Hydration and Water of Crystallization Calculations
Chemistry ⇒ Stoichiometry and Chemical Calculations
Hydration and Water of Crystallization Calculations starts at 10 and continues till grade 12.
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A 2.50 g sample of hydrated cobalt(II) chloride, CoCl_2·xH_2O, is heated to give 1.25 g of anhydrous CoCl_2. Calculate the value of x.
A 3.22 g sample of hydrated sodium carbonate, Na_2CO_3·xH_2O, is heated to give 1.20 g of anhydrous Na_2CO_3. Calculate the value of x.
A 4.50 g sample of hydrated iron(II) sulfate, FeSO_4·xH_2O, is heated to give 2.45 g of anhydrous FeSO_4. Calculate the value of x.
A 5.00 g sample of hydrated barium chloride, BaCl_2·xH_2O, is heated to constant mass. The mass of the anhydrous salt is 4.26 g. Calculate the value of x.
A 7.50 g sample of hydrated sodium thiosulfate, Na_2S_2O_3·xH_2O, is heated to give 3.30 g of anhydrous Na_2S_2O_3. Calculate the value of x.
A hydrated salt has a mass of 10.0 g. After heating, the mass is 6.0 g. If the molar mass of the anhydrous salt is 120 g/mol, calculate the number of moles of water lost per mole of salt.
A hydrated salt has a molar mass of 322 g/mol and its anhydrous form has a molar mass of 194 g/mol. How many water molecules are present per formula unit?
A hydrated salt has the formula AB_2·xH_2O. If 8.00 g of the hydrated salt gives 5.00 g of anhydrous AB_2 after heating, and the molar mass of AB_2 is 100 g/mol, calculate the value of x.
A hydrated salt has the formula CaCl_2·xH_2O. If 7.35 g of the hydrated salt yields 4.44 g of anhydrous CaCl_2 after heating, what is the value of x?
A hydrated salt has the formula MCl_2·xH_2O. If 5.00 g of the hydrated salt gives 2.70 g of anhydrous MCl_2 after heating, and the molar mass of MCl_2 is 95 g/mol, calculate the value of x.
A sample of hydrated magnesium sulfate, MgSO_4·xH_2O, has a mass of 6.16 g. After heating, the mass of the anhydrous salt is 3.00 g. Calculate the value of x.
A student heats 2.50 g of hydrated sodium sulfate, Na_2SO_4·xH_2O, and obtains 1.10 g of anhydrous Na_2SO_4. Calculate the value of x.
Calculate the percentage by mass of water in CuSO_4·5H_2O.
Describe how you would experimentally determine the percentage of water in a sample of hydrated salt.
Describe the steps involved in determining the formula of a hydrated salt experimentally.
Explain the difference between a hydrated and an anhydrous salt.
Explain why hydrated salts often have different colors compared to their anhydrous forms.
Explain why it is important to heat a hydrated salt to constant mass when determining its formula.
Explain why some salts become powdery when exposed to air.
Explain why the mass of a hydrated salt decreases upon heating.
