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- A silver nitrate soluti on contains 14.77 g of primary standard AGNO3 , in 1.00 L what volume of this solution is needed toreact completely with 50.00 ml. of 0.01808 M Na2S. 1. O10.40 ml. 2. O 20.79 ml. 6.10 ml. 4. O12.31 ml. 5. O18.21 ml. 3.Determinati 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…Fertilizer sample 1.150 g containing SO4 -2 ion is dissolved in 500ml dist. Water. 100ml of the solution was precipitated with BaCl2 solution as BaSO4 weighing 0.436 g. % mass of SO42- = ?
- Answ GA 20. Answ My C X C Write C The F X C Whe x akeCovalentActivity.do?locator=assignment-take [Review Topics] [References) Use the References to access important values if needed for this question. When 25.0 mL of a 1.99×104 M lead nitrate solution is combined with 15.0 mL of a 6.28×10-4 M sodium iodide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to Submit Answer Retry Entire Group 1 more group attempt remaining क Ni ENG US Home End Inso/index.html?deploymentld%=55750828934189288909969212&eiSBN=9781305657571&snapshotld%32199898&id%3... ☆ IDTAP Q Search this cou Use the References to access important values if needed for this question. The concentration of H3ASO3 in a solution is determined by titration with a 0.1945 M Ce+ solution. The balanced net ionic equation for the reaction is: 2Ce*(aq) + H3ASO3(aq) + 5H2O(1) 2Ce*(aq) + H3ASO4(aq) + 2H3O*(aq) (a) If 19.83 mL of the 0.1945 M Ce** solution are needed to react completely with 30.00 mL of the H3ASO3 solution, what is the concentration of the H3ASO3 solution? M (b) Which of the two solutions was in the buret during the titration? (c) Suppose at the end of the titration, the solution containing the Ce³* ion is transferred to a volumetric flask and diluted to 300. mL. What is the concentration of Ce3+In the diluted solution? Submit Answer 5 question attempts remainingName: Date: Section: Data Report Sheet: Determination of Iron by Reaction with Permanganate: A Titration Unknown # We 01 X E Trial I Trial II III [BL Mass of Unknown 0.512 Initial Burette mL 0.00 mL Final Burette mL 20.5mL mL 0.2 Total MnO, Added Moles MnO, Added Moles Fe?+ Present Grams Fe²* Present Weight % Fe Average Weight % Fe in Sample
- E. Analysis of a mixture consisting of NaOH + NażCO3 + inert matter gives the following data: Sample portions are titrated. With one portion, an end point with phenolphthalein is obtained in cold solution, with 44.52 mL of 0.5000 N HCI. The other portion requires 46.53 mL of the acid for an end point with methyl orange. Calculate the percentage composition of the original sample. 10.00 g. Its aqueous solution is diluted to 250.0 mL and two separate 25.00 mL10. A 0.514 gram sample of NazCO, (106.0 g/mol) was dissolved in distilled water in a 100.0 mi volumetric flask. The molar concentration of Na,CO, in solution is: 0.0485 M 0.0370 M b. 0.4849 M 0.0340 M 0.0330 M d. е.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 choice
- A solution is made by mixing 500.0 mL of 0.04540 M Na, HASO, with 500.0 mL of 0.02245 M NaOH. Complete the mass balance expressions for the sodium and arsenate species in the final solution. (HASO + M [Na*] = M étv hulu MacBook Pro G Search or type URL 24 4. & 6 8 RI Y U F H K V. 0O1. 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/LA limestone sample weighing 400 mg was dissolved in acid treated with excess sodium oxalate. The solution was made basic and the resulting calcium oxalate was filtered, washed and redissolved in dilute acid. This solution required 14.0 mL of 0.00865 M KMnO4. What is the % Ca of the limestone.