Question

If a Crystalline Compound Contains molecules of water and if produces 6.54g of its anhydrous salt when heated to 110°C and to of water. Determine the molar mass of the compound if the cation is xts and the anion is 50%. Suggest the formula of the compound.

Answer 1

The empirical formula of the compound is CoCl2 · 2H2O and the molecular formula is CoCl2 · 4H2O.

Step-by-step explanation:

To determine the empirical formula of the compound, we need to find the ratio of the number of moles of water molecules to the number of moles of the anhydrous salt formed. This can be done by dividing the mass of water by its molar mass and dividing the mass of the anhydrous salt by its molar mass. In this case, the empirical formula of the compound is CoCl2 · 2H2O.

To determine the molecular formula of the compound, we need to know the molar mass. In this case, the molar mass is given as 94.1 g/mol. To find the ratio of the molar mass of the compound to the molar mass of the empirical formula, divide the given molar mass by the molar mass of the empirical formula. If the ratio is a whole number, multiply the subscripts in the empirical formula by that number. In this case, the molecular formula of the compound is CoCl2 · 4H2O.