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formula of the hydrate shows the ratio of the moles of anhydrous salt to the moles of water; in the above case, that ratio is 1:5. In this experiment, you will be given a sample of hydrate.
You weight out a 0.470-sample of hydrated nickel(II ) chloride, NiCl 2 ·xH 2 O. Upon heating, the mass of the anhydrous salt that remains is 0.256 grams. What is the formula of the hydrate? What is the name of the hydrate? Answer
Examples 2 and 3 below compares the use of anhydrous, meaning no water, and monohydrate, meaning having one water of crystallisation, solids of the same compound for preparation of 250 mL of 0.2 M solutions.
Hydrate salts have chemical formulae such as OsCl3·3 H2O (osmium (III) chloride trihydrate) or Cs2S·4 H2O (cesium sulfide tetrahydrate). In these formulae, the dot indicates a weak chemical bond that is easily broken by heating the sample.
7 Αυγ 2011 · The formula of the anhydrous salt is known, so its formula weight can be calculated. The weight of the material in the crucible after heating can then be used to determine the number of moles of the anhydrous salt. Comparing these two mole numbers gives the complete formula of the hydrated salt. Dividing the moles of water by the moles of ...
Record the identity of your anhydrous salt (SrCl2, MgSO4, K2CO3, or ZnSO 4 ) based on the results of your flame test and magnesium strip test on the line below (A6).
1. Calculate the mass of each hydrated salt sample by difference. 2. Calculate the mass of water lost as the difference between the mass of the hydrated salt and the mass of the anhydrous salt. 3. Calculate the percentage of water by mass in each sample: % water = (weight of water lost÷weight of hydrated salt) X 100
