Secondary 4 Combined Science Chemistry Preliminary Examination Paper 1

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Secondary 4 Combined Science Chemistry - Preliminary Examination

Subject: Combined Science Chemistry
Level: Secondary 4
Paper: Preliminary Paper 1 (Version 1)
Duration: 1 hour 15 minutes
Total Marks: 65
Name: ____________________ Class: __________ Date: __________

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Instructions to Candidates:

1. Answer all questions.
2. Write your answers in the spaces provided.
3. For calculations, show all working clearly.
4. Use the relative atomic masses provided: H=1, C=12, N=14, O=16, Na=23, Mg=24, Al=27, S=32, Cl=35.5, K=39, Ca=40.

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Section A: Short Answer and Structured Questions (30 Marks)

Question 1 (a) State the pH value of a solution that is strongly alkaline. [1]

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(b) Describe the change in colour of universal indicator when it is added to a solution of dilute hydrochloric acid. [1]

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Question 2 A student is tasked with preparing a sample of pure sodium chloride. (a) Name the most suitable method for preparing this salt. [1]

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(b) State the reactants required for this method. [1]

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(c) Explain why the salt must be heated until the solution is saturated before cooling. [2]

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Question 3 The following chemical reactions are carried out in a laboratory: I. $\text{HCl(aq)} + \text{NaOH(aq)} \rightarrow \text{NaCl(aq)} + \text{H}_2\text{O(l)}$ II. $\text{Zn(s)} + 2\text{HCl(aq)} \rightarrow \text{ZnCl}_2\text{(aq)} + \text{H}_2\text{(g)}$ III. $\text{CaCO}_3\text{(s)} + 2\text{HCl(aq)} \rightarrow \text{CaCl}_2\text{(aq)} + \text{H}_2\text{O(l)} + \text{CO}_2\text{(g)}$

(a) Classify reaction I using a term from the list: {Addition, Neutralisation, Substitution, Redox}. [1]

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(b) Classify reaction II using a term from the list: {Addition, Neutralisation, Substitution, Redox}. [1]

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(c) For reaction III, state the observation made when the gas produced is bubbled through limewater. [1]

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Question 4 A solution of an unknown salt X is tested. When aqueous silver nitrate is added, a white precipitate is formed. When dilute nitric acid is added to the precipitate, it remains insoluble. (a) Identify the anion present in salt X. [1]

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(b) If salt X is found to be soluble in water, suggest a possible formula for salt X. [1]

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Question 5 (a) Define the term 'strong acid'. [2]

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(b) Give one example of a weak acid. [1]

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Question 6 A student wants to measure exactly $25.0\text{ cm}^3$ of $0.1\text{ mol/dm}^3$ sodium hydroxide solution for a titration. (a) Which piece of apparatus is most suitable for measuring this volume accurately? [1]

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(b) Explain your choice of apparatus in (a). [1]

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Question 7 (a) Write a balanced chemical equation, including state symbols, for the reaction between magnesium ribbon and dilute sulfuric acid. [3]

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(b) State the test for the gas evolved in part (a) and the expected result. [2]

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Section B: Data Interpretation and Calculations (35 Marks)

Question 8 A student reacts $2.4\text{ g}$ of magnesium ribbon with an excess of $1.0\text{ mol/dm}^3$ hydrochloric acid. $\text{Mg(s)} + 2\text{HCl(aq)} \rightarrow \text{MgCl}_2\text{(aq)} + \text{H}_2\text{(g)}$

(a) Calculate the number of moles of magnesium used. [2]

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(b) Calculate the volume of hydrogen gas produced at room temperature and pressure (RTP). (Molar volume of gas at RTP = $24\text{ dm}^3\text{mol}^{-1}$) [3]

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(c) Calculate the mass of $\text{MgCl}_2$ produced. [3]

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Question 9 The table below shows the pH values of four different solutions.

Solution	pH Value
A	2
B	7
C	9
D	13

(a) Which solution is the strongest base? Explain your answer. [2]

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(b) If solution A is dilute nitric acid, describe the change in pH if the solution is diluted with distilled water. Explain your reasoning. [3]

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Question 10 A sample of an organic acid is suspected to be unsaturated. (a) Describe a chemical test to confirm if the organic acid is unsaturated. [2]

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(b) State the observation if the acid is indeed unsaturated. [1]

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Question 11 A student performs a titration to find the concentration of a solution of sulfuric acid ($\text{H}_2\text{SO}_4$). $25.0\text{ cm}^3$ of the acid is neutralized by $20.0\text{ cm}^3$ of $0.5\text{ mol/dm}^3$ sodium hydroxide ($\text{NaOH}$). $\text{H}_2\text{SO}_4\text{(aq)} + 2\text{NaOH(aq)} \rightarrow \text{Na}_2\text{SO}_4\text{(aq)} + 2\text{H}_2\text{O(l)}$

