ijmb model questions vol1 2024 chemistry | Practical

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Question 1 View Details
A mass spectrometer was used to analyse a sample of an unknown element X. The instrument gave the following data for the two most abundant isotopes: | Isotope (m/z) | Relative abundance | |---------------|--------------------| | 35.0 | 75.8 % | | 37.0 | 24.2 % | Using this information, answer the questions below.
Question Parts
(a)
Calculate the relative atomic mass of element X.
(b)
From the periodic table, suggest the most probable identity of element X and give its group and period.
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Question 2 View Details
A gravimetric analysis was carried out to determine the equivalent weight of an unknown metal M. Procedure summary: 1. A 0.500 g sample of the metal was dissolved in excess hydrochloric acid. 2. The solution was evaporated to dryness and the residue was heated to convert the metal to its chloride, MCl₂·6H₂O. 3. The dried crystals of the hydrate were weighed and gave a mass of 0.845 g. The formula mass of MCl₂·6H₂O is 203.3 g mol⁻¹. Answer the questions below.
Question Parts
(a)
Calculate the equivalent weight of metal M.
(b)
Using the periodic table, propose a possible identity for metal M and give its symbol, atomic number and common oxidation state.
(c)
Discuss two possible sources of error in this experiment and explain how each would affect the calculated equivalent weight.
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Question 3 View Details
An unknown white solid (X) is to be identified. The following experimental procedures were carried out: 1. 1.00 g of X was added to 100 mL of distilled water and the mixture was stirred. Conductivity of the filtrate was measured as 0.85 µS·cm⁻¹. 2. Solubility observation: X dissolved only sparingly, leaving a slight residue. 3. A flame test on a small amount of the solid produced an orange‑red flame. 4. The aqueous filtrate was treated with excess aqueous AgNO₃ solution. The precipitate formed was filtered, dried and weighed. The mass of AgCl obtained was 1.29 g. Using the above information, answer the questions that follow.
Question Parts
(a)
State the two qualitative tests performed and record the observations obtained for each.
(b)
From the observations in part (a), deduce the type of bonding present in X and suggest the probable metal ion present.
(c)
Using the mass of AgCl obtained, calculate the empirical formula of the unknown compound X.
(d)
Suggest two possible sources of error in this experiment and explain how each could affect the calculated formula.
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Question 4 View Details
A 25.00 mL sample of an unknown hydrochloric acid solution was titrated against a standard sodium hydroxide solution. The NaOH solution was standardized as 0.1000 M. During the titration, the endpoint (phenolphthalein colour change) was reached after the addition of 30.25 mL of the NaOH solution. Using this data, answer the questions that follow.
Question Parts
(a)
Calculate the number of moles of NaOH that were used in the titration.
(b)
Determine the molarity of the HCl solution.
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