a 3.211 g sample of gypsum a hydrated salt of magnesuim sulfate, MgSO4.XH2OIS HEATED IN A CRUCIBLE UNTIL A CONSTANT MASS IS REACHED . THE MASS OF THE ANHYDROUS MgSO4 IS 2.539g
a) calculate the percentage by the mass of water in the hydrated MgSO4.xH2O
b) calculate the moles , the amount of H2O released during heating and the amount (in moles) of the anhydrates MgSO4 remaining after heating
c) calculate the value of x in MgSO4.xH2O/ This is the empirical formula of the hydrated magnesium sulfate

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pstnonsonjoku pstnonsonjoku · Answer 1 · 2022-07-21T17:05:04+02:00

From the calculation, the compound is MgSO4.2H2O.

A hydrated salt is a salt that contains molecules of the water of crystallization.

a) Percentage of the water of crystallization = 3.211 g - 2.539g/ 3.211 g * 100/1 = 21%

b) Number of moles of water of crystallization = 3.211 g - 2.539g/ 18 g/mol =

0.037 moles

c) Number of moles of anhydrous salt = 2.539g/120 g/mol = 0.021 moles

Number of moles of hydrated salt = 3.211 g/120 + 18x

Hence;

0.021 = 3.211 /120 + 18x

0.021(120 + 18x) = 3.211

2.52 + 0.378x = 3.211

0.378x = 3.211 - 2.52

x = 3.211 - 2.52/ 0.378

x = 2

Hence the compound is MgSO4.2H2O

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