Chem lab Purpose . To determine a trial ion product (Q) for lead…

Question Answered step-by-step Chem lab Purpose . To determine a trial ion product (Q) for lead… Chem lab Purpose.To determine a trial ion product (Q) for lead (II) iodide that is a close as possible to its solubility product constant (Ksp).Materials-0.010 mol/L KI(aq) (dropper bottle)   -0.10 mol/L Pb(NO3)2(aq)-5mL graduated pipette with bulb      -50 mL beakerProcedure 1. Bring the 50 mL beaker to the Pb(NO3)2(aq) bottle. Fill the graduated pipette with Pb(NO3)2(aq) to the zero line. Drain the graduated pipette to the 4.50 mL line into the beaker. This will add 4.50 mL of Pb(NO3)2(aq) to the beaker. Drain the remaining Pb(NO3)2(aq) back into the bottle. Return to your lab bench. 2. Unscrew the dropper from the KI(aq) bottle. With the dropper fully submerged in the liquid,squeeze the bulb and then release the bulb (this will fill the dropper). 3.Withdraw the dropper from the bottle and hold it vertically above the beaker. Adding liquid drop-by-drop, carefully count the number of drops that it takes to achieve a faint yellow precipitate that persists upon swirling of the beaker. The data for this is already recorded in the table below.  4.Dispose of the beaker contents into the inorganic waste container.Thoroughly clean and dry the beaker. 5.Repeat the above steps two more times for a total of three trials.Image transcription textTrial 1 Trial 2 Trial 3 number of KI(aq)drops 23 25 24 volume of KI(aq) (ml)[note: 1 drop has a volume of 0.0462 ml]… Show more6. In the space below, use your data from above to determine the average volume of KI(a) added to achieve the faint yellow precipitate Please answer the following question below  based on all the information provided above.  1.Calculate the average total volume of the solution in the beaker when the faint yellow precipitate was observed. 2. Calculate the average concentration of lead (I) ions and iodide ions in the solution when the faint yellow precipitate was observed. 3. Write the balanced solubility equilibrium for lead (II) iodide. Be sure to include states. 4.Write the trial ion product (Q) expression for the solubility equilibrium of lead (Il) iodide. 5.Use your answers to questions 2 and 4 to calculate the experimental lead (Il) iodide Q value. 6. Compare your lead (Il) iodide Q value from question 5 to Ksp for lead (Il) iodide. Explain why it makes sense that these values are not equal. (Assume that your experiment occurred at 25 °C). 7.How would your experimental Q value differ if you performed the experiment at a lower temperature? Explain your reasoning using appropriate concepts and terminology. 8. Calculate the molar solubility of lead (I) iodide at 25 °C. 9.It your goal was to precipitate Pb^2+ from a solution, why is KI(aq) a better choice than KCl(aq)? 10.Name an anion that would precipitate Pb^2+(aq) more easily than I- (aq), Briefly explain your answer .-Please do the calculation on paper and make sure your handwriting is clear. For the part where you have to explain not calculate, you don’t have to write it on paper but you can if you want too -Please be detailed -All the data needed to answer the questions have been provided  Science Chemistry CHEM N/A Share QuestionEmailCopy link Comments (0)