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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
Example #3: A compound is found to have the formula XBr 2,...
- Calculate Empirical Formula When Given Mass Data
Example #2: On analysis, a compound with molar mass 60 g/mol...
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Determine the formula of a hydrate Hydrate lab calculations....
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Problem #5a: A solution was made by dissolving 52.0 g of...
- The Mole
Determine formula of a hydrate; Hydrate lab calculations....
- Hydrate Lab Calculations
Example #2: Solid copper(II) chloride forms a hydrate of...
- 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.
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).
A hydrate is a compound that has one or more water molecules bound to each formula unit. Several examples include sodium carbonate decahydrate (Na2CO3 •10H2O), also known as washing soda; magnesium sulfate heptahydrate (MgSO4 •7H2O), commonly called Epsom salt; and calcium sulfate dihydrate (CaSO4 • 2H2O), which is known as gypsum.
Example #2: Solid copper(II) chloride forms a hydrate of formula CuCl 2 ⋅ xH 2 O. A student heated a sample of hydrated copper(II) chloride, in order to determine the value of x. The following results were obtained: mass of crucible = 16.221 g mass of crucible and hydrated copper(II) chloride = 18.360 g
17 cze 2023 · A hydrate contains a definite number of water molecules bound to each ionic compound (also called the anhydrous salt). The formula of the hydrate is represented by the formula of the anhydrous salt followed by a dot and x H 2 O, where x is the number of moles of water per mole of the anhydrous salt. The hydrate is named by naming the anhydrous ...
Determine the hydrate's chemical formula (number of waters attached). Solution: 1) Mass of H 2 O removed after heating = mass of hydrate − mass of anhydrate
