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1. Metal sulfates are hygroscopic and will absorb water from the atmosphere. As a result, they must be kept in desiccators to keep them dry. Suppose, hypothetically, that the unknown metal sulfate was not desiccated. Would this error lead you to obtain a higher mass % of sulfate or a lower mass % of sulfate in the unknown? Explain. 2. In this experiment, an excess of the BaCl2 solution was added to the metal sulfate solution. Suppose, hypothetically, that an excess of the BaCl2 solution was not used. Would this error lead you to obtain a higher mass % of sulfate or a lower mass % of sulfate in the unknown? Explain. 3. The last step of the procedure involved vigorously heating the BaSO4 precipitate and filter paper in the crucible. Suppose, hypothetically, that tiny pieces of the filter paper still remained mixed in with the BaSO4 after heating. Would this error lead you to obtain a higher mass % of sulfate or a lower mass % of sulfate in the unknown? Explain. 4.An unknown metal sulfate is analyzed and determined to be 72.07% sulfate by mass. Assuming that the charge on the metal cation is +3, determine the identity of this metal cation.

Sagot :

Actual amount of sulfates show lower mass percentage of sulfate and less amount of BaSO4 will be formed and if tiny pieces of filter paper remains in the BaSO4 leading to less mass % of sulfates.

When metal sulfates are hygroscopic and will absorb water from the atmosphere as a result they must be kept in desiccators to keep them dry. the unknown metal sulfate was not desiccated. If the sulfate not desiccated the total weight will be higher for a sulfate . So actual amount sulfate will show lower mass % of sulfate. if excess of BaCl2 is not used, it would lead to lower mass % of sulfate as BaCl​2 will be the limiting reagent so less amount of BaSO4 will be formed. if tiny pieces of filter paper remains in the BaSO4 residue it will so higher mass altogether leading to less mass % of sulfates.

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