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ASAP.
Please refer to second picture to answer the question.
The answer to second picture are:
a) 1.49
b.) 148.92
Step by step
Solved in 4 steps
- Standardization of 1N H2SO4 Titration 1 Titration 2 Titration 3 Titration 4 Mass of flask and Sodium Carbonate 1.5067 g 1.5098 g 1.5076 g 1.5077 Final buret reading (mL) 22 mL 22mL 21.5 mL 22.5 mL Volume of Sulphuric acid used (mL) 30 mL 30 mL 30 mL 30 mL What is the result of my titration?Part 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: _______________Table 1. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48 1.89 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) 49.32 49.06 49.93 Table 2. Titration data Table view List view Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48 1.89 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) 49.32 49.06 49.93 Expected color at end point Choose... Choose... Choose... Volume of NaOH used (mL) 1. Average Volume of NaOH used in liters 2. Average moles of NaOH used (mol) 3. Average moles of acetic acid (mol) 4. Average molarity of acetic acid (M) 5. Average mass of acetic acid (g)…
- 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= 0.117Do you always have to use a primary standard in the standardization of titrant? Why or why not?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 Hd
- What is Analyte and Titrant? Explain each in 3-5 sentences.C. 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 0.2412For your fine titrations, after reaching the x-1 mL mark from your rough titration, you should add EDTA in 1 mL increments until you reach the endpoint. True False
- What is the best sequence of steps for filling the burette with NaOH for a titration? Lower the burette to eye' level, insert the funnel in the top of the burette, slowly add the NaOH through the funnel, check the burette stopcock is closed O Check the burette stopcock is closed, lower the burette to eye level, insert a funnel in the top of the burette, slowly add the NaOH through the funnel Check the burette stopcock is closed, insert the funnel in the top of the burette, slowly add the NaOH through the funnel, lower the burette to eye levelWhich one of the following is NOT a source of error during a titration? Group of answer choices Adding too much sodium hydroxide solution to the analyte Refilling the buret during a titration trial Rinsing the buret with the analyte Adding indicator to the analyteWhy should we do a standardization every time we do a titration?