Report predicted pKa, observed pKa and percent error from graph please if you could please explain :) IV. Titration of monobasic sodium phosphate. Volume of 1.0M NaOH added (ml) Measured pH Volume of 1.0M NaOH Measured added (ml) 0.0 4.59 5.0 7.09 0.5 5.67 6.0 7.33 1.0 6.01 7.0 7.60
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- You have a sample of approximately 100 mg/L of calcium carbonate and the standardized EDTA has a concentration of 0.00085 M. If you only want to spend approximately 15 mL of the titrant and add 25 mL of sample in the Erlenmeyer flask, can you use it or should you dilute it? the sample?, how much? Solution: No, 29 mL would be needed to titrate the sample, you must dilute it approximately 1: 2. Taking, for example, 25 mL of sample and making up to 50 mL.If the water sample used for titration was buffered with acid instead of alkali, the amount of EDTA required to reach the endpoint will: a. stay constant b. be indeterminatec. increased. decreaseA. Why is the titration of the oxalate in the green salt with KMnO4 performed prior to carrying out the redox titration for iron content? (Why can’t you do them the other way – iron first then oxalate?) B. In a titration using 0.02000 M KMnO4 solution, the following data were obtained: Buret readings: FINAL = 15.31 mL INITIAL = 5.02 mL How many moles of KMnO4 were used?
- A 0.045 0 M solution of HA is 0.60% dissociated. Find pKa for HA.Which of the following statements is true regarding permanganimetry? a) Permanganate solution can oxidize water which is catalyzed by the presence of manganese dioxide or manganese ion. b) The light pink endpoint color for permanganimetry tends to fade with time due to the catalytic reaction. c) Standardization of the permanganate titrant is carried out at elevated temperature with sodium oxalate. d) all of these e) none of these2,5 ml volume has taken from an “hypothetic” solution which includes (3+) Sb and (3+) Fe and at the titration with 0.1004 N KMnO4, the wasted amount has found as 16,4 mL. The other 2,5 mL that has taken, has reduced with Zn after that, this 2,5 mL solution has titrates with the same KMnO4 solution solution and the wasted amount is 26,5mL. With these datas find the %concentrations of the ions at the solution.
- The concentration of a solution of EDTA was determined by standardizing against a solution of Ca2+ prepared from the primary standard CaCO3. A 0.4302g sample of CaCO3 was transferred to a 60mL volumetric flask, dissolved using a minimum of 6 M HCl solution, and diluted to volume. A 44mL portion of this solution was transferred into a 250-mL Erlenmeyer flask and the pH adjusted by adding 5 mL of a pH 10 NH3-NH4 L buffer containing a small amount of Mg2+ EDTA. After adding calmagite as a visual indicator, the solution was titrated with the EDTA, requiring 632mL to reach the end point. Calculate the molar concentration of the titrantIf an Ecell of 0.495V was noted when your cell was set-up. What is thesolution pH?Please show all work. 1. estimate the position of the equivalance point 2. estimate the position of the half-equivalance point 3. calculate the percent error in the experimental pKa value (accepted pKa value is 4.75) 4. Identify the buffering region 5. Identify the volme ranges that corresponed to the initial color and the final color of the indicator Volume pH 0 2.88 0.05 2.9 0.14 2.95 0.55 3.14 1.15 3.35 1.45 3.44 1.97 3.56 2.36 3.63 2.77 3.69 3.17 3.75 3.78 3.84 4.09 3.86 4.59 3.92 5 3.98 5.39 4 5.8 4.03 6.3 4.09 6.6 4.11 6.99 4.13 7.5 4.17 8.01 4.22 8.31 4.23 8.8 4.27 9.2 4.3 9.5 4.3 9.91 4.34 10.53 4.37 10.92 4.4 11.33 4.41 11.63 4.44 12.14 4.47 12.53 4.47 12.94 4.51 13.35 4.52 13.74 4.56 14.14 4.56 14.54 4.59 15.04 4.62 15.33 4.64 15.73 4.65 16.22 4.67 16.62 4.71 17.02 4.72 17.33 4.73 17.73 4.75 18.34 4.79 18.63 4.8 19.02 4.82 19.43 4.84 19.92 4.88 20.33 4.9 20.73 4.92…
- Quantitative analysis of metal ions in pharmaceutical and cosmetic products can be done using direct and indirect complexometric titrations employing concepts of complex formation, masking, and blocking. For example, all Fe3+, Mg2+, Al3+ and Zn2+ can form a complex with EDTA at pH 10. However, at pH 5, Mg-EDTA complex formation is inhibited, whereas at pH 2, only Fe-EDTA complex formation is favored. Knowing these, an analyst tried to determine the % composition of a 0.1000 g sample containing soluble salts of Fe3+, Mg2+, and Al3+. The sample was initially dissolved in 250.0 mL of distilled water. To determine the total ion content of the sample, a 50.00 mL aliquot was buffered to pH 10.00 before adding 50.00 mL of 0.0500 M EDTA, and the excess EDTA was back titrated with 24.18 mL of 0.0750 M standard Zn2+ solution until the EBT endpoint. Another 50.00 mL aliquot was buffered to pH 2.00 and was added with small amount of SCN- producing blood-red Fe(SCN)2+ complex. This was titrated…A. What is the characteristic color of ferric ions in solution? B. Why is the titration of the oxalate in the green salt with KMnO4 performed prior to carrying out the redox titration for iron content? (Why can’t you do them the other way – iron first then oxalate?) C. In a titration using 0.02000 M KMnO4 solution, the following data were obtained: Buret readings: FINAL = 15.31 mL INITIAL = 5.02 mL How many moles of KMnO4 were used?For the complexiometric titration of Ca2 + ions in the shell of the egg sample weighing 62,576 g, the necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The prepared solution was titrated with 23.6 mL of 0.0095 M EDTA solution. What is the value of the amount of calcium in the sample in terms of% CaCO3? (Ca: 40, C: 12, O: 16 g / mol)