# Formula Of Sulfate

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Determining the Chemical Formula of Hydrated Copper (Ⅱ) Sulfate Using the Empirical Formula

Introduction

In this experiment, the molecular formula of hydrated Copper (Ⅱ) Sulfate will be determined.

In order to determine the molecular formula, the empirical formula is needed which is the ratio of moles of one substance to another. In this experiment, it is the ratio of Copper (Ⅱ) Sulfate to water.

CuSO₄・XH₂O

The empirical formula can be determined if the moles of the compared substances are calculated and then divided by the smallest mole. Since there are large quantities of particles in any given substance, the mole is a unit used to group particles to make it easier to calculate large numbers. The amount of particles in one mole is
The mass of the element divided by the total mass of the compound equals to the percent mass.

Percent mass of H₂O = 0.160.355 = 0.45 = 45%

Therefore, the average percent mass of hydrate is 45 percent.

The percent mass calculated in this experiment will not be similar to the results of other groups. Since the percent mass calculated is an average, it is most likely that the number calculated is different from the actual number of hydrates in the formula. In addition, all the masses calculated are subject to possible random errors which would differ our results from those of others. Otherwise, in the theoretical situation, our percent mass would be the same since the amount of hydrate is the same across all