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Acids, Bases and Salts · CSEC Chemistry

153 past-paper questions on Acids, Bases and Salts, part of Principles of Chemistry, from every CSEC Chemistry paper on Quelpr.

Practise Acids, Bases and Salts
  1. 1(a)(i)2 marks· Chemistry Q1 1(a)(i)Differentiate between a 'strong acid' and a 'weak acid'.
  2. 1(a)(i)2 marks· Chemistry Q1 1(a)(i)Explain how a salt is formed.
  3. 1(a)(i)2 marks· Chemistry Q1 1(a)(i)Define the term 'normal salt'.
  4. 1(a)(i)a)4 marks· Chemistry Q1 1(a)(i)a)What is meant by EACH of the following? pH scale
  5. 1(a)(i)b)4 marks· Chemistry Q1 1(a)(i)b)What is meant by EACH of the following? The end point of an acid-base titration
  6. 1(a)(ii)2 marks· Chemistry Q1 1(a)(ii)Identify ONE other type of salt that can be formed from the reaction between dilute sulfuric acid and sodium hydroxide. Write the chemical formula for that salt.
  7. 1(a)(ii)1 mark· Chemistry Q1 1(a)(ii)Suggest ONE other base that could be used instead of NaOH.
  8. 1(a)(ii)2 marks· Chemistry Q1 1(a)(ii)What is the difference between 'anhydrous salts' and 'hydrated salts'?
  9. 1(a)(ii)2 marks· Chemistry Q1 1(a)(ii)Complete Table 1 below by recording the missing pH meter readings from Figure 1.
  10. 1(a)(iii)1 mark· Chemistry Q1 1(a)(iii)State the name of ONE other acid that can also produce the type of salt identified in (ii) above.
  11. 1(a)(iii)3 marks· Chemistry Q1 1(a)(iii)Using the graph paper provided on page 5 and the data in Table 1, plot a graph of pH against volume of sodium hydroxide added.
  12. 1(a)(iv)1 mark· Chemistry Q1 1(a)(iv)Use the graph to determine the volume of sodium hydroxide which reacts completely with the 20 cm³ of 0.005 mol dm⁻³ sulphuric acid.
  13. 1(b)(i)2 marks· Chemistry Q1 1(b)(i)Complete Table 1 by using the readings shown in Figure 1.
  14. 1(b)(ii)1 mark· Chemistry Q1 1(b)(ii)Determine the volume of acid used to neutralize 25 cm³ of NaOH.
  15. 1(b)(iii)1 mark· Chemistry Q1 1(b)(iii)Explain why NO indicator was used in the procedure in Part B.
  16. 1(b)(iv)2 marks· Chemistry Q1 1(b)(iv)Complete the procedure for Part B by stating Step 3. Step 3 is required for obtaining a dry sample of the normal salt.
  17. 1(b)(viii)1 mark· Chemistry Q1 1(b)(viii)The actual mass of salt obtained by the students was 0.09 g. Suggest ONE possible reason for the difference between the mass of salt expected and the mass obtained.
  18. 1(c)3 marks· Chemistry Q1 1(c)Describe an appropriate method to produce a pure solid sample of silver chloride starting with silver nitrate solution. (Hint! All silver salts are decomposed by light.)
  19. 1(c)(i)2 marks· Chemistry Q1 1(c)(i)Outline the procedure for the experiment.
  20. 1(c)(ii)1 mark· Chemistry Q1 1(c)(ii)List the materials necessary.
  21. 1(c)(iii)1 mark· Chemistry Q1 1(c)(iii)What evidence will result from your procedure to distinguish between the two acids?
  22. 2(a)(i)1 mark· Chemistry Q2 2(a)(i)Define the terms 'acid' and 'alkali'.
  23. 2(a)(ii)1 mark· Chemistry Q2 2(a)(ii)Define the terms 'acid salts' and 'normal salts'.
  24. 2(a)(ii)1 mark· Chemistry Q2 2(a)(ii)Would the solution formed from the reaction of X with water be acidic or basic? Explain your answer.
  25. 2(a)(iii)1 mark· Chemistry Q2 2(a)(iii)State the molecular formula for the normal salt formed from the reaction between phosphoric acid and sodium hydroxide.
