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2 marksAcids, Bases and Salts

CSEC Chemistry · January 2014 · Paper 2 · Question 1(a)(i)

Students are preparing a normal salt by reacting aqueous sodium hydroxide with dilute sulfuric acid. They are provided with a dilute solution of sulfuric acid (4.9 g dm⁻³), 5 g of sodium hydroxide, and methyl orange indicator. They follow a procedure involving titration.

Define the term 'normal salt'.

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Other parts of this question

  1. 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…[2 marks]
  2. 1(a)(iii)State the name of ONE other acid that can also produce the type of salt identified in (ii) above.[1 mark]
  3. 1(b)(i)Complete Table 1 by using the readings shown in Figure 1.[2 marks]
  4. 1(b)(ii)Determine the volume of acid used to neutralize 25 cm³ of NaOH.[1 mark]
  5. 1(b)(iii)Explain why NO indicator was used in the procedure in Part B.[1 mark]
  6. 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.[2 marks]
  7. 1(b)(v)Write a balanced equation for the formation of the normal salt from sulfuric acid and sodium hydroxide.[2 marks]
  8. 1(b)(vi)Calculate the number of moles of sulfuric acid used to neutralize the sodium hydroxide.[3 marks]
  9. 1(b)(vii)Calculate the mass of the normal salt expected from the reaction.[2 marks]
  10. 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…[1 mark]
  11. 1(b)(ix)The students noticed that when the sodium hydroxide solution was made in Part A, the volumetric flask got warm. Draw an energy profile diagram to show the heat…[3 marks]
  12. 1(c)Complete Table 2 by inserting the inference and writing an ionic equation as indicated.[3 marks]

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