Suppose 79.3 mL of a 0.200 M solution of Na2SO4 reacts with 143 mL of a 0.388 M solution of MgCl2 to produce MgSO4 and NaCl as shown in the balanced reaction. Na2SO4(aq)+MgCl2(aq)⟶MgSO4(s)+2NaCl (aq)

Determine the limiting reactant for the given reaction.
a. Na2SO4
b. NaCl
c. MgCl2
d. MgSO4

Calculate the mass of MgSO4 that can be produced in the given reaction.

Only 0.378 g of MgSO4 are isolated after carrying out the reaction. Calculate the percent yield of MgSO4.

13. calculate the initial concentration (before precipitation) of carbonate ions after the addition of each 0.05 ml of solution b to the 1.00 l beaker of solution a. divide the work among group members and write the answers in the table in model 3. assume the volume change as solution b is added is negligible. 14. notice the initial concentrations of zn2+ - and cu2+ in the table in model 3. a. explain how these were obtained from the data in model 2. b. as solution b is added and precipitates form, do these initial concentrations change? 15. use the data in model 2 to indicate the presence of precipitate (either znco3 or cuco3) after each 0.05 ml addition of solution b in model 3. 16. use the initial concentrations of carbonate ions and zinc ions to calculate the reaction quotient, qsp for the zinc carbonate scenarios in model 3. divide the work among group members and write the answers in the table in model 3. 17. use the initial concentrations of carbonate ion and copper(ii) ions to calculate the qsp for the copper(ii) carbonate scenarios in model 3. divide the work among group members and write the answers in the table in model 3.

Which statement describes james chadwick’s discovery.

Which element has the lowest electronegativity? calcium(ca) gallium(ga) selenium(se) bromine(br)