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How would the empirical formula of copper (II) sulfate be affected if some of the sample sticks to the stirring rod?
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Some of what sample sticks to what stirring rod and how was it used?
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A chemist heats a sample of copper(II) sulfate and finds that 63.9% of the mass is copper(II) sulfate and the other 36.1% by
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Take a 100 g sample to give you 63.9 g CuSO4 and 36.1 g H2O Convert to mols. mols CuSO4 =
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3.05g of hydrated copper sulfate produces 1.94g of anhydrous copper sulfate.Assuming complete removal of all water of
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Still haven't received my answer to my questions
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a sample of anhydrous copper 2 sulphate contains 6.54g copper 3.2g sulphur and 6.4g oxygen determine the empirical formula of
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To determine the empirical formula, we need to find the ratio of the elements present in the
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A 2.50 gram sample of bronze was dissolved in sulfuric acid. The copper in the sample reacted with sulfuric acid to form copper
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moles S2O3^-2 = M x L = 0.0315*1M = 0.0315. Now you want to convert this to moles Cu, using the
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A 1.250 g sample of copper wire was heated in air and reacted with oxygen to give 1.565 g of copper oxide product. Calculate the
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When I worked the question I got cu = 0.0196 and o= 0.0196 so the empirical formula is CUO
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You have been asked to do a dilution of a copper sulfate solution. The solution to be diluted is 2.88 M copper sulfate.
What
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To determine the volume of the 2.88 M copper sulfate solution required to make a 250 mL of 1.03 M
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Determine the percent by mass of water in your sample of hydrated copper (II) sulfate.
Mass of water = 0.95 g Mass of anhydrous
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% H2O = (mass H2O/mass sample)*100 = ?
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3.05 g of hydrated copper sulfate produce 1.94 g of anhydrous salt. Assuming complete removal of water of crystallisation,
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To determine the formula of hydrated copper sulfate, we need to analyze the information given and
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3.05 g hydrated copper sulfate produces 1.94 g of anhydrous salt.Assuming complete removal of all water of
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3.05 g - 1.94 = 1.11 g H2O abd 1.94 g CuSO4 mols H2O = grams H2O/molar mass H2O mols CuSO4 = grams
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The mass of the CuSO4 x 5H2O sample is 1.664 g. The mass of the recovered copper is 1.198 g.
1. Compute the experimental percent
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Something is haywire here. mass sample = 1.664 g. mass recovered Cu = 1.198 g. percent Cu =
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Back again with another problem :)
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