Titration Results Initial buret reading (ml) Final buret reading (ml) Total volume used (mL) 0.00 15.00 15.00 HCI Trial 1.10M 0.05 31.10 31.05 NaOH SP 15.00 30.00 15.00 HCI Trial 2 16.05 44.25 28.20 NaOH
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- It is a solution of unknown concentration in which a solution of accurately known concentration is gradually added until the reaction is complete. Analyte Endpoint Indicator TitrantPart A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________A student carries out a titration to determine the molar mass and structure of a weak acid A. The student follows the method below. Dissolve a weighed mass of A in 100 cm3 of distilled water and make the solution up to 250 cm in a beaker. Add the solution of A to a burette. Titrate the solution of A with a standard solution of sodium hydroxide, NAOH. (a) What is meant by the term standard solution? (b) Sodium hydroxide is an alkali. What is meant by the term alkali? (c) The student carries out a trial, followed by three further titrations. The diagram shows the initial and final burette readings for the three further titrations. The student measures all burette readings to the nearest 0.05 cm3. Titration 1 Titration 2 Titration 3 Initial reading Final reading Initial reading Final reading Initial reading Final reading 27
- A solution of HCl was titrated against sodium carbonate. What is the titer for Trial 1 in the given data? T2 0.3562 0.3479 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (ml) Vol HCI used (ml) 35.10 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L) ATitration is the addition of a chemically equivalent volume of a solution of known concentration called analyte titrant fluent None of themTable 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.19 2.26 2.39 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 48.55 49.43 49.99 Expected color at end point Volume of NaOH used (mL) Average Volume of NaOH used in liters Average moles of NaOH used (mol) Average moles of acetic acid (mol) Average molarity of acetic acid (M) Average mass of acetic acid (g) Average mass of vinegar (g) (assume the density of vinegar is 1.00 g/mL) Average mass % of acetic acid in vinegar Known mass % of acetic acid in vinegar is 5.45% Percent Error
- Identify which of the graphs represent the given titration experiments best. Graph A Graph B 12 12 11- 11- 10- 10- 9- 9- 8- 8- 7- 7- 6- 6- 5- 5- 4- 3- 3- 2- 2 1 10 15 20 25 30 35 40 45 50 10 15 20 25 30 35 40 45 50 Titrant.volume Cml). Titrant.volume (mL). Answer Bank This graph does not represent a titration. a basic solution titrated with an acid an acidic solution titrated with a base Hd HdC. Titration of acid by a base Standardization of NaOH Volume of NaOH Mass of KHP Initial buret Final buret Trial used Molarity of NaOH (g) reading (mL) reading (mL) (mL) (1) (2) (3) (4) (5) 1.2075 0.7 25 24.3 0.243 (6) (7) (8) (9) (10) 1.2062 16.4 40.9 24.49 0.2412Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Expected color at end point Volume of NaOH used (mL) 48.08 47.98 47.89 Compute for the ff: a. Average moles of acetic acid (mol)? b. Average molarity of acetic acid (M)? c. Average molarity of acetic acid (M)?
- Titration Experiment 1: Acid-Base Titration: Unknown HCl Write chemical equation *+ HClcags N s → Naclceg) + H,O Write NIE OH c) + HEogs → H2OC) Enter the data into the table and choose three titrations to find the molarity of the unknown HCI. Unknown # HCI Titration 1 Titration 2 Titration 3 Titration 4 Titration 5 Volume NaOH used to titrate unknown HCI solution 17.43ml 16.5O ml662 mll16.57ml16.6dmL Molarity of NaOH used for each titration 0.2564 0.1787/01692/0.1704/oiado1703 Molarity of HCI Average M HCI (avg ± standard deviation) 10.1717 1.63 % Precision Calculations 1. Provide one representative calculation that you used to determine the molarity of HCI. Be sure to show all units and use proper sig figs! V HCI-25mL MHCI =? VN2OH = 16.6lmL MNAOH=0.2564 MHCI VHCI=MNAOH VAa OH MHCI 25=O. 1564 16.61 MHCI= 0.2564.16.61 25 MHCI=0.1703 2. Average molarity of three titrations. 6.1787+0.1692+0.1704+0.1619+ O.1703 MACI= 0.117Quantity of Acetic Acid in Salad Dressing Titration Results: 1000 μL aliquots of salad dressing against a sodium hydroxide solution Please only fill in 3 concordant results! Titration number: 1 2 3 Error Final burette reading (mL) 7.9 15 22.2 ±0.05 mL Initial burette reading (mL) 0.9 7.9 17 ±0.05 mL Titre (mL) 7 7.1 7.2 ±0.10 mL Average (mean) volume of concordant titres: 7.1 Concentration of Acetic Acid (M) (to 3 sig figs): 6.88 mL IM Concentration of Acetic Acid (as %w/v) (to 3 sig figs): % Note: %w/v = (g/mL) x 100%Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a standardized solution II. Wash the burette with a standardized solution III. Fill the burette to the 50-mL mark IV. Prepare a contrast paper to determine burette volume and titration endpoint I, Il and IV only 1, III and IV only II, III and IV only O I, II, and III only