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Standard Grade Revision

Standard Grade Revision. Units 8 and 9. Q1. The non-metal sulphur reacts with oxygen to produce sulphur dioxide. a) Write a balanced equation, using symbols and formulae, for the reaction between sulphur and oxygen. What type of bonding is present in sulphur dioxide?

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Standard Grade Revision

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  1. Standard Grade Revision Units 8 and 9 • Q1. The non-metal sulphur reacts with oxygen to produce sulphur dioxide. • a) Write a balanced equation, using symbols and formulae, for the reaction between sulphur and oxygen. • What type of bonding is present in sulphur dioxide? • c) Sulphur dioxide dissolves in water. Suggest a pH for the solution. • S + O2 SO2 • Covalent bonds between the atoms in the molecules. Van der waals forces between the molecules. • (c) A pH less than 7 would be expected – sulphur dioxide is an acidic gas. Standard Grade Chemistry

  2. Units 8 and 9 Revision Q2. The pH of a solution can be found using a pH meter. The pH values of some solutions are shown in the table. Solution pH vinegar 3 cola 5 fruit juice 5 bleach 9 detergent 8 (a) Name the two alkaline solutions in the table. (b) Name the ion found in all acid solutions. (c) What pH value would pure water have? (d) When magnesium is reacted with vinegar, hydrogen gas is given off. What is the test for hydrogen gas? (a) Bleach and detergent. (b) Hydrogen ion [ H+(aq)] (c) pH of 7 (neutral) (d) Hydrogen burns with ‘pop’ Standard Grade Chemistry

  3. Units 8 and 9 Revision Q3. Laurie carried out an experiment to make copper sulphate crystals. (a) Name the type of chemical reaction taking place between the copper oxide and the dilute sulphuric acid. b) How is the excess copper oxide removed in step 4? c) Why would copper sulphate not be made by adding copper metal to dilute sulphuric acid? • Neutralisation • Filtration. • (c) Copper does not react with acid. Standard Grade Chemistry

  4. (i) pH less than 7 (an acidic solution). • (ii) pH more than 7 (an alkaline solution) (b) Insoluble in water. (c) 4 Na + O2 2Na2O Q4. The workcard below gives details of an experiment. • What would have been the pH of the solution when the element burned was • (i) carbon? • (ii) sodium? • (b) Suggest a reason why the pH of aluminium oxide could not be measured. • You may wish to use page 5 of the data booklet. • (c) Write a balanced equation, using symbols and formulae, for the reaction between sodium and oxygen. Standard Grade Chemistry

  5. Units 8 and 9 Revision. Q5. The box shows the names of some common ionic compounds. ammonium chloride copper carbonate potassium chloride calcium nitrate magnesium sulphate sodium hydroxide • Which two of these compounds are bases? • Which of these compounds is a salt formed from sulphuric acid? • (c) Which of these ionic compounds dissolves in water to form • an alkaline solution? • (d) Identify the compound that could be prepared by precipitation. • (You may wish to refer to page 5 of the data booklet) (a) Copper carbonate Sodium hydroxide (b) Magnesium sulphate. (c) Sodium hydroxide. (d) Copper carbonate Q6. Fish cannot survive in lochs if acid rain makes the pH of the water too low. • Sulphur dioxide • (b) H+(aq) • (c) Lime (calcium oxide) • Name the gas which causes acid rain. • (b) Which ion causes the water in the loch to be acidic? • (c) Name a substance which could be added to the loch to increase the pH of the water. Standard Grade Chemistry

  6. Units 8 and 9 Revision. Q7. Lee added magnesium carbonate to dilute hydrochloric acid in a beaker until no more reacts MgCO3(s) + 2HCl(aq)  MgCl2 (aq) + CO2 (g) + H2O(l) The contents of the beaker were then filtered. (a) What kind of reaction is shown by the balanced equation? (b) Which compound shown in the balanced equation is the residue? (c) Which two compounds would be present in the flask? (d) How would Lee know when the reaction had stopped? (e) In the reaction 0.05 moles of MgCO3 was reacted. What mass is present in 0.05 moles of MgCO3? (a) Neutralisation (b) MgCO3 (c) MgCl2 and H2O (d) No more gas given off and some MgCO3 solid left unreacted. (e) 4.2 g Standard Grade Chemistry

  7. mass n gfm n C V (l) Units 8 and 9 Revision. Q8. Calculate the mass of (a) 0.25 moles of sodium hydroxide (NaOH) (b) 0.1 moles of calcium carbonate. (Use your data book to write the formula of calcium carbonate) Q9. How many moles are present in (a) 2.2 g of carbon dioxide? (b) 1000g of ammonium nitrate? (NH4NO3) • 10g • (b) 10g • 0.05 mol • (b) 12.5 mol Q10. How many moles are present in 200 cm3 of a 0.5 mol/l solution of sodium chloride? 0.25 mol Q11. What is the concentration of solution which contains 0.5 moles of sodium chloride in 250 cm3 of solution? 2 mol/l Standard Grade Chemistry

  8. Q12. Egg shells and sea shells contain calcium carbonate. Calcium carbonate reacts with dilute hydrochloric acid to produce carbon dioxide gas. (a) State the test for carbon dioxide. (b) Adam wanted to find out which type of shell contained the most calcium carbonate. He set up the experiment shown below. (a) Turns lime water chalky (or milky). • State two ways in which Adam would know when the reaction had finished. • (ii) Adam repeated the experiment using 5g sea shell. Here are his results. • Sea shell Egg shell • Balance reading • at start / g 106.19 106.19 • Balance reading • at end / g 104.22 104.01 • Which type of shell contained the most calcium carbonate? Standard Grade Chemistry (b) (i) No more gas given off and unreacted solidc alcium carbonate left. (ii) Egg shell – it had the biggest decrease in mass.

  9. Units 8 and 9 Revision. Q13. The balanced equation for the reaction of zinc with hydrochloric acid is Zn + 2HCl  ZnCl2 + H2 (a) Calculate the mass of zinc required to produce 0.5 mole of hydrogen. (b) Calculate the mass of hydrogen produced when 3.275 g of zinc reacts with excess hydrochloric acid.   (a) 32.75 g (b)0.1 g Q14. Bones are formed when calcium ions and phosphate ions combine to form insoluble calcium phosphate, Ca3(PO4)2. This reaction can be reproduced in the laboratory by adding a solution of calcium chloride to a solution of sodium phosphate. 3Ca2+(aq) + 6Cl-(aq) + 6Na+(aq) + 2PO43-(aq)  6Na+(aq) + 6Cl-(aq) + (Ca2+)3(PO43-)2(s) (a) Write the formula for the spectator ions. (b) (i) What name is given to this type of reaction? (ii) What technique could be used to remove the calcium phosphate from the mixture? (a)Na+(aq) and Cl-(aq) (b) (i) Precipitation. (ii) Filtration. Standard Grade Chemistry

  10. Q15. A pupil carried out a titration using the chemicals and apparatus shown below. • How would the pupil know when to stop adding acid from the burette. • (b) (i) What average volume should be used to calculate the number of moles of • sulphuric acid needed to neutralise the potassium hydroxide solution? • (ii) Calculate the number of moles of sulphuric acid in this average volume. • (iii) The equation for the titration is •   H2SO4 + 2KOH  K2SO4 + 2H2O • Calculate the number of moles of potassium hydroxide in 20cm3 of the potassium hydroxide solution. (a) By noting the colour change of the indicator. (b) (i) 20.6 cm3 (ii) 0.00412 mol (iii) 0.00814 mol Standard Grade Chemistry

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