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Design an experiment to accurately determine the empirical formula of a given hydrate. Predict how experimental factors will impact the accuracy and precision of results. Calculate the molar ratio of water to anhydrous solid to determine the hydrate's formula.
- 1.7: Experiment 6
Design an experiment to accurately determine the empirical...
- 1.7: Experiment 6
Example #1: A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate? Solution: 1) Determine mass of water driven off: 15.67 − 7.58 = 8.09 g of water. 2) Determine moles of MgCO 3 and water:
A student carries out an experiment to determine the amount of water of crystallisation in the formula of hydrated salt. The student intends to remove the water by heating the hydrated salt. diagram of the apparatus used by the student is shown below.
7 Ιουν 2024 · Worked example. Calculating water of crystallisation. 11.25 g of hydrated copper sulfate, CuSO4.xH2O, is heated until a constant mass of 7.19 g. Calculate the formula of the hydrated copper (II) sulfate. Ar (Cu) = 63.5 Ar (S) = 3. Ar (O) = 16 Ar (H) = 1. Answer: Examiner Tip.
Design an experiment to accurately determine the empirical formula of a given hydrate. Predict how experimental factors will impact the accuracy and precision of results. Calculate the molar ratio of water to anhydrous solid to determine the hydrate's formula.
Determine how many molecules of water of crystallization are present in the sample and thus deduce the chemical formula of hydrated copper(ll) sulfate. Solution: 31.8 g + 48.0 g = 79.8 g (the mass of the anhydrous CuSO 4 )
In this experiment, a hydrated salt will be heated to constant weight, removing the water of hydration. The loss of mass will be the mass of water present in the original salt. Using the mass of the water in the sample, the molar mass of water, the mass of the anhydrous salt, and the formula of the
