A 0.1017-g sample of KBro, (MM 167.0) was dissolved in dilute HCl and treated with an unmeasured excess of KI. The liberated 12 required 39.75 ml of a sodium thiosulfate solution. Calculate the molar concentration of the Na,S,0; 61 + Bro, + 6H* → 31, + Br + 3H,0 25,0,2 + 1, → 21 + S,0¿²
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- A 30 ml solution of I- was treated with 50 ml of 0.365 M AgNO3. The resulting AgI precipitate was filtered. The resulting filtrate was back-titrated with 37.60 ml of 0.287 M KSCN. According to these data, how many grams of I- are in the sample? (I:127) (Ag:107,86),(N:14),(O:16),(K:39,098),(C:12,011),(S:32,066)Calcium in a 5.00 mL urine sample was precipitated, redissolved and required 16.15 mL of 0.1157 N KMnO4. Calculate the % (w/v) of calcium in the urine.5. 0.1500 g sample of chromium ore was dissolved and the chromium oxidized to chromate ion. The solution was treated with 25.00 mL of 0.3500 M AGNO3. The resulting precipitate, from the reaction of the excess and analyte in 1: 1 mole relationship, Ag2CrO4 was removed and discarded. The excess AGNO3 required 30.50 mL of 0.200 M KSCN for titration in a 1:1 mole relationship. Calculate the % Cr2O3 in the ore if the mole relationship between Cr2O3 and CrO42- is 1:2 respectively.
- A sensitive method for 12 in the presence of Cl₂ and Br₂ entails oxidation of the 1₂ to 103 with Br₂. The excess Br₂ is then removed by boiling or by reduction with formate ion. The 103 produced is determined by addition of excess 1₂ and titration of the resulting 1₂. A 1.307-g sample of mixed halides was dissolved and analyzed by the foregoing procedure. A volume of 19.72 mL of 0.04926 M thiosulfate was required for the titration. Calculate the percentage of KI in the sample.A solid containing tris was dissolved in water and brought to a total volume of 50.00 ml. A 10.00 ml aliquot of the solution was titrated with 0.09978 M HCl to a bromcresol green endpoint. The aliquot consumed 38.93 ml of titrant. Calculate the weight of tris in the original sample.A sample of Al;(SO.); weighing 7.52-g was dissolved in enough water and diluted to 250.0-mL. 100.0-mL of the dilution was transferred to another flask, 10.0-mL of 0.050M EDTA, 20-ml of buffer solution, 50-mL of alcohol and 2.0-ml dithizone TS were added. The resulting solution required 8.7-mL of 0.031M ZnSO, to reach the endpoint. (Note: Each ml of 0.050M EDTA is equivalent to 16.66-mg Al:(SO.);•18H;0). Compute for the percent purity of the sample.
- 4. A 0.1017 g sample of KBRO, (MM=166.1) was dissolved in dilute HCI and treated with an unmeasured excess of KI. The liberated iodine required 39.75 mL of Na:S:03. Calculate the molar concentration of sodium thiosulfate. 1 mol BrO3 = 3 mol 1: = 6 mol S:0:22) A 100.0-mL sample of spring water was treated to convert any iron present to Fe2*. Addition of 25.00 mb. of 0.008 M K2Cr207 resulted in the reaction 6F22+ + Cr2O72- + 14H*2 6FE3+ + 2Cr3+ + 14H2O The excess K2C12O7 was back-titrated with 8.53 ml of 0.00949 M Fe2* şolution. Calculate the molar concentration of iron in the sample.The digestion of a 0.1432 g sample of a compound containing phosphorous in a mixture of HNO3 and H2SO, resulted in the formation of CO2, H2O and H3PO4 Addition of ammonium molybdate yielded a solid having the composition (NH)3PO, 12M0O3 (MW=1876.3 g/mol). This precipitate was filtered washed, and dissolved in 50 00 mL of 0.2000 M NaOH: (NH,)3PO4-12MO03(s)+ 26OH (aq) HPO,2 (aq) +12M00,2 (aq) +14H2O(1) + 3NH3(g) After the solution was boiled to remove NH3, the excess NaOH was titrated with 14.71mL of 0.1741 M HCI to a phenolphthalein end point (back titration). Calculate the percentage of phosphorous in the solid sample. 6.19% 10.6% O 27.6% O0 238% O 19.5
- A solution containing 50.0 mL of 0.100 M EDTA buffered to pH 10.00 was titrated with 50.0 mL of 0.020 0 M Hg(CIO4): S.C.E. || titration solution | Hg(l) From the cell voltage E = –0.027 V, find the formation constant of Hg(EDTA)²¯A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br- The liberated nickel ion required 11.70 mL of 0.002146 M EDTA. Calculate mmol Ni in the 50.00 mL aliquot. Calculate mmol Br- in the 50.00 mL aliquot. Calculate the percentage of NaBr (102.894) in the 1.000 g sample.A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br-50.00 mL remaining solution was analyzed for its Br- content by potentiometry using a metallic electrode of the second kind. a) Write the cell notation of the potentiometric set-up with SCE as the reference electrode. b) Write the Nernst equation that describes the indicator electrode set-up. Ecell recorded in running the solution using the potentiometric set-up was Ecell = 0.0286 V. (E0Ag/AgBr = 0.095 V) c) Compute for Eind. d) Compute pBr in the 50.00 mL aliquot. e) Compute for % NaBr ( in the potentiometric technique).