Answer Happy

THE MOLES FOR PB(NO)3 AND KI ARE BELOW
7. Calculate the molarities of the Pb(NO3​)2​ and KI solutions the student made. Remember: molarity = L solution  mol solute. ​ Remember that you need the molar mass of the solute in order to determine the number of moles. All information you need to get started is given to you in the Part 2 experimental setup on page 6 . Record your calculated molarities in the lab report. 8. Using the data in Table 3, calculate the molarities of the Pb2+ ion and I' ion in each of the nine solutions. Record these molarities in Table 4, below. Remember that there is one Pb2+ ion formed for every one unit of Pb(NO3​)2​ used. Also remember that there is one I− ion formed for every one KI unit used. Use the dilution formula: ConcentrationinitiaVolumeinitial ≡ Concentrationfinal Volumefinal The initial concentration is the concentration you calculated in Step 7. The initial volume is the volume for the particular ion from Table 3. You are solving for the final concentration. The final volume is, in all cases, 10.00 mL 7 Name: Date: Section: Table 4. Solubility Data.
9. Using Equation 5 , write the Ksp​ expression for the slightly soluble solid. 10. Using the data in Table 4, calculate a Q for each reaction. You will calculate Q just like Ksp​, except you will use the experimental values in Table 4 instead of equilibrium values. 11. The data given in Tables 3 and 4 allow you to bracket the real value for Ksp​. Using the data in Table 4 and the guidelines in Table 1, determine an estimated value for Ksp​. Record this value in your lab report. 12. The lab report will ask you to calculate a percent error. Remember that percent error has the formula shown below: Percent error =⌊ Accepted value − experimental value ⊥×100% Accepted value The value you estimate for the Ksp​ is the experimental value. 13. Submit the photographs and complete the report, which is in the form of an online quiz.
Table 3. Solution Preparation and Precipitate Formation.