Question

A metallurgical firm wishes to dispose of 1200 gallons of waste sulfuric acid whose molarity is 1.05 M. Before disposal, it will be reacted with calcium hydroxide (slaked lime), which costs $0.25 per pound. Write the balanced chemical equation for this process. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) Determine the cost that the firm will incur from this use of slaked lime. Cost

Answer 1

Answer:

The balanced chemical equation for this process:

$H_2SO_4(aq)+Ca(OH)_2(s)\rightarrow 2H_2O(l)+CaSO_4(aq)$

$194.51 is the cost that the firm will incur from this use of slaked lime.

Explanation:

The balanced chemical equation for this process

$H_2SO_4(aq)+Ca(OH)_2(s)\rightarrow 2H_2O(l)+CaSO_4(aq)$

Moles of sulfuric acid = n

Volume of sulfuric acid disposed = V = 1200 gallons = 3.785 × 1200 L = 4,542 L

1 gallon = 3.785 Liter

Morality of the sulfuric acid = M = 1.05 m

$Molarity(M)=\frac{n}{V(L)}$

$n=m\times V=1.05 M\times 4,542 L=4,769.1 mol$

According to reaction, 1 mol of sulfuric acid reacts with 1 mole of calcium hydroxide.Then 4,769.1 moles of sulfuric acid will recat with ;

$\frac{1}{1}\times 4,769.1 mol=4,769.1 mol$ of calcium hydroxide

Mass of 4,769.1 moles of calcium hydroxide:

4,769.1 mol  74 g/mol = 352,913.4 g

= $\frac{352,913.4 }{453.6} pounds =778.03 pounds$

(1 pound = 453.6 grams)

Cost of 1 pound of slaked lime  = $0.25

Cost of 778.03 pounds of slaked lime  = $0.25 × 778.03 = $194.51

$194.51 is the cost that the firm will incur from this use of slaked lime.