[macbookloser]

Scenario 3:
In small amounts (1 ppm = 1 mg/L) copper (ii) ions are used as an algaecide in swimming
pools.   Blue Water Pool Treatments                                                             (BWPT), a producer of algaecide and other pool
chemicals, recently had an incident at one of their manufacturing plants; someone added too
much copper sulphate to the product mixture, resulting in an algaecide that is more
concentrated than the labelling (and usage instructions) indicate. The remedy of course is to
dilute the product mixture, but to do so, BWPT must first determine the current     



questions:
1. Flow much Cu2+ ion is present in the test solution in moles/L
2. The labelling on the product bottle gives the instruction to use 1 mL of product per L of
pool water'. Using this ratio, calculate the concentration of Cu2+ that the product must
have to achieve the desired 1 ppm Cu2+.

answer for question one is 0.05679 mol/l

[chenbeier]

1 ppm Cu²⁺ = 1 mg/l = 0,0635 mol/l

If the solution contain 0,05679 mol/l then it is less and not to much.

What mean mol/12?

[macbookloser]

oh it was a typo. How did you get 0,0635 mol/l?

I understand 1 ppm Cu2+ = 1 mg/l

did you use the molar mass of copper sulphate ?

[chenbeier]

Sorry there is a calculation error by me

It has to be 0,001 g /l / 63,5 g/ mol = 1,57 *10^-5 mol/l

[macbookloser]

oh thanks . I understand now. You used the atomic weight. Thank you so much!!