Question

what percent of theoretical moles was actually required to get to the end point?

3. Write the reaction for Part B in "molecular" (whole formula) form and in net ionic form: lar" equation: MgSO4 caw) +2NaOH anant MgOH)215) + Na-Souca Net ionic equation: Mg? Cans + 20 Heaga > MgCOH)2 (5) NIE 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. Mass of NaOH solution:36.708 g of 0.20% Mass of MgSO4 solution: 5.869 gof.0% Mass of NaOH solute: Mass of MgSO4 solute: 75.86914 Moles of NaOH: 0.91777 Moles of MgSO4 0.6032 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? 0.45889 What percent of the theoretical moles was actually required to get to the end point? This "% of theoretical moles" calculation is similar to, but different from a "%Yield" calculation. How is it different?

Answer 1

Mq804 + 2NaOH - MOCOH)2 + NAJ SO 4. 0.63032 0.91777 Theoretically required moles = 0.45889 actually What percent of the theoretical moles was required to get the end point? Required no. of moles x 100. Given number of moles. x 100 = 72.8% 0.45885 0.63032 The percent of theoretical moles actually required to get the end point - 72.8%