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Secondary 3 Chemistry Semestral Assessment 2 (End of Year) Paper 3

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TuitionGoWhere Practice Paper - Chemistry Secondary 3

TuitionGoWhere Secondary School (AI)

Subject: Chemistry
Level: Secondary 3 (Express)
Assessment: SA2 Practice Paper (Version 3 of 5)
Topic Focus: Acids, Bases, and Salts
Duration: 1 Hour
Total Marks: 50

Name: ________________________
Class: ________________________
Date: ________________________

Instructions to Candidates

Write your name, class, and date in the spaces above.
Answer all questions.
Write your answers in the spaces provided on this question paper.
The number of marks is given in brackets [ ] at the end of each question or part question.
You may use a calculator.
A copy of the Periodic Table is provided on page 12 (not included in this extract, assume standard data).

Section A: Structured Questions (30 Marks)

Answer all questions in this section.

1. Soil Acidity and Neutralisation
A farmer tests the soil in his field and finds that the pH is 5.0. He wishes to raise the pH to a more neutral level to improve crop growth.

(a) State the name of the solid compound commonly added to soil to increase the pH. [1]

(b) Explain, with the aid of a chemical equation, how this compound neutralises the acidity in the soil. [2]

2. Preparation of Salts
Salts can be prepared by various methods depending on their solubility.

(a) Name the method used to prepare a sample of lead(II) sulfate from lead(II) nitrate solution and dilute sulfuric acid. [1]

(b) Describe the essential steps to obtain a pure, dry sample of lead(II) sulfate crystals after the reaction has occurred. [3]

3. Titration Analysis
A student performs a titration to determine the concentration of a solution of sulfuric acid, $H_2SO_4$ .
$25.0 \text{ cm}^3$ of $0.10 \text{ mol/dm}^3$ sodium hydroxide, $NaOH$ , is pipetted into a conical flask.
The sulfuric acid is added from a burette. The equation for the reaction is:
$2NaOH(aq) + H_2SO_4(aq) \rightarrow Na_2SO_4(aq) + 2H_2O(l)$

The following burette readings were recorded:

Titration	Rough	1	2	3
Final reading / $\text{cm}^3$	24.50	23.80	47.90	24.10
Initial reading / $\text{cm}^3$	0.00	0.00	23.80	0.00
Volume used / $\text{cm}^3$	24.50	23.80	24.10	24.10

(a) Identify the concordant results from the table above. [1]

(b) Calculate the average volume of sulfuric acid used. [1]
_________________________________________________________________________ $\text{cm}^3$

(c) Calculate the number of moles of sodium hydroxide present in the conical flask. [1]
_________________________________________________________________________ mol

(d) Calculate the concentration of the sulfuric acid in $\text{mol/dm}^3$ . [2]

4. Properties of Ammonia
Ammonia is an important industrial chemical.

(a) State the conditions required for the Haber Process to manufacture ammonia. [2]
Temperature: ________________________
Pressure: ________________________
Catalyst: ________________________

(b) Ammonia is a weak base. Explain what is meant by the term weak base. [2]

(ii) Write the chemical equation for this reaction. [1]

5. Identification of Ions
Solution X is known to contain one cation and one anion. The following tests are performed:

Test	Observation
Add aqueous sodium hydroxide, dropwise then in excess.	White precipitate formed, which dissolves in excess.
Add aqueous ammonia, dropwise then in excess.	White precipitate formed, which dissolves in excess.
Add dilute nitric acid followed by aqueous barium nitrate.	White precipitate formed.

(a) Identify the cation present in Solution X. [1]

(b) Identify the anion present in Solution X. [1]

6. Strong and Weak Acids
Two acids, Hydrochloric acid ( $HCl$ ) and Ethanoic acid ( $CH_3COOH$ ), have the same concentration of $1.0 \text{ mol/dm}^3$ .

(a) Explain why hydrochloric acid has a lower pH than ethanoic acid. [2]

(b) Describe a simple experimental method, other than measuring pH, to distinguish between these two acids of the same concentration. State the expected observations. [2]
Method: ___________________________________________________________________
Observation for HCl: ______________________________________________________
Observation for $CH_3COOH$ : _______________________________________________

Section B: Free Response Questions (20 Marks)

Answer all questions in this section.

7. Reaction Rates and Acids
Magnesium ribbon reacts with dilute hydrochloric acid to produce hydrogen gas.
$Mg(s) + 2HCl(aq) \rightarrow MgCl_2(aq) + H_2(g)$

A student investigates the effect of acid concentration on the rate of reaction. She measures the volume of hydrogen gas produced every 30 seconds.

(a) Sketch a graph showing the volume of hydrogen gas produced against time for:

Experiment A: $1.0 \text{ mol/dm}^3$ HCl
Experiment B: $0.5 \text{ mol/dm}^3$ HCl
Label the curves A and B. [3]

Graph space

(b) Explain, in terms of particle collision theory, why the initial rate of reaction in Experiment A is faster than in Experiment B. [2]

(c) The student repeats Experiment A but uses magnesium powder instead of magnesium ribbon.
(i) State how the initial rate of reaction changes. [1]

(ii) Explain this change. [1]

8. Salt Preparation and Yield
Copper(II) sulfate crystals can be prepared by reacting excess copper(II) oxide with dilute sulfuric acid.

