Quelpr

Titrimetric (Volumetric) Methods of Analysis · CAPE Chemistry Unit 2

88 past-paper questions on Titrimetric (Volumetric) Methods of Analysis, part of Analytical Methods and Separation Techniques, from every CAPE Chemistry Unit 2 paper on Quelpr.

Practise Titrimetric (Volumetric) Methods of Analysis
  1. 1(b)4 marks· CAPE Chemistry Unit 2 · 2005 · Paper 2Outline the steps needed to prepare a buffer solution of known pH and to determine that the solution is of the required pH.
  2. 4(b)(i)3 marks· CAPE Chemistry Unit 2 · 2005 · Paper 2Calculate the concentration of H+ ions in the 0.020 mol dm-3 solution of niacin at 298 K.
  3. 4(b)(ii)3 marks· CAPE Chemistry Unit 2 · 2005 · Paper 2Calculate the concentrations of niacin and the conjugate base in solution at 298 K.
  4. 4(b)(iii)3 marks· CAPE Chemistry Unit 2 · 2005 · Paper 2Calculate Ka for niacin at 298 K.
  5. 4(c)(ii)3 marks· CAPE Chemistry Unit 2 · 2005 · Paper 2Comment on the suitability of using a weak base to determine the concentration of niacin in solution by titration.
  6. 5(a)2 marks· CAPE Chemistry Unit 2 · 2006 · Paper 2Define the term 'buffer solution'.
  7. 5(b)(i)1 mark· CAPE Chemistry Unit 2 · 2006 · Paper 2Suggest a reason for adding a buffer to the pool.
  8. 5(b)(ii)2 marks· CAPE Chemistry Unit 2 · 2006 · Paper 2Use the equation HCO₃⁻(aq) + H₂O(l) ⇌ H₃O⁺(aq) + CO₃²⁻(aq) to explain how the aqueous hydrogen carbonate ion acts as a buffer.
  9. 5(c)(ii)1 mark· CAPE Chemistry Unit 2 · 2006 · Paper 2State ONE industry in which buffers are used.
  10. 5(d)(i)2 marks· CAPE Chemistry Unit 2 · 2006 · Paper 2Calculate the concentration of the sodium ethanoate solution in mol dm⁻³.
  11. 5(d)(ii)5 marks· CAPE Chemistry Unit 2 · 2006 · Paper 2K_a for ethanoic acid is equal to 1.8 × 10⁻⁵ mol dm⁻³. Write the expression for K_a and use it to calculate the pH of the buffer solution. State any assumptions made in the calculation.
  12. 5(e)(i)2 marks· CAPE Chemistry Unit 2 · 2006 · Paper 2Find the new concentrations of sodium ethanoate and ethanoic acid.
  13. 5(e)(ii)2 marks· CAPE Chemistry Unit 2 · 2006 · Paper 2Comment on the pH of the new solution and explain your answer.
  14. 6(b)(iii)2 marks· CAPE Chemistry Unit 2 · 2006 · Paper 2Suggest what would be observed when aqueous P reacts with aqueous iron(III) chloride. Explain your answer.
  15. 4(a)2 marks· CAPE Chemistry Unit 2 · 2007 · Paper 2Define the term 'buffer solution'.
  16. 4(b)(i)3 marks· CAPE Chemistry Unit 2 · 2007 · Paper 2Explain how a buffer mixture of a weak acid and its salt maintains pH upon the addition of strong acid.
  17. 4(b)(ii)3 marks· CAPE Chemistry Unit 2 · 2007 · Paper 2Explain how a buffer mixture of a weak acid and its salt maintains pH upon the addition of strong alkali.
  18. 4(c)(i)(a)2 marks· CAPE Chemistry Unit 2 · 2007 · Paper 2During periods of strenuous exercise, carbon dioxide builds up in the blood. Explain the effect of this build-up on the buffer system with reference to Equations 1 and 2.
  19. 4(c)(i)(b)4 marks· CAPE Chemistry Unit 2 · 2007 · Paper 2Explain how breathing more deeply and quickly during exercise can reverse this effect.
  20. 4(d)(i)1 mark· CAPE Chemistry Unit 2 · 2007 · Paper 2Write the expression for K_a of ethanoic acid.