  26. 2(a)(v)1 mark· Chemistry Q2 2(a)(v)State the molecular formula for an acid salt formed from the reaction between phosphoric acid and sodium hydroxide.
  27. 2(b)3 marks· Chemistry Q2 2(b)Which element in Table 2 forms an oxide which readily dissolves in water to give a solution with a pH greater than 7? Write a balanced equation to support your answer.
  28. 2(b)1 mark· Chemistry Q2 2(b)Which of the two acids is stronger?
  29. 2(b)(ii)4 marks· Chemistry Q2 2(b)(ii)Outline a suitable laboratory method for preparing a dry sample of calcium sulphate. Include a relevant equation in your answer.
  30. 2(b)(iii)2 marks· Chemistry Q2 2(b)(iii)Write a balanced chemical equation for the reaction of the carbonate of Q with dilute hydrochloric acid. Equation:
  31. 2(c)(i)1 mark· Chemistry Q2 2(c)(i)Which of the Suspensions, P or Q, could serve as an antacid?
  32. 2(c)(i)2 marks· Chemistry Q2 2(c)(i)Name TWO acids present in orange juice.
  33. 2(c)(ii)2 marks· Chemistry Q2 2(c)(ii)Write a chemical equation to support your answer to (c) (i).
  34. 2(c)(ii)1 mark· Chemistry Q2 2(c)(ii)State the type of chemical reaction that takes place in the treatment of excess stomach acid.
  35. 2(c)(iii)1 mark· Chemistry Q2 2(c)(iii)Hence, name ONE substance that can be used to treat excess stomach acid.
  36. 2(d)(i)1 mark· Chemistry Q2 2(d)(i)Suggest the name of a common household chemical that can be used to clean such tarnished copper ornaments.
  37. 2(d)(ii)2 marks· Chemistry Q2 2(d)(ii)Write a suitable ionic equation to show the reaction in (d) (i) above.
  38. 3(b)(ii)2 marks· Chemistry Q3 3(b)(ii)Write a balanced equation for the reaction of E with solid magnesium oxide (MgO).
  39. 3(b)(ii)2 marks· Chemistry Q3 3(b)(ii)Is the solution of Compound Q acidic or basic? State a reason for your answer.
  40. 3(c)(i)2 marks· Chemistry Q3 3(c)(i)Write a balanced equation for the reaction of ethanoic acid with magnesium metal, Mg (s).
  41. 3(c)(ii)1 mark· Chemistry Q3 3(c)(ii)Would this reaction take place at room temperature?
  42. 4(a)4 marks· Chemistry Q4 4(a)Define the term 'salt'. Identify ONE product that EACH of the salts mentioned above is used to manufacture.
  43. 4(a)(i)10 marks· Chemistry Q4 4(a)(i)State the expected observations and write balanced chemical equations to explain any reactions that take place. Give the chemical test(s) which may be used to identify any gases produced. Record your answer in a table…
  44. 4(a)(i)5 marks· Chemistry Q4 4(a)(i)Describe ONE method for the preparation of dry calcium carbonate in the laboratory. In your answer, include an equation for the reaction as well as the steps that are involved in its preparation.
  45. 4(a)(ii)1 mark· Chemistry Q4 4(a)(ii)The main ingredient in Epsom salts is magnesium sulfate. List ONE use of Epsom salts.
  46. 4(a)(ii)2 marks· Chemistry Q4 4(a)(ii)Iron(II) oxide reacts with dilute sulphuric acid to give a pale green solution. Write the equation for the reaction between iron(II) oxide and dilute sulphuric acid.
  47. 4(a)(ii)2 marks· Chemistry Q4 4(a)(ii)Outline a method that can be used to obtain a solid sample of a salt where EITHER the K₂CO₃ OR Zn completely reacts with the dilute nitric acid as described in (a) (i) above.
  48. 4(a)(iii)4 marks· Chemistry Q4 4(a)(iii)Describe any difference(s) that may be observed in the reaction indicated in (a)(i) above, if dilute sulphuric acid were to be used instead of dilute hydrochloric acid. Give a reason for your answer.
  49. 4(a)(iii)2 marks· Chemistry Q4 4(a)(iii)Give ONE test that can be used to distinguish the solution of the oxide of Element Y from the solution of the oxide of sulphur.