(a) Why is excess copper(II) oxide used? [1]

(b) After the reaction is complete, the mixture is filtered.
(i) What is removed by filtration? [1]

(ii) What is present in the filtrate? [1]

(c) The filtrate is heated to saturation and then left to cool. Crystals form.
Explain why cooling the solution causes crystals to form. [2]

(d) In an experiment, $25.0 \text{ cm}^3$ of $2.0 \text{ mol/dm}^3$ sulfuric acid was used.
Calculate the maximum theoretical mass of copper(II) sulfate crystals ( $CuSO_4 \cdot 5H_2O$ ) that could be formed.
[Relative atomic masses: H=1, O=16, S=32, Cu=63.5] [3]

Mass = ________________________ g

(e) The actual mass of crystals obtained was $10.5 \text{ g}$ . Calculate the percentage yield. [1]

Percentage Yield = ________________________ %

9. Environmental Chemistry
Sulfur dioxide ( $SO_2$ ) is a pollutant gas released from the combustion of fossil fuels containing sulfur.

(a) Describe the environmental effect of sulfur dioxide emissions. [2]

(b) Flue gas desulfurisation is used to remove sulfur dioxide from power station emissions. Calcium carbonate is used in this process.
Write the chemical equation for the reaction between calcium carbonate and sulfur dioxide. [2]

END OF PAPER

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Answers

TuitionGoWhere Practice Paper - Chemistry Secondary 3

Answer Key & Marking Scheme
Assessment: SA2 Practice Paper (Version 3 of 5)
Topic Focus: Acids, Bases, and Salts

Section A: Structured Questions

1. Soil Acidity and Neutralisation
(a) Calcium oxide / Calcium hydroxide / Calcium carbonate.
(Accept: Quicklime, Slaked lime, Limestone. Do not accept just "Lime" without specification if ambiguous, but usually accepted in Sec 3. Best answer: Calcium oxide or Calcium hydroxide.) [1]

(b) Equation:
$CaO(s) + 2H^+(aq) \rightarrow Ca^{2+}(aq) + H_2O(l)$
OR
$Ca(OH)_2(s) + 2H^+(aq) \rightarrow Ca^{2+}(aq) + 2H_2O(l)$
OR
$CaCO_3(s) + 2H^+(aq) \rightarrow Ca^{2+}(aq) + H_2O(l) + CO_2(g)$
(1 mark for correct reactants/products, 1 mark for balancing/state symbols if required by strict marking, but usually 1 mark for correct chemical change description. Given [2], allow 1 for identifying neutralisation reaction type and 1 for equation.)
Marking Note: Accept word equation if chemical formula is incorrect but concept is clear? No, Sec 3 requires chemical equations.
[2]

2. Preparation of Salts
(a) Precipitation. [1]

(b) 1. Filter the mixture to collect the residue (precipitate).
2. Wash the residue with distilled water to remove soluble impurities.
3. Dry the residue between filter papers or in an oven.
(1 mark per correct step, max 3) [3]

(c) Sodium sulfate is soluble in water. Precipitation method is only for insoluble salts.
(Or: Sodium salts are all soluble, so no precipitate forms.) [1]

3. Titration Analysis
(a) Titration 2 and 3 (24.10 and 24.10).
(Note: Titration 1 is 23.80, which is >0.10 cm³ different from 2 and 3. Rough is ignored.) [1]

(b) Average volume = $\frac{24.10 + 24.10}{2} = 24.10 \text{ cm}^3$ . [1]

(d) From equation: 2 mol NaOH reacts with 1 mol $H_2SO_4$ .
Moles of $H_2SO_4 = \frac{0.0025}{2} = 0.00125 \text{ mol}$ .
Concentration of $H_2SO_4 = \frac{n}{V} = \frac{0.00125}{\frac{24.10}{1000}} = \frac{0.00125}{0.0241} \approx 0.0519 \text{ mol/dm}^3$ .
(Accept 0.052 mol/dm³) [2]

4. Properties of Ammonia
(a) Temperature: 450°C
Pressure: 200 atm
Catalyst: Iron
(1 mark for each correct condition, max 2 if only 2 blanks? Question asks for 3 items but marks [2]. Usually 1 mark for T/P combo and 1 for Catalyst, or 1 for each of any two. Let's assume 1 mark for T, 1 mark for P, Catalyst is bonus or part of T/P. Standard marking: 1 mark for correct T, 1 mark for correct P. Catalyst often required for full credit in some schemes, but here [2] marks for 3 lines suggests 1 mark for T/P pair and 1 for Catalyst? Or 1 mark each for any two. Let's award 1 for T, 1 for P. Catalyst is standard knowledge.)
Correction: Usually 3 marks for 3 conditions. If [2], likely 1 for T and 1 for P/Catalyst combined or just T and P. Let's award:
Temp: 450°C [1]
Pressure: 200 atm [1]
(Catalyst: Iron - if student writes it, no penalty, but marks capped at 2) [2]

