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A 10.00 g sample of MgSO4.7H₂O (246.48 g mol¹) was heated in an oven at 105°C until all the waters of hydration was evaporated off to generate MgSO4 (anhydrous). The sample was then dissolved in 250 mL of distilled water and diluted to a final volume of 0.5 L. The amount of SO42 in parts per million (ppm) in the final solution is: Molar masses in g mol-¹: MgSO4.7H₂O = 246.48; H₂O = 18.02 9766.0 ppm 3806.08 ppm E 7795.60 ppm 15964.77 ppm
A mass of barium sulfate is produced when 1 kg of zinc sulfate is mixed with 1 kg of barium sulfide in aqueous solution according to the following balanced equation: ZnSO (aq) + BaS(aq) - ZnS(s) + BaSO4(aq) ZnSO₂ = 161.46 g mol¹, Bas=169.41 g mol: ZnS =97.47 g mol¹; BaSO4 = 233.38 g mol¹1¹ The percentage (%) of Zn that remains in the reactant is: 4.60 % 18.96 96 3.40%
What mass of a solution of H₂SO4 (98.08 g mol-1) (in grams) is required to completely neutralize 500 mL of a 30 % (m/m) Ba(OH)2 (171.34 g mol-¹) solution (density at 25°C = 1.175 g mL^¹)? Eqn: H₂SO4(aq) + Ba(OH)₂ (aq) →BaSO4(s) + 2H₂O(l) 30.0 g 14.60 g 100.89 g 17.17 g
A 1.35 g sample of a substance containing C, H, N, and O is burned in air to produce 0.810 g of H₂O(g) and 1.32 g of CO₂(g). In a separate analysis, a mass sample of 0.735 g of the same substance produced 31.80 % of N in a conversion of the sample to NH3. The percentage % 0 in the sample weighing 1.35 g is: Molar masses (g mol-¹): CO₂ = 44, H₂O = 18; NH3 = 17.04, C = 12.01; H = 1.01; N = 14.01; 0 = 16.00 78.87% 34.82 % 49.29 % 16.0%