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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.
- Determine Identity of an Element From a Binary Formula and a Percent Composition
2) Subtract weight of the two bromines: 223.3515 − 159.808 =...
- Calculate Empirical Formula When Given Mass Data
Example #2: On analysis, a compound with molar mass 60 g/mol...
- Calculate Empirical Formula When Given Percent Composition Data
O ---> 3.1212 / 1.5608 = 2. 4) Write the empirical formula:...
- Determine Identity of an Element From a Binary Formula and a Percent Composition
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.
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A hydrate can usually be converted to the anhydrous compound by heating. For example, the anhydrous compound cobalt (II) chloride is blue, while the hydrate is a distinctive magenta color (as seen below). The hydrated form of cobalt (II) chloride contains six water molecules in each formula unit.
30 kwi 2018 · For example, the chemical formula of anhydrous copper (II) sulfate is Cu(SO 4). The molar mass of this compound is equal to the molar mass of copper plus the molar mass of sulfur plus four times the molar mass of oxygen (since there are four oxygen atoms in the molecule).
17 cze 2023 · Calculate the percent water of hydration of your unknown hydrate sample from each determination and take the average, if you did two. Obtain the identity of the unknown from your instructor. Calculate the percent water of hydration from the chemical formula. How does this compare with your experimental data? 8.0 POST-LAB QUESTIONS AND CONCLUSIONS
22 wrz 2021 · 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.
