Trial % Acetic Acid 1 5.292 5.940 5.828 f. How much NaOH solution in mL would you have used per trial. g. Report %Acetic acid content of the sample as mean tsd. 23
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- 5. From the stock solutions of 1.00-mol L acetic acid and 1.00-mol L of sodium acetate, six solutions were prepared with the acetic acid and acetate concentrations shown in the table below. The pk of acetic acid is 4.756. [Acetic acid). [Acetate). Final volume, Solutio mol L mol L ml A. 0.10 100 0.0000351 100 0.10 0.10 100 0.010 0.010 100 0.10 0.15 100 0.15 0.10 100 -1 Determine the volume of the stock solutions of 1.00-mol Lacetic acid and 1.00-mol L of sodium acetate needed to prepare the solutions. Write your answer in the table below. a. Vol. acetic acid, ml Vol. of acetate, ml Solution A b. Calculate for the initial pH of the solutions and write the pH in the table below. Solution Initial pH A Which solution(s) have the same pH? C.apacit d. The purity of KHP standard was taken as 100% when in actual it was not. Clear my choice A 10.00 ml sample of Y(OH)2 was titrated to the stoichiometric point with 14.50 mL of 0.2345 M H2X. The total number of moles of Y(OH)2 is O a. 0.0034 O b. 0.00469 O c. 0.00034 O d. 0.0068 Clear my choice2. In one gravimetric analysis, the aluminum in a 1.2g sample of impure NHAI(SO4)2 was precipitate as hydrous ALO3.XH2O. The precipitate was filtered and ignited at 1000 °C to give anhydrous Al2O3 which weighed 0.1798g. Calculate the % Al inthe sample. 3. A sample of 0.4500g impure potassium chloride was dissolved in water treated with excess silver nitrate solution. 0.8402 g of silver chloride was precipitated. What is the percentage of potassium chloride in the sample?
- A (aq) + ...B(aq) C(s) + D (aq) ... .. Experimental | Volume of B/ mL Mass of Run precipitate/g 1 1.2 5.40 2 1.4 7.24 1.6 9.02 4 1.8 9.90 2.0 10.86 6. 2.2 10.90 7 2.4 10.88 8 2.6 10.84 9. 2.8 10.86 A series of experiment was performed to determine the mole ratio of a given reaction. 1 mL of 1 Molar A added to nine beakers, then the increasing amount of 1 Molar B added to these beakers. Volume of B and mass of precipitate of C are given in the table below. Find the mole ratios through plotting a graph.Mass of Sample Volume of KMnO, solution used in titration Equivalents of permanganate used Equivalents of iron (II) in sample Moles of iron (II) in sample Grams of Iron in Sample % Iron in Sample Average % Iron in Unknown Instructor's Grade for Precision in Part B. Sample Calculations Part B: 0.58179 0.68719 28.19 ml 31,96m6 007662 00266 2 11 nDeterminati an 25 ml by dissolving 110n (111) per 1 This (as ml 750ml experiment Solution The to of was The a and process Q on added The portion layer taken 1 volumetric diluted Litre Colution Two These of in diluted ml soo 1% ETA of Question A. reaction an Solution 0₁ 446 9 of A. R. hydrated sulphate, (NH4) Fe (504) ₂ · 12H₂0 2 of distilled then of wertel) 0,0446 g/L of lion Absorbance was 250 ml in to ·layers frask was Is 2. 3. Was Chlore form and were 5 ml, 10 ml, 15 ml por tions 4. Iron • iron (111) four oxine it mixture the done. (111) seperatory conducted Volume SMT as 10 ml 15 ml 20 ml Plo + absorbance formed readings a (A.R) Jayer measured the por tions Solution was Water diluted out 20 ml were then Each of these mark against funnel as was after with for 8- ity droxy quinolate. follows. to iron (111) solution was prepared of then Calibration was ) 10 obtain collected. ammonium F. W-481,979 then these Absorbance 0,076 0,169 9185 0₁234. Shook. the shaking added portions…
- The chloride in the sample is to be determined gravimetrically by precipitating and weighing AgCl. What weight in grams of sample should be taken so that the percentage of Cl is obtained by simply multiplying the weight of the AgCl precipitate by 10?1. One of the methods of eliminating interferences, is by adding solvents to the solution in which components to be removed are soluble, which method is this? a. Complexation b. Extraction lon-exchange d. Precipitate С. 2. Which of the following properties of precipitates is desired in gravimetry? a. Large b. Pure С. Free of contaminants d. All of the choicesDATA AND RESULTS: Titration Data (Standardization of EDTA) Example II Mass, g Caco, 0.0250 0.0251 0.0246 0.0254 Final reading, mL 25.00 24.91 24.87 25.31 Initial Reading, mL 0.00 0.02 0.02 0.02 Volume, mL EDTA 25.00 Molarity of EDTA, M 0.009992 B. Analysis Data Example II Volume of Sample, mL 25.00 24.90 25.10 25.0 Final reading, mL 27.46 25.08 25.06 24.99 Initial Reading, mL 0.00 0.02 0.02 0.02 Volume of EDTA, mL 27.46 Molarity of EDTA, M 0.009992 Ca" concentration, ppm 440 STATISTICAL EVALUATION OF RESULTS Standardization of EDTA Mean, M EDTA Median, M EDTA Standard Deviation Ci for u at 95% Prob. Level Reported value: M EDTA Ca" Concentration Mean, Ca" ppm Median, Ca" ppm Standard deviation Cl for u at 95% Prob. Level Reported value: Ca" ppm
- A 0.64 g sample containing KCl ( mw = 74.6 ) is dissolved in 50mL of water and titrated to the Ag2CrO4 end point, requiring 26.2 mL of 0.15 M AgNO3 .The %w/w KCl in the sample is ?1. Molarity of the NaOH solution 0.238 mol/L Trial 1 Trial 2 Trial 2. Volume of H;PO4 added to flask 22.0 mL 22.0 mL 22.0 mL 3. Initial NaOH volume _0.25_ mL _0.75_ mL 0.55 mL 4. Final NaOH volume 17.60_ mL 18.20_ mL _17.90_ mL 5. NAOH volume used for titration to reach green end point mL mL mL 6. NaOH volume used for titration 7. Moles of NaOH used for titration mol mel mel 8. Moles of H;PO4 that reacted mol mel mol 9. Volume of H;PO4 added to flask L 10. Molarity of H3PO4 mol/L mol/L mol/L2. A 0.5131-g sample containing KBr is dissolved in 50 mL distilled water. Titrating with 0.04614 M AgNO3 requires 25.13 mL to reach the Mohr endpoint. A blank titration requires 0.65 mL to reach the same endpoint. Report the % (w/w) KBr in the sample. [Ans. 26.19 % (w/w)]