Weight Empty Beaker Wt Beaker +Cu sample before heating Wt. Beaker+ Cu sample af

Question

Weight Empty Beaker Wt Beaker +Cu sample before heating Wt. Beaker+ Cu sample after Heating 34.5910 40.5089 38.3903 CuSO Wi Ssangk3793 5.9179 Wt after heating Wt H2O 2.1186 % Water 35.80% 36.08%) Theoretical Copper(II) Sulfate Final answer 5.91 Mass of copper sulfate hydrate Mass of copper sulfate anhydride Calculate mass of water Calculatethe-r assof ter- 100%*( asswater)/(masshydrate) -35-30% Molar mass of water (H-0) Molar mass of CusOs te) - (mass anhydride Sum of masses of 2 H and 10 sum of masses of Cu. S and 4 O -1159.40 l massa hydride)/ 01 r. ass cusalo oa38 mass water)/( molar mass of water) 7 Moles of anhydride Moles of water f water to anhydride (moles water)Y(moles of anhydride) 4.2903C Based on the ratio calculated above Empirical formula and name of the compound (True -actual value)/(true value)1002 % Error using % water You must show your work below

Explanation / Answer

10. Molar mass of copper sulphate anhydrous (CuSO4) is : 159.609 g/ mole

Mass of anhydrous copper sulfate= 3.7993 grams

3.7993 grams of CuSO4 = (3.7993 / 159.609) moles = 0.0238 mole of CuSO4

Mass of water attached in hydrated copper sulphate = 2.1186 grams

Molar mass of water = 18.01 g/ mole

2.1186 grams of water = (2.1186/ 18.01 ) mole = 0.1177 mole

So, in the hydrated salt: 0.0238 moles of copper sulphate is attached to 0.1177 moles of water

So, in the hydrated salt , 1 mole of copper sulphate is attached to (0.1177/ 0.0238) moles = 5 moles of water

So, in the salt each CuSO4 molecule is attached to 5 H2O molecules

So, the empirical formula of the salt is CuSO4.5H2O. Name : copper sulphate pentahydrate

11. Actual formula of the hydrated salt is CuSO4.6H2O

% error using water = 100* (6-5)/ (6) = 16.67%

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