  50. 4(b)6 marks· Chemistry Q4 4(b)Outline the laboratory preparation of a pure, dry sample of CaCO₃. Include in your response a balanced chemical equation.
  51. 4(c)5 marks· Chemistry Q4 4(c)Write a balanced chemical equation with state symbols to illustrate how NaNO₃ can be prepared in the laboratory. Explain why NaNO₃ cannot be prepared utilizing the same method used for the preparation of CaCO₃.
  52. 4(c)(ii)3 marks· Chemistry Q4 4(c)(ii)State whether an aqueous solution of this compound would be acidic or basic and give ONE reason for your answer.
  53. 4(c)(iii)1 mark· Chemistry Q4 4(c)(iii)State ONE test to determine if an aqueous solution of this compound is acidic or basic.
  54. 4(d)(i)2 marks· Chemistry Q4 4(d)(i)Describe a test that can be used to identify the solution formed with sulphur dioxide.
  55. 4(d)(ii)1 mark· Chemistry Q4 4(d)(ii)Write a balanced equation to support the use of this test.
  56. 5(a)(i)2 marks· Chemistry Q5 5(a)(i)Amphoteric oxide
  57. 5(a)(i)2 marks· Chemistry Q5 5(a)(i)Write balanced equations for the reactions between hydrochloric acid and sodium sulphite.
  58. 5(a)(i)5 marks· Chemistry Q5 5(a)(i)State the name of the anhydride and describe how it is produced. (The conditions for the reactions are necessary but there is no need to write the equations.)
  59. 5(a)(ii)2 marks· Chemistry Q5 5(a)(ii)Write balanced equations for the reactions between hydrochloric acid and sodium carbonate.
  60. 5(a)(ii)2 marks· Chemistry Q5 5(a)(ii)Acid anhydride
  61. 5(a)(iii)2 marks· Chemistry Q5 5(a)(iii)Suggest why the anhydride is NOT directly added to water to produce sulfuric acid.
  62. 5(a)(iii)2 marks· Chemistry Q5 5(a)(iii)When sulphur trioxide gets into the atmosphere, it can form acid rain which can destroy buildings made from limestone. Write an ionic equation which BEST represents the chemical reaction taking place when acid rain…
  63. 5(b)(i)5 marks· Chemistry Q5 5(b)(i)To determine if zinc oxide is amphoteric
  64. 5(b)(ii)1 mark· Chemistry Q5 5(b)(ii)To determine if zinc oxide is an acid anhydride
  65. 5(c)3 marks· Chemistry Q5 5(c)Suggest the type of reaction that takes place when the magnesium oxide is mixed with the sour wine. Write a balanced chemical equation for this reaction.
  66. 5(c)(ii)1 mark· Chemistry Q5 5(c)(ii)Write an equation for the reaction between sulphur (IV) oxide and water.
  67. 5(c)(iii)2 marks· Chemistry Q5 5(c)(iii)State whether the salt formed will be soluble in water, giving a reason for your answer.
  68. 5(d)(i)2 marks· Chemistry Q5 5(d)(i)Give the name of ONE reagent that could be used for this purpose. Support your answer by writing a chemical equation, using ONE of the named pollutants mentioned above.
  69. 5(e)4 marks· Chemistry Q5 5(e)Briefly outline how a dry sample of the sulphate of Q can be prepared from a sample of the metal nitrate of Q. Include an ionic equation to illustrate your method of preparation.
  70. 6(a)2 marks· Chemistry Q6 6(a)Give TWO reasons why humans may need to cook their food.
  71. 6(b)(i)1 mark· Chemistry Q6 6(b)(i)State ONE problem associated with acidic soils.
  72. 6(b)(ii)2 marks· Chemistry Q6 6(b)(ii)Use a balanced ionic equation to explain how the addition of lime can increase the pH of acidic soils.
  73. 6(b)(iii)2 marks· Chemistry Q6 6(b)(iii)Baking soda, NaHCO₃, can also be used to tenderize meat. Suggest why this is possible.
  74. 6(b)(iii)3 marks· Chemistry Q6 6(b)(iii)Lime can also cause nitrogen to be lost from soils. State a reason for this. Include a balanced ionic equation with state symbols in your answer.
