Calculate the molarity of a solution containing 15 mg of CuS04 × 5H20 in 1.00 L of solution. (6 pts)
MY ANSWER
15 mg = 0.015 g. And the molar mass is 249.72 g / mol. So then we do 0.015 / 249.72 x1.00 =
0 00006007 mol L.
or 6.01 x10^-5 mol I
6. Explain in words how you would prepare 1.00 L of a 15 mg L solution of CuS04 x 5H2O (5 pts)
(HELP ME WITH THIS PLEASE!)
Weigh 15 mg CuSO4.5H2O, transfer to a 1 L volumetric flask, add some distilled water, swirl to dissolve all of the solid, add distilled water to the mark of the volumetric flask, stopper, mix thoroughly, label, done. Your calculations are correct.
Thank you so much
To prepare a 1.00 L solution of CuSO4 × 5H2O with a concentration of 15 mg/L, you need to follow these steps:
1. Determine the molar mass of CuSO4 × 5H2O. CuSO4 has a molar mass of 159.61 g/mol, and 5H2O has a molar mass of 90.09 g/mol. Adding them together gives a total molar mass of 249.72 g/mol.
2. Convert the desired concentration from mg/L to g/L. Since 1 g = 1000 mg, 15 mg/L is equivalent to 0.015 g/L.
3. Use the molar mass calculated in step 1 to convert the mass from step 2 to moles. Divide the mass (0.015 g) by the molar mass (249.72 g/mol). This gives you 6.006 x 10^-5 mol/L.
4. Finally, to prepare the 1.00 L solution, dissolve 6.006 x 10^-5 mol of CuSO4 × 5H2O in enough solvent to make a total volume of 1.00 L.
Note: It is important to accurately measure the mass of CuSO4 × 5H2O and the volume of the solvent to ensure the concentration and volume of the prepared solution are correct.