Water draining from abandoned mines on Iron Mountain in California is extremely

Question

Water draining from abandoned mines on Iron Mountain in California is extremely acidic and leaches iron, zinc, and other metals from the underlying rock (Figure P4.132). One liter of drainage contains as much as 80.0 g of dissolved iron and 6 g of zinc.

a.

Calculate the molarity of iron and of zinc in the drainage.

b

One source of the dissolved iron is the reaction between water containing H2SO4 and solid Fe(OH)3. Complete the following chemical equation, and write a net ionic equation for the process.

2 Fe(OH)3(s) + 3 H2SO4(aq) ?

c.

Sources of zinc include the mineral smithsonite, ZnCO3. Write a balanced net ionic equation for the reaction between smithsonite and H2SO4 that produces Zn2+(aq).

a.

Calculate the molarity of iron and of zinc in the drainage.

b

One source of the dissolved iron is the reaction between water containing H2SO4 and solid Fe(OH)3. Complete the following chemical equation, and write a net ionic equation for the process.

2 Fe(OH)3(s) + 3 H2SO4(aq) ?

c.

Sources of zinc include the mineral smithsonite, ZnCO3. Write a balanced net ionic equation for the reaction between smithsonite and H2SO4 that produces Zn2+(aq).

Explanation / Answer

a.

Mass of Fe = 80 g
Molar mass of Fe = 56 g/mol
So, 56 g of Fe = 1 mol
or, 1 g of Fe = (1/56) mol
or, 80 g of Fe = (80/56) mol = 1.43 mol

Volume = 1 L

So, molarity of Fe = 1.43 mol / 1 L = 1.43 M

Mass of Zn = 65.5 g
Molar mass of Zn = 65.5 g/mol
So, 65.5 g of Zn = 1 mol
or, 1 g of Zn = (1/65.5) mol
or, 6 g of Zn = (6/65.5) mol = 0.09 mol

Volume = 1 L

So, molarity of Zn = 0.09 mol / 1 L = 0.09 M

(b)

The balanced equation is

2Fe(OH)3(s) + 3H2SO4(aq) --> Fe2(SO4)3 (aq) + 6H2O (l)

(c) No question given.

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