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Chemistry
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11 Dec 2019

Given that molecular weight of ZnSO4*7H2O is 287.53 g/mol, calculate

1) the mass of ZnSO4*7H2O to give 200mL of 0.04M solution

2) When 3.8357g of ZnSO4*7H2O is used, what is the molarity of ZnSO4 solution

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Related questions

PLEASE SHOW WORK--- WILL RATE :)

  1. Predict how the Ecell for the copper/zinccell in part 1 would change (increase, decrease, or remain thesame) if:

**Part 1 cell: Cu (s) in 0.1 M CuSO4(aq) and Zn (s) in 0.1 M ZnSO4(aq)

a. The concentration of the anode solution was changedto 1 M.

b. The concentrations of the cathode solution werechanged to 1 M.

c. A larger piece of metal was used.

2. Calculate the Ecell for the copperconcentration cell in part 2 if 0.01 M CuSO4 was usedinstead of 0.1 M CuSO4.

**Cu concentration cell: Cu (s) in 0.1 MCuSO4 (aq) and Cu (s) in 1 M ZnSO4(aq)

What mass of Zn(s) is required in order to completely precipitate the mass of Cu 2+ ions produced in the reaction CuSO4 +Zn --> Cu +ZnSO4. Why is more zinc used? Why might it be necessary to add more zinc than that?

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