Formulas (CIE A Level Chemistry)

Cobalt(II) sulfate is used in storage batteries, electroplating baths and as an additive to soils and animal feeds.

A sample of hydrated cobalt sulfate, CoSO₄•xH₂O, has a relative formula mass of 173.0.

Calculate a value for 'x'.

A student completed an experiment to determine the value of ‘x’ in a hydrated salt.

They heated a solid sample of the salt, CoSO₄.xH₂O, in a crucible for 60 seconds and recorded the following set of results.

Use the data obtained by the student in Table 2.1 to calculate a value for ‘x’.

The actual value for x in CoSO₄.xH₂O is 6.

Cobalt(II) sulfate undergoes a displacement reaction with magnesium because magnesium is a more reactive metal than cobalt.

Write an ionic equation for this reaction. State symbols are not required.

Chevreul's salt or copper(I, II) sulfite dihydrate, Cu₃(SO₃)₂•2H₂O, is an unusual hydrated salt as it contains copper in both of its common oxidation states.

The first step in the formation of Chevreul's salt is the reaction of aqueous copper sulfate with a solution of potassium metabisulfite, K₂S₂O₅.

Balance the equation for the reaction to form the anhydrous Chevreul's salt.

The chemical formula of Chevreul's salt is sometimes written as Cu₂SO₃•CuSO₃•2H₂O to show that it contains copper(I) sulfite and copper(II) sulfite.

Calculate the percentage by mass of copper(I) ions in copper(I) sulfite

Show your working.

Chevreul's salt can react with ammonia solution to form a deep blue solution of the tetraamminecopper(II) complex, [Cu(NH₃)₄]²⁺ (aq). It can also react with hydrochloric acid to form a white solid of copper(I) chloride, water and sulfur dioxide.

Write an ionic equation for the formation of copper(I) chloride from Chevreul's salt. State symbols are not required.

When Chevreul's salt is heated in an inert atmosphere, it is stable to around 200 ^oC. Above this temperature, a variety of compounds can be produced although the final product of sustained heating at high temperatures is copper(II) oxide.

During the heating process, a sample of the mixture is taken. After separation, the most common compound was analysed and found to contain 39.8% copper, 20.1% sulfur and the rest oxygen.

Calculate the empirical formula of the most common compound. Show your working.

A synthetic carbohydrate was isotopically labelled with carbon-13.

Analysis of a 12 g sample of the carbohydrate found it to contain 6.93 g carbon, 0.80 g hydrogen and the remainder was oxygen.

Determine the empirical formulae of the carbohydrate.

The fermentation of glucose, C₆H₁₂O₆, is one method scientists can use to produce ethanol.  

Write a balanced symbol equation for this reaction. 

During the fermentation process in the reaction in part (b), 312 g of ethanol was produced from 1.5 kg of glucose. 

Calculate the percentage yield of this reaction to 1 decimal place. If you were unable to produce an equation for part (b), assume that 1 mole of glucose would produce 4 moles of ethanol for this question (this is not the correct molar ratio). 

Magnesium carbonate is a common antacid that is used to react with and neutralise excess stomach acid, HCl. 

MgCO₃ (s) + 2HCl (aq) MgCl₂ (aq) + CO₂ (g) + H₂O (l)

The total mass of the reactants is 9.91 g.

Calculate the volume of carbon dioxide that is produced at room temperature and pressure.

Another magnesium salt, magnesium sulfate, can exist in hydrated or anhydrous forms.

6.31 g of a sample of magnesium sulphate, MgSO₄.xH₂O, was strongly heated until a mass of 3.61 g of solid remained with no further change in mass recorded.

Calculate the number of moles of water of crystallisation, x, in the magnesium sulphate sample.

moles of water = ..................... mol

Another sample of hydrated magnesium sulphate, MgSO₄.xH₂O, is found to contain 51.1% water by mass.

Calculate the number of moles of water of crystallisation, x, in this sample.

moles of water = ..................... mol

Describe the effect on the value of x obtained if the salt was not heated strongly to a constant mass.

The coca-cola company states that a 12 oz can of coke contains 34 mg of caffeine, M_r = 194.19 g mol^-1.

Calculate the number of moles of caffeine in a can of coke.

moles of caffeine = .................... mol

Caffeine is made up of 49.48%  carbon, 5.20% hydrogen, 28.85% nitrogen and the rest is oxygen.

Calculate the empirical formula of caffeine.

Calculate the molecular formula of caffeine using your answer from part (b).

Apatite is a general term used for a family of various calcium phosphate compounds commonly found in rocks and minerals, bones and teeth.

Fluorapatite, Ca₅(PO₄)₃F, reacts with sulfuric acid to form hydrogen phosphate, calcium sulfate and hydrogen fluoride.

Write the balanced chemical equation for this reaction.

Fluorapatite, Ca₅(PO₄)₃F, can also react with sulfuric acid to form calcium dihydrogenphosphate, Ca(H₂PO₄)₂, calcium sulfate and hydrogen fluoride.

2Ca₅(PO₄)₃F + 7H₂SO₄ → 3Ca(H₂PO₄)₂ + 7CaSO₄ + 2HF

Calculate the mass of calcium dihydrogenphosphate formed when 50.2 g of Ca₅(PO₄)₃F reacts with 87.9 g H₂SO₄.

mass of Ca(H₂PO₄)₂ = ............................ g