# I need help with my lab the whole thing please. i Dont know how to do the calculations abstract: The

I need help with my lab the whole thing please. i Dont know how to do the calculations abstract: The aim of the experiment was to learn how successfully dilute stock (concentrated) solutions of 1.0 M NaOH and 0.020 M KMnO4solutions. The general dilution equation is: McVc= MdVd In the equation above: Mc is the molarity of the concentrated solution – was given Vcis the volume of the concentrated solution – has to be calculated Mdis the molarity of the diluted solution – was given Vdis the volume of the diluted
question I need help with my lab the whole thing please. i Dont know how to do the calculations abstract: The aim of the experiment was to learn how successfully dilute stock (concentrated) solutions of 1.0 M NaOH and 0.020 M KMnO4solutions. The general dilution equation is: McVc= MdVd In the equation above: Mc is the molarity of the concentrated solution – was given Vcis the volume of the concentrated solution – has to be calculated Mdis the molarity of the diluted solution – was given Vdis the volume of the diluted solution – was given To calculate the volume of the concentrated solution, we modify the equation above to the formula: Vc= In addition, we calculated the volume of water needed to dilute the solution completely according to formula Vw= In Part I of experiment, we tested pH of diluted NaOH solutions, which allow us to calculate molarity of diluted solutions using following formula: [OH-] = We also need to learn the rules of Sig Fig in logarithms. Explain the rule in your worlds below: In Part II of experiment, using a spectrometer we measured the absorbance of diluted KMnO4solutions and we apply Beers Law to calculate molarity of diluted KMnO4. Beers Law is : A = a*b*M Where: A is absorption of the solution (measured by us ) in nm a is a is molar absorptivity coefficient = 2.24 x103cm-1M-1 b is the path of light length in cuvette = 1.0 cm M is the molarity of the sample M = mol/L To calculate the molarity of the dilute potassium permanganate solutions we used following M = RESULTS: Table 8.1 Serial dilutions of NaOH solutions Solution A: was made by diluting 1.0 M NaOH. Required diluted molarity was 1.0 x10-1M, required volume 25.0 mL Solution B: was made by diluting solution A. Required diluted molarity was 1.0 x10-3M, required volume 20.0 mL Solution C: was made by diluting solution B. Required diluted molarity was 1.0 x10-5M, required volume 20.0 mL Solution NaOH Mc Vc Vw Vd Md pH A 1.0 M 2.5 mL 22.5 mL 25.0 mL 1.0 X 10-1M 12.17 B 1.0 X 10-1M 0.20 mL 19.8 mL 20.0 mL 1.0 X 10-3M 9.60 C 1.0 X 10-3M 0.20 mL 19.8 mL 20.0 mL 1.0 X 10-5M 5.80 1. For Table 8.1 show how did you calculate volume of concentrated NaOH solution and volume of water Vw, which has to be used in order to obtain requested Vdfor the diluted solutions A,B,C. Fill empty boxes in a table. Solution A Solution B Solution C 2. Calculate molarity of diluted NaOH solutions using your pH data. Show your calculations. Report results in right SF as measured concentration (each wrong answer is -2 Pt) Solution A: [OH-] = Solution B: [OH-] = Solution C: [OH-] = 3. Calculate % error for each solution using required molarity as accepted value. Table 8.2 Serial dilutions of KMnO4solutions Please explain how you did serial dilutions for solutions D, E, F, G using example for solution D Solution D was made by diluting: 2.0 X 10-2M KMnO4.Required diluted molarity was 2.0 x10-3M, required volume 25.0 mL Solution E was made by: diluting Solution F was made by diluting: Solution G was made by diluting: Solution Mc Vc Vw Vd Md Absorbance D 2.0 X 10-2M 2.5 mL 22.5 mL 25.0 mL 2.0 X 10-3M 3.00 E 2.0 X 10-3M 1.0 mL 9.0 mL 10.0 2.0 x 10^-4 .384 F 2.0 X 10-4M 5.0 mL 5.0 mL 10.0 1.0 x 10^-4 .128 G 1.0 X 10-4M 5.0 mL 5.0 mL 10.0 5.0 x 10^-5 0.053 1. For Table 8.1 show how did you calculate volume of concentrated KMnO4solution and volume of water Vw, which has to be used in order to obtain requested Vdfor the diluted solutions D,E,F,G. Fill empty boxes in a table. Solution D Vc= Vw= Solution E Vc= Vw= Solution F Vc= Vw= Solution G Vc= Vw= 1. Calculate molarity diluted KMnO4 Report results in right SF as measured molarity (wrong SF -2 pt) D.M= A/ab = E. M= A/ab = F. M= A/ab = G. M= A/ab = 2. Calculate % error for each solution using required molarity as accept value. CONCLUSIONS: PART I: Summary Table for dilutions of NaOH solution Solution pH Molarity measured Molarity required % Error A 1.0×10-1 B 1.0×10-3 C 1.0×10-5 PART II: Summary Table for dilutions of KMnO4solutions Solution Absorbance Molarity measured Molarity required % Error D 2.0 X 10-3M E 2.0 X 10-4M F 1.0 X 10-4M G 5.0 X 10-5M

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