  75. 6(c)5 marks· Chemistry Q6 6(c)Suggest a possible explanation for this practice. Write ONE chemical equation to support this practice.
  76. 6(d)3 marks· Chemistry Q6 6(d)A description of a test of soil acidity.
  77. 6(e)2 marks· Chemistry Q6 6(e)The chemical name and formula for lime. Advise when lime should be used.
  78. 6(f)3 marks· Chemistry Q6 6(f)A reason why lime should NOT be added to the soil at the same time as a commercial ammonium fertilizer. Include a balanced chemical equation to support your answer.
  79. 7(a)(i)1 mark· Chemistry Q7 7(a)(i)State the importance of EACH of the following factors in plant growth: Mineral balance
  80. 7(a)(ii)1 mark· Chemistry Q7 7(a)(ii)State the importance of EACH of the following factors in plant growth: pH
  81. 7(a)(iii)2 marks· Chemistry Q7 7(a)(iii)State the importance of EACH of the following factors in plant growth: Humus content of the soil
  82. 7(b)(i)1 mark· Chemistry Q7 7(b)(i)Write the chemical formula for lime.
  83. 7(b)(ii)1 mark· Chemistry Q7 7(b)(ii)What is the effect of lime on the acidity of a soil?
  84. 7(b)(ii)4 marks· Chemistry Q7 7(b)(ii)The Officer finds the soil to be acidic and recommends the addition of lime. Suggest ONE possible reason for the acidic nature of the soil. Explain the effect of adding lime to the soil. Use a suitable equation to…
  85. 7(b)(iii)2 marks· Chemistry Q7 7(b)(iii)Write a balanced ionic equation to illustrate the action of lime on soil.
  86. 7(b)(iv)4 marks· Chemistry Q7 7(b)(iv)A cotton farmer recognizes that his soil needs more nitrogen, and lime, so he adds an ammonium fertiliser and lime to the soil at the same time. Explain how this action could cause nitrogen to be lost. Use a balanced…
  87. 7(c)3 marks· Chemistry Q7 7(c)Suggest ONE way in which lime can cause nitrogen to be lost from the soil. Include a balanced ionic equation in your answer.
  88. 7(c)5 marks· Chemistry Q7 7(c)The farmer, in addition to adding the recommended lime to the soil, also decides to add an ammonium fertilizer, thinking that it would increase his crop yield. Do you think that the farmer's decision to add both lime…
  89. 1(a)(i)2 marks· CSEC Chemistry · January 2002 · Paper 2Explain what is meant by a 'normal salt' and an 'acid salt'.
  90. 1(a)(ii)2 marks· CSEC Chemistry · January 2002 · Paper 2Describe a suitable test to distinguish between a normal salt and an acid salt.
  91. 1(b)(i)4.5 marks· CSEC Chemistry · January 2002 · Paper 2In preparing samples of barium sulphate and zinc sulphate, discuss the possibilities of using the action of acid on the metal.
  92. 1(b)(i) [P2]4 marks· CSEC Chemistry · January 2002 · Paper 2Read off the height of the precipitate present in EACH test tube in millimetre and record it on the table.
  93. 1(b)(ii)4.5 marks· CSEC Chemistry · January 2002 · Paper 2In preparing samples of barium sulphate and zinc sulphate, discuss the possibilities of using titration using acid and alkali.
  94. 1(b)(ii) [P2]6 marks· CSEC Chemistry · January 2002 · Paper 2Plot the results on the grid provided and draw the line of best fit.
  95. 1(b)(iv) [P2]3 marks· CSEC Chemistry · January 2002 · Paper 2Name the ions present in the SOLUTION in Test tube 6 on page 4.
  96. 1(c)(i)2 marks· CSEC Chemistry · January 2002 · Paper 2Giving full experimental details, outline a suitable method for preparing a sample of dry barium sulphate, specifying the reactions to be used.
  97. 1(c)(ii)3 marks· CSEC Chemistry · January 2002 · Paper 2Provide a description of the method for preparing the dry barium sulphate sample.
  98. 1(c)(iii)2 marks· CSEC Chemistry · January 2002 · Paper 2Write all relevant equations for the preparation of barium sulphate.
