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For the lab "Spectrophotometric determination of solubility product constant" what is the procedure? and experiment plan?
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- Can you help me find the theoretical yield of precipitate in trial 1 & 2Hatsume Mei wanted to maintain the pH of a certain solution within a specified range. What should she use to accomplish this? Analyte Titrant Standard BufferBefore you proceed with the titration proper, you must first determine the exact concentration of the titrant by titrating it against a primary standard. What process is this called? A) Titration B) Spectroscopy Gravimetry D Standardization
- Write the Ksp expression for the sparingly soluble compound silver cyanide, AgCN. If either the numerator or denominator is 1, please enter 1. Ksp = Submit Answer Retry Entire Group 8 more group attempts remainingContent ra/courses/_74259_1/cl/outline for.. O 12 Steps of Gamble... m Veterans Portal O*NET OnLine EC Home | exploreheal.. Scholarships - SAL. Patient 3) In Part B of the experiment, what volume of ethyldiamine should you add? 4) Why does adding 95% ethanol to the solution cause the compound to precipitate? pH pre-lab At 1) What are you trying to calculate in part A? What are you trying to calculate in part B? 2) HF is as weak, monoptoric acid with a Ka value of 6.6x104, Calculate the pH of a 0.25 M solution of this acid. 3) If you made a buffer solution of HF and NaF, what would be the conjugate base? 4) If the concentration of HF was 0.15 M and the concentration of NaF was 0,25 M. what would be the pH of the buffer? 5) Write a reaction for the neutralization that would occur if you added a small amount of NaOH to the buffer solution desribed in question 3. Ca(OH)2 pre-lab At 1) What are you using as an indicator in this lab? What color indicates the titration has reached completion?…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= 0.117
- Preparation and Standardization of KMnO4 solution Experimental data Complete the table below. Trial 1 0.2001 g Trial 2 0.2065 g Trial 3 Weight of sodium oxalate (Na2C2O4, MM= 134 g/mol) Titration data 0.2050 g Final reading Initial reading 29.86 mL 0.00 mL 30.66 mL 30.52 mL 0.00 mL 0.00 mL Total vol. of KMNO4 used Computed Molarity of KMNO4 solution Mean Molarity Computed Normality of KMNO4 Mean Normality of KMNO4 solution Reaction Involved: Calculations:Table 12.9 (data) Buffer Initial pH pH after adding HCI pH after adding NaOH 6 8 6 4 Solution A 5-6 8 Solution B8-9 10 Solution C7 9-10 Solution D 5 Boiled distilled water 5 9-10 4 9 Table 12.10 (report) Solutions able to buffer well against acid Solutions able to buffer well against base Solutions able to buffer well against acid or base Solutions with little or no buffering ability against acid or baseIdentify 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
- The color change at the endpoint should persist for 30 seconds. Explain why the time lapse is a good titration technique.True or False Very Insoluble precipitates are not the best candidates for gravimetric analysis.which of the 6 tests are you doing if you mix two solutions together and a precipitate occurs? Color, flame Tex, acidity Test, solubility ,complex ion formation, gas producing reaction Make a statement of the test that you would like to run first during the investigation and why. A flow chart of your expected results. Safety concerns? A flow chart of the actual results. Make a table summarizing the conclusions (identity chemicals in bottles A-F). Provide brief justification