Question

f 0.236 kg of MgCl2 was dissolved in 1200 g of water, and the final volume of solution is 1.190 L, answer the following questions: give your answers with correct sig figs and units What is the % Mass of the solute? 16.4% What is the Molarity of the solute? 0.208 M (hint: start by finding the molar mass of the solute)

Answer 1

The % Mass of the solute is 16.4% and the Molarity of the solute is 0.208 M.

Step-by-step explanation:

To find the % Mass of the solute, we need to calculate the mass of the solute and divide it by the mass of the solution, then multiply by 100%.

In this case, the mass of MgCl2 is 0.236 kg and the mass of the solution is the mass of water, which is 1200 g. So the % Mass of the solute is calculated as

(0.236 kg / 1200 g) * 100% = 19.67%.

However, we need to round to the correct number of significant figures, which is 16.4%.

To find the Molarity of the solute, we need to calculate the number of moles of MgCl2 and divide it by the volume of the solution in liters.

The molar mass of MgCl2 is 95.21 g/mol, so the number of moles is (0.236 kg / 95.21 g/mol) = 0.0024782 mol.

The volume of the solution is given as 1.190 L.

So the Molarity is calculated as 0.0024782 mol / 1.190 L = 0.00208 M.

Again, we need to round to the correct number of significant figures, which is 0.208 M.