(b) A weak base partially ionises/dissociates in water.
It produces a low concentration of hydroxide ions ( $OH^-$ ).
(1 mark for "partial ionisation", 1 mark for reference to $OH^-$ or equilibrium) [2]

5. Identification of Ions
(a) Zinc ion ( $Zn^{2+}$ ).
(Aluminium also forms white ppt soluble in excess NaOH, but Al(OH)3 is insoluble in excess ammonia. Zn(OH)2 is soluble in excess ammonia. Therefore, it must be Zinc.) [1]

(b) Sulfate ion ( $SO_4^{2-}$ ). [1]

6. Strong and Weak Acids
(a) HCl is a strong acid and fully ionises in water to produce a high concentration of $H^+$ ions.
Ethanoic acid is a weak acid and only partially ionises, producing a lower concentration of $H^+$ ions.
Lower $[H^+]$ means higher pH.
(1 mark for full vs partial ionisation, 1 mark for link to $[H^+]$ and pH) [2]

(b) Method: React equal volumes/concentrations of each acid with a named metal (e.g., Magnesium) or carbonate (e.g., Calcium Carbonate).
Observation for HCl: Faster rate of effervescence / bubbles produced more vigorously.
Observation for $CH_3COOH$ : Slower rate of effervescence.
(1 mark for method, 1 mark for correct comparison of observations) [2]

Section B: Free Response Questions

7. Reaction Rates and Acids
(a) Graph:

Y-axis: Volume of $H_2$ ( $\text{cm}^3$ ), X-axis: Time (s).
Curve A: Steeper initial gradient, levels off at a higher or same volume?
Note: Same amount of Mg and same volume of acid? The question implies same volume of acid but different concentration. If acid is in excess, final volume depends on Mg. If Mg is in excess, final volume depends on acid moles.
Standard Assumption: Usually, Mg is the limiting reagent in these "rate" questions unless specified. If Mg is limiting, both curves level off at the same final volume.
Curve A (1.0 M): Steeper slope, reaches plateau earlier.
Curve B (0.5 M): Less steep slope, reaches plateau later.
Both reach same maximum volume.
(1 mark for correct shape/labels, 1 mark for A steeper than B, 1 mark for same final volume) [3]

(b) Higher concentration means more particles per unit volume.
This leads to a higher frequency of effective collisions between Mg and $H^+$ ions.
(1 mark for more particles/collisions, 1 mark for frequency of effective collisions) [2]

(c) (i) Rate increases. [1]
(ii) Powder has a larger surface area than ribbon.
This allows more frequent collisions between reactant particles. [1]

8. Salt Preparation and Yield
(a) To ensure all the sulfuric acid reacts.
(Or: To ensure the acid is the limiting reagent and is completely used up.) [1]

(b) (i) Excess copper(II) oxide (unreacted solid). [1]
(ii) Copper(II) sulfate solution (and water). [1]

(c) Solubility of copper(II) sulfate decreases as temperature decreases.
The solution becomes supersaturated, and the excess solute crystallises out.
(1 mark for solubility decreases with temp, 1 mark for crystallisation) [2]

(d) Moles of $H_2SO_4 = 2.0 \times \frac{25.0}{1000} = 0.050 \text{ mol}$ .
Ratio $H_2SO_4 : CuSO_4 \cdot 5H_2O$ is 1:1.
Moles of crystals = 0.050 mol.
Molar Mass of $CuSO_4 \cdot 5H_2O = 63.5 + 32 + (4 \times 16) + 5(18) = 159.5 + 90 = 249.5 \text{ g/mol}$ .
Mass = $0.050 \times 249.5 = 12.475 \text{ g}$ .
(Accept 12.5 g) [3]

(e) Percentage Yield = $\frac{\text{Actual}}{\text{Theoretical}} \times 100 = \frac{10.5}{12.475} \times 100 \approx 84.17\%$ .
(Accept 84.2%) [1]

9. Environmental Chemistry
(a) Sulfur dioxide dissolves in rainwater to form sulfuric acid.
This causes acid rain, which lowers the pH of soil and water bodies, damaging plants and aquatic life / corroding buildings.
(1 mark for formation of acid rain, 1 mark for effect) [2]

(b) $CaCO_3(s) + SO_2(g) \rightarrow CaSO_3(s) + CO_2(g)$ .
(Note: Often oxidised to sulfate in air, but primary reaction is sulfite. Accept $2CaCO_3 + 2SO_2 + O_2 \rightarrow 2CaSO_4 + 2CO_2$ if advanced. Standard Sec 3: Carbonate + Acid Gas -> Salt + CO2. SO2 is acidic oxide.)
Equation: $CaCO_3 + SO_2 \rightarrow CaSO_3 + CO_2$ . [2]

(c) Car exhausts / Internal combustion engines / Lightning.
(High temperature causes Nitrogen and Oxygen from air to react.) [1]

END OF MARKING SCHEME