(a) Calculate the number of moles of $\text{NaOH}$ used. [2]

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(b) Determine the number of moles of $\text{H}_2\text{SO}_4$ that reacted. [2]

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(c) Calculate the concentration of the sulfuric acid in $\text{mol/dm}^3$. [3]

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Question 12 Explain, using the concept of proton transfer, why an acid reacts with a base to form a salt and water. [4]

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Question 13 (a) State the chemical formula of the salt formed when potassium hydroxide reacts with phosphoric acid. [1]

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(b) Describe how you would obtain a pure, dry sample of this salt from the resulting solution. [4]

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Answer Key - Combined Science Chemistry Preliminary Paper 1 (Version 1)

Section A

Question 1 (a) pH 11 to 14 (Accept any value in this range). [1] (b) Changes from green/yellow to red. [1]

Question 2 (a) Titration. [1] (b) Sodium hydroxide ($\text{NaOH}$) and Hydrochloric acid ($\text{HCl}$). [1] (c) To ensure maximum yield of crystals upon cooling / To allow crystals to form as the solubility decreases with temperature. [2]

Question 3 (a) Neutralisation. [1] (b) Redox (or Substitution). [1] (c) Limewater turns milky/cloudy. [1]

Question 4 (a) Chloride ($\text{Cl}^-$). [1] (b) $\text{NaCl}$ or $\text{KCl}$ or $\text{MgCl}_2$ etc. [1]

Question 5 (a) An acid that completely ionizes/dissociates in aqueous solution to produce a high concentration of $\text{H}^+$ ions. [2] (b) Ethanoic acid / Citric acid. [1]

Question 6 (a) Pipette. [1] (b) It is designed to deliver a single, fixed volume with very high precision/accuracy. [1]

Question 7 (a) $\text{Mg(s)} + \text{H}_2\text{SO}_4\text{(aq)} \rightarrow \text{MgSO}_4\text{(aq)} + \text{H}_2\text{(g)}$ [3] - 1 mark for correct formulae. - 1 mark for balancing. - 1 mark for all correct state symbols. (b) Test: Use a lighted splint. Result: Gas burns with a 'pop' sound. [2]

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Section B

Question 8 (a) $\text{Moles of Mg} = \text{mass} / \text{molar mass} = 2.4 / 24 = 0.1\text{ mol}$. [2] (b) $\text{Mole ratio Mg : H}_2 = 1 : 1$. $\text{Moles of H}_2 = 0.1\text{ mol}$. $\text{Volume} = 0.1 \times 24 = 2.4\text{ dm}^3$. [3] (c) $\text{Mole ratio Mg : MgCl}_2 = 1 : 1$. $\text{Moles of MgCl}_2 = 0.1\text{ mol}$. $\text{Molar mass of MgCl}_2 = 24 + (35.5 \times 2) = 95\text{ g/mol}$. $\text{Mass} = 0.1 \times 95 = 9.5\text{ g}$. [3]

Question 9 (a) Solution D. [1] It has the highest pH value (13), indicating the highest concentration of $\text{OH}^-$ ions. [1] (b) pH increases (becomes less acidic/moves towards 7). [1] Dilution decreases the concentration of $\text{H}^+$ ions per unit volume. [2]

Question 10 (a) Add bromine water to the organic acid. [2] (b) The orange/brown bromine water is decolorized. [1]

Question 11 (a) $\text{Moles of NaOH} = (0.5 \times 20.0) / 1000 = 0.01\text{ mol}$. [2] (b) $\text{Mole ratio H}_2\text{SO}_4 : \text{NaOH} = 1 : 2$. $\text{Moles of H}_2\text{SO}_4 = 0.01 / 2 = 0.005\text{ mol}$. [2] (c) $\text{Concentration} = \text{moles} / \text{volume (dm}^3\text{)}$ $\text{Conc} = 0.005 / (25.0 / 1000) = 0.005 / 0.025 = 0.2\text{ mol/dm}^3$. [3]

Question 12 Acids are proton ($\text{H}^+$) donors. [1] Bases are proton ($\text{H}^+$) acceptors. [1] In a neutralisation reaction, the acid transfers a proton to the base. [1] This forms water ($\text{H}_2\text{O}$) and a salt consisting of the remaining ions. [1]

Question 13 (a) $\text{K}_3\text{PO}_4$. [1] (b)

• Heat the solution in an evaporating dish to concentrate it/until saturated. [1]
• Allow the solution to cool to crystallize the salt. [1]
• Filter the crystals from the remaining solution. [1]
• Wash crystals with a small amount of cold distilled water and dry between filter papers. [1]