Question

dont know how to do it or if is right .
need help doing 3

TOLD UITSLEITEEREI, IU "Molecular” equation: 2 Nao Hlap + MgSoa (ay) - Na2S04 () + Mg(OH)2 (5) Net ionic equation: 20 Heag) + Mg2+L9) - Mg (OH) 2. (5) Calculate and report the number of grams of each solution, and of each solute, that was used to get to the end point of the reaction in Part B. Then, for the solutes, calculate the number of moles using correct significant figures. Show work for each on the back of this page. 31.9 16" 28.131 935 bol.01167 Mass of NaOH solution: 35.939 g of -20% Mass of MgSO4 solution: 3.239 g of 3% Mass of NaOH solute: 40.7187 Mass of MgSO4 solute: 162 3.239.05 Moles of NaOH: .002 mol Moles of MgSO4: bol mol Based on the moles of NaOH you used, and the coefficients of the balanced equation, how many moles of MgSO4 should have been required, theoretically? What percent of the theoretical moles was actually required to get to the end point? This % of theoretical moles" calqulation is similar to, but different from a "% Yield" calculation. How is it different? CHEM& 161 F19

. I have the mass of naoh and mass of mgs04 sultion from experiment.

Answer 1

The answers were calculated based on mass of reagens mentioned by the student based on stoicheometry

till the requiremen slution The Naon question is solved & Mason of Moteref Noolt 20.02 mot. Mass of Naon = 0.0187 moles as Naon a mass a molecular mas -0.07 187 39.gg 0.017968 moles marscy mysoy 162 g moles of MgSO4 = 162 120.36 = 0.00134 - The balonced equation is 2NaOH & Mason - Na₂SO4 + Mgonz or od for every mot Imole NaOH - 1 mole mason is required 0.0179 moles of NCOH 2 1 0.0179 moles Mason required = 0.00895 moles required The percentage pant can not be determined as data is inscefficient