5-30. Generate a curve for the titration of 50.00 mL of a solution in which the analytical concentration of NaOH is 0.1000 and that for hydrazine is 0.0800 M. Calculate the pH after addition of 0.00, 10.00, 20.00, 24.00, 25.00, 26.00, 35.00, 44.00, 45.00, 46.00, and 50.00 mL of 0.2000 m HCIO,.
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- 7-36. A 50.00-mL aliquot of 0.1000 M NaOH is titrated with 0.1000 M HCI. Calculate the pH of the solution after the addition of 0.00, 10.00, 25.00, 40.00, 45.00, 49.00, 50.00, 51.00, 55.00, and 60.00 mL of acid and prepare a titration curve from the data.Generate a curve for the titration of 50.00 mL of a solution in which the analytical concentration of HClO4 is 0.1000 M and that of formic acid is 0.0800 M. Calculate the pH after the addition of 0.00,10.00, 20.00, 24.00, 25.00, 26.00, 35.00, 44.00, 45.00, 46.00 and 50,00 ml of KOH 0,2000 M.Generate a curve for the titration of 50.00 mL of a solution in which the analytical concentration of NaOH is 0.1000 M and that for hydrazine is 0.0800 M. Calculate the pH after addition of 0.00, 10.00, 20.00, 24.00, 25.00, 26.00, 35.00, 44.00, 45.00, 46.00, and 50.00 mL of 0.2000 M HClO4.
- A student titrates 29.00 mL of 0.2250 M pyridine (Kb = 1.7*10-9) with 0.3750 M HBr. Calculate the pH after the addition of 6.50 mL, 8.70 mL, 9.90 mL, 10.00 mL, 10.80 mL, 15.00 mL, 17.40 mL, 18.70 mL and 36.00 mL of HBr. Plot the results of your calculations as pH versus mL of HBr added9-20. (a) Calculate how many milliliters of 0.100 M HCI should be added to how many grams of sodium acetate dihy- drate (NaOAc· 2H2O, FM 118.06) to prepare 250.0 mL of 0.100 M buffer, pH 5.00. (b) If you mixed what you calculated, the pH would not be 5.00. Describe how you would actually prepare this buffer in the lab.A student titrates 29.00 mL of 0.2250 M pyridine (Kb = 1.7*10-9) with 0.3750 M HBr. Calculate the pH after the addition of 0.00 mL, 2.00 mL, 3.60 mL, 5.00 mL, 6.50 mL, 8.70 mL, 9.90 mL, 10.00 mL, 10.80 mL, 15.00 mL, 17.40 mL, 18.70 mL and 36.00 mL of HBr.
- Hello ! I have to answer to this question : Generate a curve for the titration of 50.00 mL of a solution in which the analytical concentration of NaOH is 0.1000 M and that for hydrazine is 0.0800 M. Calculate the pH after addition of 0.00, 10.00, 25.00, 35.00, 45.00 and 50.00 mL of 0.2000 M HClO4.I can't do this exercice with Excel and I need to determinate if there are approximations at each step and if there are, I need to verify them . And I can't do it.. Can you help me ? Thank you Pauline40.00 ml of 0.1200 benzoic acid is titrated with 0.1000 M NaOH. Calculate the pH after the addition of the following volumes (ml) of titrant: (a) 0.00; (b) 24.00; (c) 48.00. Ka for benzoic acid is 6.6 x 10-5.Data for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact concentration of the standard NaOH solution to calculate the moles of NaOH. Quantity Еxample Trial 1 Trial 2 Trial 3 M NaOH (exact concentration) 0.992 M 0.953 M 0.953 M 0.953 M V initial buret reading = V, 0.20 mL 1.20 mL 0.52 mL 0.15 mL V final buret reading = V, 12.90 mL 14.22 mL 13.71 mL 13.31 mL %3D Vep = VNAOH added = V; - V, 12.70 mL 13.02 mL 13.19 mL 13.16 mL Vep = VNAOH in L 0.01270 L 0.01302 L 0.01319 L 0.01316 L moles NaOH = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol MNAOH X VNAOH moles AA = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol moles NaOH V sample = V acid 0.0150 L 0.0150 L 0.0150 L 0.0150 L (15.00 mL) (15.00 mL) (15.00 mL) Actual molarity 0.840 M 0.827 M 0.840 M 0.833 M of AA Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). 2. Use your average AA concentration to calculate the mass…
- Construct a curve for the titration of 50.00 mL of a 0.1000 M solution of compound A with a 0.2000 M solution of compound B in the following table. For each titration, calculate the pH after the addition of 0.00, 12.50, 20.00, 24.00, 25.00, 26.00, 37.50, 45.00, 49.00, 50.00, 51.00, and 60.00 mL of compound B.where, Compound A (H2SO3) pka1 = 1.23 x 10^-2 pka2 = 6.6 x 10 ^-8 Compound B (NaOHGiven the titration curves below, answer the following questions. 14 12 10 6. 4 Volume of strong base (mL) HdCalculate the pH at the following points for the titration of 50.00 mL of 0.0100 mol L-1 H2SO4 with 0.0100 mol L-1 NaOH standard solution.Vbase = 0.0; 10.0; 20.0; 25.0; 25.5; 40.0; 50.0 and 100.0.Plot a graph of pH versus Vbase.Perform the same procedure for H2SO4 and 0.01 mol L-1 NaOH concentrations.Generate the titration curves for the two solutions, compare them and justify.