will form a precipitate (limiting/excess reagent question). Determine the final ionic concentrations. Show ALL work using Chem Type for full

Answer 1

To calculate the concentration of MgSO4 in a mixture using gravimetric analysis, we compute the number of moles of the BaSO4 precipitate, then find the equivalent moles of MgSO4 and calculate the mass percent based on the initial mass of the mixture.

Step-by-step explanation:

The question involves a gravimetric analysis to determine the concentration of magnesium sulfate (MgSO4) in a mixture based on the mass of a resulting precipitate, which is barium sulfate (BaSO4). In this process, MgSO4 is reacted with barium nitrate (Ba(NO3)2) to form the insoluble BaSO4.

To find the mass percent of MgSO4, we would first calculate the number of moles of BaSO4 precipitated and then use stoichiometry to find the moles of MgSO4 originally present. Given that 0.6168 g of BaSO4 is precipitated and the molar mass of BaSO4 is 233.43 g/mol, we can convert this mass to moles.

The stoichiometry of the reaction is 1:1, so the moles of MgSO4 in the mixture will be equal to the moles of BaSO4 formed. Once we know the moles of MgSO4, we can find its mass by multiplying by its molar mass and then determine the mass percent by dividing this mass by the total mass of the mixture and multiplying by 100%.