Assignment:
Chemical XYZ is added to a substrate at a defined rate of 1.17% of the dry weight of the substrate; paper makers alum (Al2(SO4)3-14H2O) is added to the substrate at a rate of 45% of the Chemical XYZ rate; the dry weight of the substrate is given as 1460 lbs/1000 ft2
The molecular weight of the alum is given as:
2 x Al = 54 g/mol }
3 x S = 96 g/mol } 594 g/mol total
28 x H = 28 g/mol }
26 x O = 416 g/mol }
Assuming 100% retention of the alum, what is the weight % Al+3 present in the substrate after alum addition and convert the weight % of Al+3 to ppm:
However, if in reality, the solubility of the alum is given as 87 g/100 cc's and we assumed a 10 liter solution of water, and the preceding masses of material were present or added to the 10 liter water solution (e.g. 1.465 lbs of "stuff"; .01714 lbs of XYZ; and .007713 lbs alum):
How would we then determine how much Al+3 actually dissolved? What is the dissolved and un-dissolved weight fraction of Al+3 present in the solution? And, what would the equivalent ppm value of the Al+3 (dissolved & un-dissolved) be as a function of the total solution?
Provide complete and step by step solution for the question and show calculations and use formulas.