Chapter 4, Problem 4.11QAP

Describe how you would prepare each solution. 1.00 L of 0.125-M Na2CO3 from solid Na2CO3 500. mL of 0.0215-M KMnO4 from solid KMnO4

Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.

Silver ions can be found in some of the city water piped into homes. The average concentration of silver ions in city water is 0.028 ppm. (a) How many milligrams of silver ions would you ingest daily if you drank eight glasses (eight oz/glass) of city water daily? (b) How many liters of city water are required to recover 1.00 g of silver chemically?

Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?

What mass of oxalic acid, H2C2O4, is required to prepare 250. mL of a solution that has a concentration of 0.15 M H2C2O4?

Insulin is a hormone responsible for the regulation of glucose levels in the blood. An aqueous solution of insulin has an osmotic pressure of 2.5 mm Hg at 25C. It is prepared by dissolving 0.100 g of insulin in enough water to make 125 mL of solution. What is the molar mass of insulin?