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  1. chem.libretexts.org › Courses › University_of_Arkansas_Little_Rock2.12: Hydrates - Chemistry LibreTexts

    Formula of a Hydrate (\(\text{Anhydrous Solid}\ce{*}x\ce{H2O}\)) The formula of a hydrate can be determined by dehydrating a known mass of the hydrate, then comparing the masses of the original hydrate and the resulting anhydrous solid.

  2. 22 Σεπ 2021 · The formula of a hydrate can be determined by dehydrating a known mass of the hydrate, then comparing the masses of the original hydrate and the resulting anhydrous solid. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate (\ref{3}):

  3. What is the formula of the hydrate? Solution: 1) Determine mass of water driven off: 15.67 − 7.58 = 8.09 g of water. 2) Determine moles of MgCO 3 and water: MgCO 3 ---> 7.58 g / 84.313 g/mol = 0.0899 mol H 2 O ---> 8.09 g / 18.015 g/mol = 0.449 mol.

  4. 2 Νοε 2023 · Salts that contain water within their structure are called hydrated salts. Anhydrous salts are those that contain no water in their structure. A common example is copper (II) sulfate which crystallises forming the salt hydrated copper (II) sulfate, which is blue.

  5. Design an experiment to accurately determine the empirical formula of a given hydrate. Predict how experimental factors will impact the accuracy and precision of results. Calculate the molar ratio of water to anhydrous solid to determine the hydrate's formula.

  6. We can find the percent of water in a hydrate experimentally by accurately determining the mass of the hydrate and the mass of the anhydrous salt. The difference in mass is due to the water lost by the hydrate.

  7. Solution: (a) What was the mass of the anhydrous salt? 16.499 g − 15.807 g = 0.692 g. (b) How many moles of anhydrous salt is this? 0.692 g / 133.341 g/mol = 0.0051897 mol (carry some extra digits) (c) What was the mass of the water driven off? 17.061 g − 16.499 g = 0.562 g. (d) How many moles of water is this?

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