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- Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).Consider the titration of 80.00 mL of 0.100 M Ba(OH)2 with 0.400 M HCl. Calculate the pH at the following volumes of the titrant: VT = 0.00 (Initial Stage) VT = 20.00 VT = 30.00 VT = 40.00 (Equivalence Point Stage) VT = 50.00 VT = 80.00For the titration of 50.00 mL of 0.300 M RbC7H5O2 (WB) with 0.200 M HNO3 (SA). Ka (HC7H5O2) = 6.3 x 10-5 Express pH value to two decimal places. Determine the pH after the addition 12.50 mL of HNO3.
- Calculate the final concentration of citrate buffer in a test tube containing the following components: 250 µl of 25 mM p-nitrophenol phosphate, 100 µL 0.5 mg.ml-1 acid phosphatase and 150 µl 100 mM citrate buffer pH 4.8. Provide the answer together with unit in the answer box.For the titration of 50.00 mL of 0.300 M RbC7H5O2 (WB) with 0.200 M HNO3 (SA). Ka (HC7H5O2) = 6.3 x 10-5 Express pH value to two decimal places. Determine the initial pH before any acid is added.For the titration of 50.00 mL of 0.300 M RbC7H5O2 (WB) with 0.200 M HNO3 (SA).Ka (HC7H5O2) = 6.3 x 10-5Express pH value to two decimal places.Determine the pH after the addition 90.00 mL of HNO3.
- A carbonate mixture was titrated with 0.1100 M HCI. The sample weighing 850.0 mg took 21.00 mL to reach the phenolphthalein end point and an additional 14.00 mL to reach the methyl red end point. Calculate the weight percentage of the component/s.Average [EDTA] = C: Determination of the hardness of an unknown water sample: Using an unknown water sample, three 25 mL samples in 3 separate 250 mL Erlenmeyer flasks are prepared. To each flask, 5 mL of pH pH10 buffer, 3 to 5 drops of Eriochrome Black T indicator, and 15 drops of 0.03 M MgCl2 solution are added. Each flask is titrated to the end point using EDTA.Calculate 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.
- 100.0 mL sample of drinking water was buffered with ammonia at pH 10 and after addition of EBT required 21.4 mL of 0.00512 M EDTA for titration. FW CaCO3 = 100.09 g/mol. What will be the change in color at the end point? What is the water hardness in terms of ppm CaCO3?. What is the role of ammonia buffer in the analysis?Select Weak Acid as the analyte in the titration interactive. Analyte, 25.0 ml Strong Acid, 1.0. Determine the pK, of this weak acid. Indicator Phenolphthalein pink 14 pH=11.60 pK = 13.82 25 50 Titrant Added (ml) Titration Curve Concentration Chart Titrant: Strong Base, 1.0 M MOH 50 25.2 mL + HdCalculate the volume at equivalence point and subsequently the pAg when 25.75 mL of 0.1350 M I' is titrated with 32.00 mL of 0.1450 M AgNO3 titrant. Ve = ml pAg = %3D