For each of the following problems, show calculations and write legibly with cor

ID: 538583 • Letter: F

Question

For each of the following problems, show calculations and write legibly with correct spelling, punctuation, and use of chemical symbols and terminology for full credit. Our stomachs contain hydrochloric acid, which aids digestion of food. Some people experience over production of acid, leading to heartburn and other more serious conditions such as acid reflux disease. The base magnesium hydroxide is sold as an antacid, which reacts with the excess acid in an acid-base or neutralization reaction. What mass of hydrochloric acid can be neutralized by 1.00 grams of magnesium hydroxide? After several months, a nail dropped on the floor of a garage rusts completely. The nail is made of pure iron and weighs 0.57 grams. What is the mass of the rust produced from this reaction? Assume the rust that forms is pure iron (III) oxide.

Explanation / Answer

1) the reaction of acid with Mg(OH)2 will be

2HCl + Mg(OH)2 ---> MgCl2 + 2H2O

Hence as shown above in the equation

one mole of Mg(OH)2 will neutralize two moles of HCl

Moles of Mg(OH)2 taken = Mass of Mg(OH)2 / Molecular weight of Mg(OH)2

Molecular weight of Mg(OH)2 = 24 + 2 X 16 + 2X1 = 58 g / mole

Moles of Mg(OH)2 = 1 g / 58 g /mole = 0.0172 moles

so moles of HCl which can be neutralized = 2X 0.0172 moles = 0.0344 moles

Mass of HCl which can be neutralized = Moles X moelcular weight of HCl

Molecular weight of HCl = 1 + 35. 5 = 36.5 g / mole

Mass of HCl which can be neutralized = 0.0344 X 36.5 = 1.256 grams

2) the rust formed is pure iron oxide , so the moelcular formula = Fe2O3

the reaction of rusting will be

2Fe(s) + 3/2O2 --> Fe2O3

Therefore two moles of Fe will give one mole of Fe2O3

Initial moles of Fe(s) in nail = Mass of Nail / atomic weight of Fe = 0.57 / 55.8 g /mole = 0.0102 moles

Moles of Fe2O3 produced = 0.0102 / 2 moles = 0.0051 moles

Mass of Fe2O3 = Moles X molecular weight of Fe2O3

molecular weight of Fe2O3 = 2X 55.8 + 3 X 16 = 159.6 g / moles

Mass of Fe2O3 = 0.0051 X 159.6 = 0.814 grams [The mass of rust produced]

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