Oxalic acid is a diprotic acid (Ka, = 5.9 x 10-2 and Kaz = 6.4 x 10-5). %3D Identify each of the following statements as true or false regarding a titration of 1.OM oxalic acid with a 1.0 M NaOH solution at 25°C. Type in "true" or "false" for each statement. 1. At pH = 3, the predominant species in solution is amphiprotic 2. One mole of NaOH will fully neutralize one mole of oxalic acid 3. The pH at the second equivalence point will be 7 4. The first half equivalence point is at pH = 1.23 %3D 5. At pH = 6, the predominant species in solution will be the oxalate ion, C2042-

Ex. 13-5. A 50.00-mL of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point with bromocresol green indicator. Calculate the molarity of the HCl. Ва(ОН)2 + 2HCІ- ВаCl, + 2H-0

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On the following titration curve, indicate what the pH is at each point (eg. >7, =7, <7), what the major chemical species present are, and what type of solution is present Titration curve is shown on the image provided

Calculate the pH during the titration with NaOH after addition of: a) 50.00 mL of 0.1000 mol L-1 NaOH to 50.00 mL of 0.1000 mol L-1 CH3COOH (Ka= 1.75 x 10-5). b) Based on the table below, which indicator (A, B or C) is most appropriate to monitor this titration? Explain. Indicator A B C pKIndicator 3.8 9.3 5.0 Actual Transition Range (pH) 3.0 to 4.6 3.0 to 4.6 4.4 to 6.2

When titrating 25 mL of an approximately 0.1 M solution of a triprotic acid solution with 0.1052 M NaOH, a student calculates that the end point will be reached after the addition of approximately x mL of NaOH. However, after the addition of 2x mL of sodium hydroxide, no colour change is observed.  Which of the following errors could not account for this obervation?        using a 3 mole acid : 1 mole base ratio in the calculation      washing the sides of the flask with DI water during the titration and diluting the analyte solution      mistakenly using a 0.01000 M NaOH solution in the titration      failing to add an indicator to the analyte solution      mistakenly using a primary standard solution of > 1.0 M in the titration

Read sec. 14.7 2, then calculate the volume at equivalence and the pH at each of the following volumes of titrant for the titration of a 75.00 mL of a 0.049 mol L1 solution of nitrous acid (pKa = 3.37) titrated with 0.198 mol L' sodium hydroxide. %3D Ve = 18.6 mL VOH pH VOH 7.05 pH : VOH = = 12.1 pH %3D VOH = Ve %3D pH %3D Von = 27.8 pH = VoH = 55.7 pH Submit Question Jump to Answer

Suppose we titrate 20.0 mL of 0.100 M HCHO2 (Ka = 1.8 x 10-4) with 0.100 M NaOH. Calculate the pH. Before any base is added: pH = When half of the HCHO₂ has been neutralized: pH = After a total of 15.0 mL of base has been added: pH At the equivalence point: pH =

Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2–9.3? CH3COONA / CH3COOH (Ka = 1.8 x 10-5) %D NH3 / NHẠCI (Ka = 5.6 x 10-10) NaOCI / HOCI (Ką = 3.2 x 10-8) NaNO2 / HNO2 (Ka = 4.5 × 104) %D