From the masses of the water and anhydrous solid and the molar mass of the anhydrous solid (the formula of the anhydrous solid will be provided), the number of moles of . We believe our hydrate was magnesium sulfate, because the unknown hydrate was more closely related in physical appearance to that of magnesium sulfate, compared to the the three other options. Answer 2) A hydrate that . Masses are measured beforeheating to determine the mass of theoriginal sample (the hydrate)andafterheating to determine the mass of copper (II) sulfate (CuSO4) anhydrous. TPT empowers educators to teach at their best. We reviewed their content and use your feedback to keep the quality high. We could have not gotten rid of the water in the hydrate to begin with as 15 minutes of heating was perhaps too short. Calculate the percent by mass of water by dividing the mass of H 2 O in 1 mole of the hydrate by the molar mass of the hydrate and multiplying by 100%. From the calculation, you can clearly see that the units of g/mol in the numerator and denominator cancel out. In order to determine the formula of the hydrate, [\(\text{Anhydrous Solid}\ce{*}x\ce{H2O}\)], the number of moles of water per mole of anhydrous solid (\(x\)) will be calculated by dividing the number of moles of water by the number of moles of the anhydrous solid (Equation \ref{6}). Calculate the Average % of Water in the Hydrate Samples. Hydrate Lab - Google Docs The hydrate was heated until all the water evaporated, and the mass of the remining anhydrous salt was measured. 6. Before this, we had heard of this scientific word briefly in textbooks and in class, but we were never sure of its exact definition. for the imperialist) and position the flame under the crucible so that the inside blue When hydrates are heated, the water is released from the compound as water vapor. 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water.
