Answer :
To obtain the complete formula for the iron (III) chloride hydrate, we need the molar masses of iron (III) chloride and water. With this information, we can calculate the empirical formula as FeCl3·xH2O.
To determine the complete formula for the iron (III) chloride hydrate, we need to calculate the molar ratios between iron (III) chloride and water.
Mass of iron (III) chloride hydrate = 4.23 g
Mass of water = 1.69 g
First, we need to calculate the moles of iron (III) chloride and water:
Moles of iron (III) chloride = mass / molar mass of iron (III) chloride
Moles of iron (III) chloride = 4.23 g / molar mass of iron (III) chloride
Moles of water = mass / molar mass of water
Moles of water = 1.69 g / molar mass of water
Next, we need to find the simplest whole-number ratio between moles of iron (III) chloride and moles of water.
Divide both moles by the smaller value obtained:
Moles of iron (III) chloride (FeCl3) = moles of iron (III) chloride hydrate / smaller value
Moles of water (H2O) = moles of water / smaller value
Finally, we can determine the empirical formula by writing the ratio of moles as subscripts:
Empirical formula = FeCl3·xH2O
The value of x represents the number of water molecules associated with one formula unit of iron (III) chloride.
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