0.8102 g sample of impure Al2(CO3)3 (MM= 234 g/mol) decomposed with HCl; the liberated CO2 was collected on calcium oxide (CaO, MM = 56 g/mol) and precipitated as CaCO3 (MM =100 g/mol). The precipitated was weigh to 0.0515 g. Calculate the percent of aluminium (atomic mass = 27 amu) in the sample. (Express answer in proper significant figures and do not include units.)

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A: The reaction given is Al4C3(s)  +   H2O(l)    ⟶ Al(OH)3(s)  + CH4(g)

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A: Given, mass of Fe3O4 = 5.1231 g molar mass of Fe3O4 = 231.533 g/mol !! Calculate the moles of Fe3O4…

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A: Ca2+(aq) + C2O42-(aq) →CaC2O4(s) CaC2O4(s) →CaO + CO2 +CO Weighing form =Obtained precipitate is…

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Q: A 0.5000 g sample of a pesticide (DDT, C14H9Cl5, MM 354.49 g/mol) was decomposed with metallic…

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A:

Q: 2. The arsenic in a 1.203-g sample of a pesticide was converted to H3ASO4 by suitable treatment. The…

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Q: A sample of manganese weighing 1.743 g is dissolved in 4.00 M HCl. What (minimum) volume of HCl is…

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Q: Enter your answer in the provided box. A sample of 0.8360 g of an unknown compound containing barium…

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Q: on, and then titrated with pre. n't need to know the formula

A: Calculation of mass percentage of iron. Mass of iron = 55.845g/mol.

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A:

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Q: 278.01 g/mol),(molar mass=278.01 g/mol), among other components. A 3.125 g3.125 g sample of the…

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.