Question

1. True or False: a) Our titrat in this experiment is 0.100M H₂SO4. [0.5 point] b) The drop counter accounts for the mass of each drop. [0.5 point] c) We could be able to drink the solution that is produced in this lab. [0.5point] d) Mercury sulfate is soluble in solution. [0.5 point] 2. Write the balanced equation of the reaction that occurs of today's experiment.Take care of the states of each substance [i.e. (g), (I), (s), (aq)] [3 points] 3. List all requirements that must be met in order to make a gravimetric analysis to work. [5 points] 4. What should the drip rate be in order for drops to be counted accurately by the drop counter? [1 point] 5. What are the units of conductivity? 6. For today's experiment, a graph shows the relation of conductivity like; [4 points]vs. time a) In time period, before to, why is conductivity decreasing? b) In time period, after to, why is conductivityincreasing? 7. In gravimetric determination, why should we heat the titrated solution to a near-to-low boil? [2 points] 8. For 10.3 mL unknown Ba(OH)₂ solution, using 0.114 M H₂SO4 do conduct imetrictitration, the equivalence point was 8.76 mL, calculate the molarity of the this unknown Ba(OH)₂ solution. Show your all work. (3pts) 9. For 9.87 mL unknown Ba(OH)₂ solution, in gravimetric analysis, the empty, dry crucible had a mass of 8.564 g, the total mass of crucible with the precipitate was 10.187 g, calculate the concentration of this unknown Ba(OH)₂ solution.Assume the molar mass of BaSO4 is 233.4 g/mol. Show your all work. (4 pts)

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