Hydrochlorimetry Lab Report

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By adding Hydrochloric acid into solid Magnesium, in Data table #2, when Hydrochloric acid was first been added to solid Magnesium, the ribbon immediately start to bubble and producing fumes at the same time with a burning sound. Magnesium start to turn into a white liquid form. After the bubble start to disappear, more Hydrochloric acid was added, and the reactions repeats. Until none of the shiny silver Magnesium ribbon can be seen, and there is no more bubble, the reaction is over. After placing the evaporating dish on a hot plate on a scale of 7, by the data from Data table #2, the white liquid that contains Magnesium, Chlorine and Hydrogen start to release fumes. As time passed, the liquid start bubble, and the liquid start to become …show more content…
To find the moles of Magnesium, dimensional was used to multiply the molar mass of Magnesium to its measured mass, the final result is 5.3475936 x 10-3 moles.
0.13g Mg×(1mol/(24.31g))=5.3475936×〖10〗^(-3)
After adding Hydrochloric acid and been heated on the hot plate, the total mass of evaporating dish plus Magnesium Chloride is 44.96 grams. By subtracting the mass of Magnesium ribbon 0.13 grams from the total mass 44.96 grams, the mass of Magnesium Chloride was found to be 0.56 grams.
44.96-44.40=0.56g
After knowing the mas of Magnesium chloride, by subtracting the mass of Magnesium ribbon from it, the mass of Chloride was found to be 0.43 …show more content…
0.43g Cl×(1mol/(35.45g))=1.121297602×〖10〗^(-2) After knowing the moles of Magnesium and Chlorine, their mole ratio can be calculated by dividing the smaller moles, and then multiply a positive whole number to get the final empirical formula ratio of 9 Mg with 4 Cl.
(0.0121297602)/(0.0053475936)=2.26 (0.0053475936)/(0.0053475936)=1 Cl=2.26×4=9.07 Mg=1×4=4
As we know each mass of Magnesium and Chloride, the percent composition of Magnesium can be calculated when divide the mass of magnesium from the mass of Magnesium Chloride.
(0.13)/(0.56)=23.21428571%
After knowing the percent composition of Magnesium, and knowing the theoretical value as 25.5%, the percent error can be calculated by applying the formula.
(25.5-23.2142857)/(25.5)×100=8.963585451%

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