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if you have Ca(NO3)2 times xH2O do u count the Hydrate when looking for the mass % of Ca
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Yes, the hydrate counts in the mass of the crystal.
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I need help with this lab.
Write the equation for the decomposition of the hydrate, CuSO4*XH2O. Mass of crucible and hydrate:
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If you have no more data than this I can't figure it out either. 93.000 g = mass xble + hydrate
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I need help with this lab.
Write the equation for the decomposition of the hydrate, CuSO4*XH2O. Mass of crucible and hydrate:
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You don't have enough information here. 1. mass H2O = 93.000-91.196 = ? 2. mols H2O = grams
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A hydrate of zinc nitrate has the formula Zn(NO3)2 . xH2O. If the mass of 1 mol of anhydrous zinc nitrate is 63.67% of the mass
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if 4.36g of a hydrate of the salt baCl2 is heated and in the process losses 0.6431g of mass, show all your work to calculate the
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BaCl2*2H2O --> BaCl2 +2H20 4.36g ............... 3.72 ... 0.643g Convert each of the mass of product
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If 4.36g of a hydrate of the salt baCl2 is heated and in the process losses 0.6431g of mass, show all your work to calculate the
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To calculate the amount of water (X) in the hydrate BaCl2.XH2O, we need to determine the mass of
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So I did a lab determining the chemical formula of a hydrate. I really just need somebody to check this over for me. We had to
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Would the answer somehow differ if I had different amounts than the person on the link you posted?
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If a 8.6195 g of a mixture which contains (20.0 % of CuSO4.XH2O and 80.0 % of sand) was heated in
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please help me ,becauce i have final exam tomorrow
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A hydrate of copper (II) sulfate with formula CuSO4.xH2O has a molar mass of 250.0 g/mol. 2.545 g of hydrate is heated and
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CuSo4.xHO
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I don't understand these two questions. Any help on how to figure this would be great. Thanks.
1. Write the equation for the
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USUALLY, when asked to write the decomposition for hydrates, we mean to remove the water to make the
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