During a lab, you heat 1.04 g of a niso4 hydrate over a bunsen burner. after heating, the final mass of the dehydrated compound is 0.61 g. determine the formula of the hydrate and also give the full name of the hydrate.

Question

Chemistry

Landen Arroyo

19 January, 11:11

During a lab, you heat 1.04 g of a niso4 hydrate over a bunsen burner. after heating, the final mass of the dehydrated compound is 0.61 g. determine the formula of the hydrate and also give the full name of the hydrate.

+2

Answers (1)

Know the Answer?

Jaxon Weaver · Answer 1

The difference between the initial mass (1.04 g) and the final mass (0.61g) is the mass of water present in the sample:

1.04 g - 0.61 g = 0.43 g

Divide by the molar mass of water: 18.01 g / mol to obtain the number of moles of water:

0.43 g / 18.01 g / mol = 0.0239 moles

Calculate the number of moles of dehydrated NiSO4

Number of moles = mass in grams / molar mass

molar mass of NiSO4 = 154.75 g/mol

number of moles NiSO4 = 0.61 g / 154.75 g/mol = 0.00394 moles

Now determine the molar ratio water to NiSO4: 0.0239 / 0.00394 = 6.07 ≈ 6

Then, the formula of the hydrate product is NiSO4 · 6 H2O.

Use the prefix hexa (6) to name the compound: Nickel (II) sulfate hexadydrate