  99. 4(a) [P2]2 marks· CSEC Chemistry · January 2002 · Paper 2Write a balanced equation for the reaction between hydrochloric acid and marble chips.
  100. 4(d) [P2]2 marks· CSEC Chemistry · January 2002 · Paper 2Explain why nitric acid and NOT sulphuric acid could be used to replace the hydrochloric acid used in the investigation.
  101. Q41 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1Which of the following compounds is soluble in cold water?
  102. Q51 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1Which of the following oxides shows both acidic and basic properties?
  103. Q81 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1Which of the following is classified as a neutral oxide?
  104. Q371 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1Which acid functions as a dehydrating agent when concentrated?
  105. Q381 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1Which acid reacts with copper to produce an acidic, reddish-brown gas?
  106. Q471 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1Which of the compounds has a pH less than 7?
  107. Q491 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1A piece of limestone is treated with dilute hydrochloric acid. Which of the following would be observed? I. Effervescence occurs. II. A gas is evolved with a pungent odour. III. A gas is evolved which turns limewater…
  108. Q521 mark · multiple choice· CSEC Chemistry · January 2017 · Paper 1A solution has a pH of 1. This solution would be expected to react with
  109. Q41 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1Sulfuric acid is a stronger acid than ethanoic acid (acetic acid) in aqueous solution because sulfuric acid
  110. Q141 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1An acid can be defined as a
  111. Q171 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1Which of the following pairs of substances can represent solutions \text{X} and \text{Y}?
  112. Q251 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1Which of the following substances reacts with an acid, liberating a gas which turns lime water 'milky'?
  113. Q301 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1Which of the following elements form an acidic oxide when burnt in air? I. Aluminium II. Carbon III. Nitrogen
  114. Q311 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1When a piece of magnesium ribbon is burnt in air, magnesium oxide is formed. It is then placed in water and tested with litmus solution, which turns blue. The above experiment shows that magnesium oxide is
  115. Q561 mark · multiple choice· CSEC Chemistry · January 2018 · Paper 1Which of the following are reactions of ethanoic acid? I. It forms a salt with aqueous sodium hydroxide. II. It liberates carbon dioxide from a carbonate. III. It liberates hydrogen on contact with a strongly…
  116. Q51 mark · multiple choice· CSEC Chemistry · January 2019 · Paper 1Which of the following substances supplies protons as the only positive ions in aqueous solutions?
  117. Q71 mark · multiple choice· CSEC Chemistry · January 2019 · Paper 1The ionic equation for the reaction between an acid and a carbonate is represented by
  118. Q301 mark · multiple choice· CSEC Chemistry · January 2019 · Paper 1Which of the points on the graph above represents the neutralization point of the reaction?
  119. Q431 mark · multiple choice· CSEC Chemistry · January 2019 · Paper 1Which of the following compounds may be used to counteract the effects of acid rain on the soil?
  120. 1(c)2 marks· CSEC Chemistry · January 2021 · Paper 2Distinguish between a 'strong acid' and a 'weak acid'.
  121. 1(j)1 mark· CSEC Chemistry · January 2021 · Paper 2State ONE safety precaution that should have been taken during the experiment.
  122. 6(c)(i)3 marks· CSEC Chemistry · January 2021 · Paper 2Some farmers use ammonium sulfate fertilizers in the presence of a base. Explain why this is NOT a good practice.
  123. Q231 mark · multiple choice· CSEC Chemistry · May/June 2010 · Paper 1A specific base reacts with a salt to produce a gas which turns damp red litmus paper blue. Which of the following ions does the salt contain?
  124. Q241 mark · multiple choice· CSEC Chemistry · May/June 2010 · Paper 1Which of the following salts can be prepared by mixing two solutions and then filtering? I. Barium sulphate II. Calcium nitrate III. Silver chloride IV. Ammonium carbonate
  125. Q491 mark · multiple choice· CSEC Chemistry · May/June 2010 · Paper 1Sodium chloride solution is used in the laboratory preparation of soap to
  126. Q201 mark · multiple choice· CSEC Chemistry · May/June 2011 · Paper 1Sulphuric acid is a stronger acid than ethanoic acid (acetic acid) in aqueous solution because sulphuric acid
  127. Q211 mark · multiple choice· CSEC Chemistry · May/June 2011 · Paper 1Which of the following is NOT a normal salt?
  128. Q311 mark · multiple choice· CSEC Chemistry · May/June 2011 · Paper 1Which of the following elements does NOT react with \text{H}^+(\text{aq}) ions to give hydrogen gas?
