You have prepared a solution of NaOH by diluting a stock 1.5 M NaOH solution with approximately 200 mL of water. You now need to determine its precise concentration and you have performed five titration trials to standardize your solution. Here are the results of your trials: trial # mass of potassium biphthalate (mg) volume of NaOH solution (mL) 12.30 mL 1 180 mg 15.20 mL 2 180 mg 12.20 mL 3 180 mg 13.90 mL 4 180 mg 12.50 mL 5 180 mg You now have to calculate the average molar concentration of your NaOH solution and you want it to be as precise as possible. How are you going to do it? I will only use trials 1 and 3 I will use all the trials for my calculations I will discard trial 4 I will discard trials 2 and 4

You have prepared a solution of NaOH by diluting a stock 1.5 M NaOH solution with approximately 200 mL of water. You now need to determine its precise concentration and you have performed five titration trials to standardize your solution. Here are the results of your trials: trial # mass of potassium biphthalate (mg) volume of NaOH solution (mL) 12.30 mL 1 180 mg 15.20 mL 2 180 mg 12.20 mL 3 180 mg 13.90 mL 4 180 mg 12.50 mL 5 180 mg You now have to calculate the average molar concentration of your NaOH solution and you want it to be as precise as possible. How are you going to do it? I will only use trials 1 and 3 I will use all the trials for my calculations I will discard trial 4 I will discard trials 2 and 4

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section: Chapter Questions

Problem 139SCQ: Two students titrate different samples of the same solution of HCl using 0.100 M NaOH solution and...

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Two students titrate different samples of the same solution of HCl using 0.100 M NaOH solution and phenolphthalein indicator (Figure 4.12). The first student pipets 20.0 mL of the HCl solution into a flask, adds 20 mL of distilled water and a few drops of phenolphthalein solution, and titrates until a lasting pink color appears. The second student pipets 20.0 mL of the HCl solution into a flask, adds 60 mL of distilled water and a few drops of phenolphthalein solution, and titrates to the first lasting pink color. Each student correctly calculates the molarity of an HCl solution. What will the second students result be? (a) four times less than the first students result (b) four times greater than the first students result (c) two times less than the first students result (d) two times greater than the first students result (e) the same as the first students result