  21. 4(d)(ii)5 marks· CAPE Chemistry Unit 2 · 2007 · Paper 2Use the K_a expression to calculate the pH of the buffer solution.
  22. 2(a)4 marks· CAPE Chemistry Unit 2 · 2008 (T&T) · Paper 2State THREE reasons why NaHCO3 can be used as a primary standard and ONE reason why sodium hydroxide (NaOH) may NOT be used.
  23. 2(b)(i)2 marks· CAPE Chemistry Unit 2 · 2008 (T&T) · Paper 2Write the balanced equation for the reaction between sodium hydrogen carbonate and sulphuric acid.
  24. 2(b)(ii)4 marks· CAPE Chemistry Unit 2 · 2008 (T&T) · Paper 2Calculate the mass in grams of sodium hydrogen carbonate that the student used to neutralise the acid if 23.00 cm3 of 6.00 mol dm-3 sulphuric acid were used from the burette.
  25. 2(c)5 marks· CAPE Chemistry Unit 2 · 2008 (T&T) · Paper 2Outline FIVE experimental steps to be carried out in the determination of the ethanoic acid content of vinegar by titration with sodium hydroxide solution.
  26. 2(a)(i)1 mark· CAPE Chemistry Unit 2 · 2009 · Paper 2Define the term 'Equivalence point'.
  27. 2(a)(ii)1 mark· CAPE Chemistry Unit 2 · 2009 · Paper 2Define the term 'End point'.
  28. 2(b)2 marks· CAPE Chemistry Unit 2 · 2009 · Paper 2Use the example of barium chloride and sodium carbonate to explain the technique of back titration.
  29. 2(c)(i)2 marks· CAPE Chemistry Unit 2 · 2009 · Paper 2Write the equation for the precipitation of barium ions.
  30. 2(c)(ii)2 marks· CAPE Chemistry Unit 2 · 2009 · Paper 2Calculate the number of moles of Na2CO3 remaining after filtration.
  31. 2(c)(iii)1 mark· CAPE Chemistry Unit 2 · 2009 · Paper 2Deduce the number of moles of BaCl2 which reacted with the sodium carbonate solution.
  32. 2(c)(iv)1 mark· CAPE Chemistry Unit 2 · 2009 · Paper 2Calculate the concentration of barium ions in mol dm⁻³.
  33. 2(d)(i)4 marks· CAPE Chemistry Unit 2 · 2009 · Paper 2List FOUR steps a student must follow to successfully standardize a solution of potassium manganate(VII) by titration using an oxalic acid solution.
  34. 2(d)(ii)1 mark· CAPE Chemistry Unit 2 · 2009 · Paper 2Identify the indicator in the titration in (d)(i).
  35. Q171 mark · multiple choice· CAPE Chemistry Unit 2 · 2012 · Paper 1Which of the following is NOT a property of a primary standard?
  36. Q181 mark · multiple choice· CAPE Chemistry Unit 2 · 2012 · Paper 1Which of the following will NOT affect the accuracy of the results in a titrimetric analysis?
  37. Q161 mark · multiple choice· CAPE Chemistry Unit 2 · 2013 · Paper 1Which of the following factors will NOT affect the accuracy of the results in a titrimetric analysis?
  38. Q171 mark · multiple choice· CAPE Chemistry Unit 2 · 2013 · Paper 1Which of the following instruments is NOT used in titrimetry?
  39. Q181 mark · multiple choice· CAPE Chemistry Unit 2 · 2013 · Paper 1Which of the following graphs illustrates the titration of dilute sulfuric acid with potassium hydroxide solution?
  40. Q171 mark · multiple choice· CAPE Chemistry Unit 2 · 2014 · Paper 1The concentration of an ammonia solution is determined by titrating 25.0\text{ cm}^3 against 0.2\text{ mol dm}^{-3} sulfuric acid to give an end point of 27.5\text{ cm}^3. The concentration of ammonia (in…
  41. 2(b)2 marks· CAPE Chemistry Unit 2 · 2015 · Paper 2List TWO requirements which a primary standard reagent that is to be used in a titrimetric analysis must satisfy.
  42. 2(c)(i)4 marks· CAPE Chemistry Unit 2 · 2015 · Paper 2Using the results in Table 1, plot a graph of temperature against volume of acid on the axes provided on page 7.
  43. 2(c)(ii)1 mark· CAPE Chemistry Unit 2 · 2015 · Paper 2Hence, determine the end-point volume of the acid.
