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2 marksAcids, Bases and Salts

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

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.

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.

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Other parts of this question

  1. 1(a)(i)Define the term 'normal salt'.[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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