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A 1.232 g sample of a magnesium sulfate hydrate is heated until its final mass is...
Suppose you want to know the formula of a hydrate of magnesium sulfate. If you heat 1.998 g of the hydrate until all of the water is vaporized, the mass of anhydrous MgSO4 is 0.976 g. What is the formula of the hydrate, i.e. what is the value of x in MgSO4.xH2O? (The formula weight of anhydrous magnesium sulfate is 120.37 g/mol)
Question five A 15.67 g sample of a hydrate of magnesium carbonate ( MOONH:O) was heated without decomposite the carbonate, to drive off the water. The mass was reduced to 7.58 g (Molar mass of MgCO: - 84313 Smol) (5 mark) A. What is the formula of the hydrate? B. Determine the percentate in the hydrated sit
15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate? Name the hydrate
H20 MASS of H20 2.09 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula.
Metal Sulfate Hydrate lab (12 points) 4) An unknown metal sulfate hydrate (MSO XHO) sample with the recorded mass below is dissolved in water, and the sulfate ions from the sample precipitated with Ba2+ ions as BaSO4. A pre-massed filter paper is then used to collect the solid BaSO4. Experimental data was recorded below following same procedure in MSH lab. 0.6939 96.06 g/mol Molar mass of SO42- PARTA Mass of unknown metal sulfate hydrate (MSH) Mass of unknown sample sulfate...
A 6.2351 g sample of an unknown hydrate of cobalt(II) bromide is heated until all the water of hydration is removed. The CoBr2 that remains has a mass of 5.0000 g. 1. How many moles of CoBr2 are in the sample? mol 2. How many grams of water were lost in the dehydration? g 3. How many moles of water were lost? (mol) 4. What is the value of "n" in the formula CoBr2 · n H2O? (1, 2, 3,...
Need all calculations. Please make sure to make a table and show all working thanks A clean and empty beaker has a mass of 12.784 g. The beaker and hydrate have a mass of 15.895 g. After heating, the beaker and anhydrous salt have a mass of 13.889 g. What is the formula of this hydrate of magnesium sulfate MgSO4 ? H2O ? H20 18.01 g/mol MgSO4 120.37 g/mol 12.784 g Mass of Beaker 1. 2. Mass of Beaker and...
Part one's hydrate is Magnesium Sulfate. Part 2's hydrate is Copper (II) Sulfate. ID of Unknown Hydrate: Magnesium sulate Collection of Data This data must be collected to 0.0001 g precision on the analytical balances situated in the balance room. Mass of crucible and cover: 12.0385a Mass of crucible: Mass of cover: 5.3550 g 6,6835a 14.0320g Mass of crucible, cover and unknown hydrate: Mass of unknown hydrate: Mass of crucible, cover and residue After 1st heating period: After 2nd heating...
1. 51.8 g of magnesium sulfate heptahydrate is heated in an oven until all the water is driven off. What is the mass of the anhydrous compound?. 25.2 g 10.6 g O27.3g 24.5 g 26.5 g
Please explain. Thank you. (1) When a sample of ferric sulfate hydrate (EeSO4 XH20(s)) is heated to 270 C in an otherwise empty 625-mL container, it decomposes into ferric oxide (EeO(s), M 71.85 g/mol), sulfur trioxide (SO3(g), M = 80.06 g/mol), and water vapor (H20(g) 18.02 g/mol) wwwww = M = FESO4 XH2O(s) FeO(s) SO3(g) x H20 (g) wwwww www When all the FeSO4xH2O(s) in the sample decomposes, 1.80 g of FeO(s) forms and the total pressure of all gases...