one of the following is not applicable on Mohr method of O a. dichromate might be used to prepare the indicator O b. silver complex of the indicator is more favored in precipitation than silver bromide O c. it does not work in acidic medium O d. Ksp of silver halidel is lower than Ksp of silverhalide2 if silver halide 2 is more water soluble Next page
Q: 2. 6 M HCI is added to a solution of Ag*, Cu²+, Fe3•. A white precipitate forms. Predict which ions…
A: The ions present in the solution are : Ag+, Cu2+, Fe3+. When a 6M HCl is added to the solution and…
Q: 16 What weight of sample which contains 56.15 per cent Cl was taken for analysis if the precipitated…
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Q: to Y16! What weight of sample which contains 56.15 per cent Cl was taken for analysis if the…
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Q: 16! What weight of sample which contains 56.15 per cent Cl was taken for analysis if the…
A: First calculate moles of AgCl: Moles of AgCl = Mass/Molar mass = 0.5017g/(143.32gmol-1) = 3.5 ×10-3…
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Q: The % (w/w) I- (MM = 126.9) in a 0.5812-g sample was determined by Volhard titration. After adding…
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- The sulfur content of insoluble sulfides that do not readilydissolve in acid can be measured by oxidation with Br2to SO42.25Metal ions are then replaced with Hby an ion-exchange column,and sulfate is precipitated as BaSO4with a known excess ofBaCl2. The excess Ba2is then titrated with EDTA to determinehow much was present. (To make the indicator end point clearer,a small, known quantity of Zn2also is added. The EDTA titratesboth the Ba2and the Zn2.) Knowing the excess Ba2, we cancalculate how much sulfur was in the original material. To analyzethe mineral sphalerite (ZnS, FM 97.46), 5.89 mg of powderedsolid were suspended in a mixture of CCl4and H2O containing1.5 mmol Br2. After 1 h at 20 C and 2 h at 50 C, the powder dis-solved and the solvent and excess Br2were removed by heating.The residue was dissolved in 3 mL of water and passed throughan ion-exchange column to replace Zn2with H. Then 5.000 mLof 0.014 63 M BaCl2were added to precipitate all sulfate as BaSO4.After the addition of…Which of the following statements is true regarding permanganimetry? a) Permanganate solution can oxidize water which is catalyzed by the presence of manganese dioxide or manganese ion. b) The light pink endpoint color for permanganimetry tends to fade with time due to the catalytic reaction. c) Standardization of the permanganate titrant is carried out at elevated temperature with sodium oxalate. d) all of these e) none of theseWill Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.
- In the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgil must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m 1.2m? (b) If -3 the concentration of chromate indicator ased is 5 x 10M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin?(a) For the precipitation reaction: A+ + B– AB(s)Calculate the value of the equilibrium constant for 99.99% conversion to AB atthe equivalence point, assuming that the analyte content is 5.00 mmole and thetotal volume at the equivalence point is 100.00 mL.(b) What factors affect end-point sharpness in a precipitation titration? Explain.(c) Explain briefly why silver nitrate is an important reagent used in precipitationtitrations.(d) Mohr Method, Volhard Method and Fajans Method are commonly used for thevolumetric analysis of chlorides. Distinguish the three methods in terms of thetitrants and indicators used, and how the titrations are carried out.Chromel is an alloy composed of nickel, iron and chromium.A 0.6472 g sample was dissolved and diluted to 250 mL. When a50 mL aliquot of 0.05182 M EDTA was mixed with an equal volumeof the diluted sample and all the three ions were chelated, a 5.11 mLback titration with 0.06241 M copper (II) was required.The chromium in a second 50 mL aliquot was masked through theaddition of hexamethylenetetramine, titration of the Fe and Nirequired 36.28 mL of 0.05182 M EDTA.Iron and chromium were masked with pyrophosphate in a third50 mL aliquot and the nickel was titrated with 25.91 mL of theEDTA solution.Calculate the percentage of nickel, chromium and iron in thealloy.
- An antihistamine sample, brompheniramine maleate, weighing 5.01234 g was dissolved in alcohol and decomposed with metallic sodium. The resulting solution was treated with 12.00mL of 0.3121M AgNO3 to precipitate all of the liberated bromide ions as AgBr. The excess AgNO3 remaining in the solution was titrated with 9.123mL of 0.2181M KSCN to reach the endpoint. What is the %Br in the sample? Br- + Ag+ --> AgBr(s) Ag+ + SCN- --> AgSCN(s) Br = 79.904 g/molFor µ=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X- is 0.75. Calculate how many micrograms of MX2 dissolve in 324 mL of 0.10 M NaX solution. The molar mass of MX2 is 201 g/mol, and its Ksp is 3.8 x 10-9. Note that NaX is a salt of X-, an ion that participates in the equilibrium that applies to the solubility of MX2. a. 110 µg b. 27 µg c. 9.7 µg d. 44 µg e. 1000 µgTwo hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is 3.20 × 10–5, what is the Ksp value for LQ?
- Two hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is 3.20 10–5, what is the Ksp value for LQ?A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 MNa2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer untilthe pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator.Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, onwhich the solution will turn red. Calculate for the molarity of the unknown.A. Calgon conditioning can be done by____________________________.B. The colour of metal-EBT complex is ___________________________ .C. If P is less than half M (or T) then alkalinity is due to _____________________.D. Hydroxide alkalinity is determined by ____________________ indicator.E. If sample water contains Mg(HCO3)2 = 14.6 mg/lit, Ca(HCO3)2 = 16.2 mg/lit, MgCO3 = 8.4mg/lit. The temporary hardness present per litre of the sample is__________________.