Gravimetric Analysis
Chemistry ⇒ Analytical Chemistry
Gravimetric Analysis starts at 11 and continues till grade 12.
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See sample questions for grade 11
A sample containing sulfate ions is analyzed gravimetrically by precipitating as BaSO_4. If 0.233 g of BaSO_4 is obtained, calculate the mass of SO_4^{2-} in the sample. (Molar mass of BaSO_4 = 233 g/mol, SO_4^{2-} = 96 g/mol)
A sample of hydrated magnesium sulfate (MgSO_4 \cdot xH_2O) is heated until all water is lost. If the initial mass is 2.50 g and the final mass is 1.20 g, calculate the mass of water lost.
A sample of potassium chloride is analyzed gravimetrically by precipitating as AgCl. If 0.287 g of AgCl is obtained, calculate the percentage of KCl in the original 0.500 g sample. (Molar mass: AgCl = 143.5 g/mol, KCl = 74.5 g/mol)
A student is analyzing a sample for calcium by precipitating it as CaC_2O_4. If 0.250 g of CaC_2O_4 is obtained, calculate the mass of Ca^{2+} in the sample. (Molar mass of CaC_2O_4 = 128 g/mol, Ca = 40 g/mol)
A student obtained 0.400 g of PbSO_4 from a sample. Calculate the mass of Pb^{2+} in the sample. (Molar mass of PbSO_4 = 303 g/mol, Pb = 207 g/mol)
A student obtained 0.500 g of AgCl from a sample. Calculate the amount of Cl^{-} (in grams) present in the sample. (Molar mass of AgCl = 143.5 g/mol, Cl = 35.5 g/mol)
Define co-precipitation in the context of gravimetric analysis.
Describe the purpose of ignition in gravimetric analysis.
Describe the role of a desiccator in gravimetric analysis.
Explain why gravimetric analysis is considered a primary method of analysis.
Explain why it is important to use a pure and stable precipitate in gravimetric analysis.
Explain why slow addition of the precipitating agent is preferred in gravimetric analysis.
Name one common precipitating agent used in gravimetric analysis for chloride ions.
State one reason why the precipitate is washed with distilled water during gravimetric analysis.
What is gravimetric analysis?