  129. Q451 mark · multiple choice· CSEC Chemistry · May/June 2011 · Paper 1Ammonia may be produced in the laboratory by heating a mixture of ammonium chloride and
  130. Q31 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1Items 3-5 refer to the following types of substances. (A) Salt (B) Base (C) Alkali (D) Acid Match EACH item below with ONE of the options above. Each option may be used more than once, once or not at all. Which of the…
  131. Q41 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1Items 3-5 refer to the following types of substances. (A) Salt (B) Base (C) Alkali (D) Acid Match EACH item below with ONE of the options above. Each option may be used more than once, once or not at all. Which of the…
  132. Q51 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1Items 3-5 refer to the following types of substances. (A) Salt (B) Base (C) Alkali (D) Acid Match EACH item below with ONE of the options above. Each option may be used more than once, once or not at all. Which of the…
  133. Q191 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1The pH of fresh sugar cane juice which is usually 5.0–5.5 can be changed to 7.5–8.0 for more efficient processing by adding
  134. Q201 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1Which of the following salts is prepared by precipitation?
  135. Q211 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1Which of the following compounds is NOT a normal salt?
  136. Q221 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1A 'weak acid' is BEST described as one that yields a
  137. Q241 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1Which of the following salts are soluble in water? I. Ammonium carbonate II. Calcium sulfate III. Lead nitrate
  138. Q431 mark · multiple choice· CSEC Chemistry · May/June 2013 · Paper 1Ammonia may be produced in the laboratory by heating a mixture of ammonium chloride and
  139. Q171 mark · multiple choice· CSEC Chemistry · May/June 2015 · Paper 1A solution having a pH of 1 will
  140. Q191 mark · multiple choice· CSEC Chemistry · May/June 2015 · Paper 1A 'weak acid' is BEST described as one that yields a
  141. Q201 mark · multiple choice· CSEC Chemistry · May/June 2015 · Paper 1Which of the following methods may be used in the preparation of barium sulfate in the laboratory?
  142. Q211 mark · multiple choice· CSEC Chemistry · May/June 2015 · Paper 1Which TWO of the following statements describe acid salts? I. Their anions cannot dissociate to give hydrogen ions. II. They form a normal salt when all replaceable hydrogen of the acid is removed. III. Their anions…
  143. Q291 mark · multiple choice· CSEC Chemistry · May/June 2015 · Paper 1Which of the following substances is an amphoteric oxide?
  144. Q81 mark · multiple choice· CSEC Chemistry · May/June 2016 · Paper 1The disadvantage of using a soapless detergent is that it
  145. Q191 mark · multiple choice· CSEC Chemistry · May/June 2016 · Paper 1A solution has a pH of 1. This solution would be expected to react with
  146. Q211 mark · multiple choice· CSEC Chemistry · May/June 2016 · Paper 1Which of the following terms BEST describes the oxide of a metal?
  147. Q301 mark · multiple choice· CSEC Chemistry · May/June 2016 · Paper 1Which of the following oxides react with both acids and bases?
  148. Q81 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Which of the following acids will NOT form an acid salt?
  149. Q101 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Which of the following oxides may show both acidic and basic properties?
  150. Q201 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1The pH of fresh sugar cane juice, which is usually 5.0–5.5, can be changed to 7.5–8.0 for more efficient processing by adding
  151. Q211 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Which TWO of the following statements describe acid salts? I. Their anions cannot dissociate to give hydrogen ions. II. They form a normal salt when all replaceable hydrogen of the acid is removed. III. Their anions…
  152. Q401 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Which of the following processes correctly describes the equation above? \text{RCOOH}(\text{aq}) + \text{NaOH}(\text{aq}) \rightarrow \text{RCOONa}(\text{aq}) + \text{H}_2\text{O}(l)
  153. Q481 mark · multiple choice· CSEC Chemistry · May/June 2017 · Paper 1Soapless detergents are

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