  44. 2(c)(iii)2 marks· CAPE Chemistry Unit 2 · 2015 · Paper 2Calculate the concentration of the acid.
  45. 2(d)4 marks· CAPE Chemistry Unit 2 · 2015 · Paper 2Outline the experimental steps for this type of thermometric titration.
  46. Q171 mark · multiple choice· CAPE Chemistry Unit 2 · 2016 · Paper 1The concentration of an ammonia solution is determined by titrating 25.0\text{ cm}^3 against 0.2\text{ mol dm}^{-3} sulfuric acid to give an end point of 27.5\text{ cm}^3. The concentration of ammonia (in…
  47. Q301 mark · multiple choice· CAPE Chemistry Unit 2 · 2017 · Paper 1It takes 5\text{ cm}^3 of 1.4\text{ M NaOH} to neutralize 150\text{ cm}^3 of \text{HCl} with an unknown concentration. What was the original concentration of the acid?
  48. 5(a)(i)3 marks· CAPE Chemistry Unit 2 · 2017 · Paper 2List THREE characteristics of a primary standard.
  49. 5(a)(ii)2 marks· CAPE Chemistry Unit 2 · 2017 · Paper 2State whether sodium hydroxide can be considered a primary standard and give a reason for your answer.
  50. 5(b)4 marks· CAPE Chemistry Unit 2 · 2017 · Paper 2Explain fully the shape of the graph in Figure 2.
  51. 5(c)(i)1 mark· CAPE Chemistry Unit 2 · 2017 · Paper 2Calculate the number of moles of sodium hydrogen carbonate used.
  52. 5(c)(ii)2 marks· CAPE Chemistry Unit 2 · 2017 · Paper 2Calculate the number of moles of acid reacted, using the equivalence point from Figure 2.
  53. 5(c)(iii)1 mark· CAPE Chemistry Unit 2 · 2017 · Paper 2Calculate the concentration of the acid.
  54. 5(d)1 mark· CAPE Chemistry Unit 2 · 2017 · Paper 2State ONE other titrimetric method that could be used without an indicator by the student in (b).
  55. 5(e)1 mark· CAPE Chemistry Unit 2 · 2017 · Paper 2Identify the responding variable involved in the method stated in (d).
  56. 1(a)3 marks· Chemistry · Unit 2 Q1 1(a)Using the thermometer readings in Figure 1, on page 5, complete Table 1 by recording the temperatures for the additions of 5 cm³, 15 cm³ and 25 cm³ of H₂SO₄.
  57. 1(b)(i)4 marks· Chemistry · Unit 2 Q1 1(b)(i)Using the axes provided in Figure 2, on page 7, plot the graph of temperature against volume of acid added.
  58. 1(b)(ii)2 marks· Chemistry · Unit 2 Q1 1(b)(ii)Draw two lines of best fit through the points on the graph, one where the temperature is increasing and the other where the temperature is decreasing.
  59. 1(b)(iii)2 marks· Chemistry · Unit 2 Q1 1(b)(iii)On your graph, show the end point of the reaction. Record the corresponding volume below. End point of the reaction = ____ cm³
  60. 1(d)2 marks· Chemistry · Unit 2 Q1 1(d)Write a balanced chemical equation for the reaction between NaOH and H₂SO₄.
  61. 1(e)2 marks· Chemistry · Unit 2 Q1 1(e)Calculate the number of moles of H₂SO₄ used in the reaction.
  62. 1(f)2 marks· Chemistry · Unit 2 Q1 1(f)Calculate the number of moles of NaOH in 25 cm³ of the solution.
  63. 1(g)2 marks· Chemistry · Unit 2 Q1 1(g)Calculate the concentration of NaOH, in mol dm⁻³.
  64. 1(h)1 mark· Chemistry · Unit 2 Q1 1(h)Calculate the concentration of NaOH, in gdm⁻³, given the molar mass of NaOH = 40 gmol⁻¹.
  65. 1(i)2 marks· Chemistry · Unit 2 Q1 1(i)State whether the reaction that took place in the styrofoam cup was exothermic or endothermic. Explain your answer.
  66. 1(j)1 mark· Chemistry · Unit 2 Q1 1(j)State ONE safety precaution which should have been taken during the experiment.
  67. 2(a)3 marks· Chemistry · Unit 2 Q2 2(a)List THREE characteristics of ethanedioic acid that make it a suitable primary standard.
  68. 2(b)(i)3 marks· Chemistry · Unit 2 Q2 2(b)(i)List THREE reasons why NaHCO₃ can be used as a primary standard.
  69. 2(b)(ii)1 mark· Chemistry · Unit 2 Q2 2(b)(ii)State ONE reason why NaOH may NOT be used as a primary standard.
  70. 2(c)(i)1 mark· Chemistry · Unit 2 Q2 2(c)(i)Calculate EACH of the following. The number of moles MnO₄⁻ used
  71. 2(c)(i)2 marks· Chemistry · Unit 2 Q2 2(c)(i)Write the balanced equation for the reaction between sodium hydrogen carbonate and sulfuric acid.
  72. 2(c)(i)1 mark· Chemistry · Unit 2 Q2 2(c)(i)State which acid would be appropriate to use in Option 1.
  73. 2(c)(ii)1 mark· Chemistry · Unit 2 Q2 2(c)(ii)The number of moles Fe²⁺ in the 25.0 cm³ of aqueous R (aq)
  74. 2(c)(ii)4 marks· Chemistry · Unit 2 Q2 2(c)(ii)Calculate the mass (in grams) of the sodium hydrogen carbonate that the student would use to neutralize the acid, if 23.50 cm³ of the acid were used from the burette.
  75. 2(c)(ii)3 marks· Chemistry · Unit 2 Q2 2(c)(ii)In the space below, draw the titration curve that would be obtained for Option 1.
  76. 2(c)(iii)1 mark· Chemistry · Unit 2 Q2 2(c)(iii)The number of moles Fe²⁺ in 1.0 dm³ of R (aq)
  77. 2(c)(iii)3 marks· Chemistry · Unit 2 Q2 2(c)(iii)In the space below, draw the titration curve that would be obtained for Option 2.
  78. 2(c)(iv)1 mark· Chemistry · Unit 2 Q2 2(c)(iv)The mass of Fe²⁺ in 1 dm³ of R (aq)
  79. 2(c)(iv)4 marks· Chemistry · Unit 2 Q2 2(c)(iv)Using the information in Table 2 below, select the indicator(s) that cannot be used for the titrations. Option 1. Reason for selection. Option 2. Reason for selection.
  80. 2(c)(v)1 mark· Chemistry · Unit 2 Q2 2(c)(v)The percentage Fe²⁺ in the compound [The mass concentration of R is 40.90 g dm⁻³]
  81. 2(c)(v)2 marks· Chemistry · Unit 2 Q2 2(c)(v)The titration results obtained from Option 2 are listed below. Complete the table by filling in the spaces.
  82. 2(c)(vi)4 marks· Chemistry · Unit 2 Q2 2(c)(vi)Given that the stock solution of 250 cm³ contained ten tablets, use the information in (c) (v) to calculate the number of milligrams of aspirin contained in a titrated volume of 25.0 cm³ of aspirin (MW = 180.06 g/mol).
  83. 2(c)(vii)2 marks· Chemistry · Unit 2 Q2 2(c)(vii)The ingredient table below lists the milligram quantities of aspirin in a single tablet. Based on the findings in (c) (vi), state whether the information in Table 3 is accurate and give a reason for your response.
  84. 2(f)5 marks· Chemistry · Unit 2 Q2 2(f)Outline FIVE experimental steps that should be carried out to determine the ethanoic acid content of the vinegar.
  85. 6(a)(i)2 marks· Chemistry · Unit 2 Q6 6(a)(i)Describe a test that could be used to identify the gaseous product formed.
  86. 6(a)(ii)1 mark· Chemistry · Unit 2 Q6 6(a)(ii)A sample of the gas was collected in the laboratory by downward delivery. State the physical property of the gas which supports this method of collection.
  87. 6(a)(iii)2 marks· Chemistry · Unit 2 Q6 6(a)(iii)Write a chemical equation, including state symbols, for the reaction between hydrochloric acid and sodium hydrogen carbonate.
  88. 6(b)2 marks· Chemistry · Unit 2 Q6 6(b)Write an ionic equation for the reaction of magnesium with dilute hydrochloric acid.

Related topics in Analytical Methods and Separation Techniques