For the determination of Ca in blood serum, 5 mL of a serum sample is taken and the Ca2 + in it is precipitated as CaC204. The precipitate is filtered, dissolved in acid and titrated with 0.001 M KMN04 by heating. Calculate the Ca concentration in the sample since 4.94 mL of KMN04 was used.
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- For the determination of Ca in blood serum, 5 mL of a serum sample is taken and the Ca2 + in it is precipitated as CaC2O4. The precipitate is filtered, dissolved in acid and titrated with 0.001 M KMnO4 by heating. Calculate the Ca concentration in the sample since 4.94 mL of KMnO4 was used.A 0.574-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the evolved gases in a solution of NaOH. After neutralizing, the sample was treated with 26.21 mL of a 0.28 M AgNO3 solution. This precipitated the chloride (Cl-) out as AgCl and left an excess of AgNO3. The excess AgNO3 was titrated with 0.122 M KSCN and required 24.91 mL to reach the endpoint in a Volhard titration. Calculate the % w/w Cl– (35.45 g/mol) in the sample. Provide your answer to 2 places after the decimal point and without units. Reactions: Cl– + Ag+ → AgCl(s) Reaction 1 Ag+ + SCN– → AgSCN(s) Reaction 2A 0.2420 g sample cntg. Calcium is dissolver and the metal precipitated as CaC2O4. The ppt. is filtered, washed and redissolved in acid. The pH is adjusted, 25 ml of 0.0400 M EDTA added and the xcss EDTA titrated with 33.28 ml of 0.012102 M MG2+. Calculate the % Ca (40.078) in the sample.
- The brine solution has a significant amount of chloride, and it is determined by the Volhard method. A 10.0-aliquot of the solution is treated with 15.25 mL of standard 0.1163 M AgNO3 solution. The excess silver is titrated with standard 0.101 M KSCN solution, requiring 3.28 mL to reach the red Fe(SCN)2+ end point. Calculate the concentration of chloride in the brine solution in mg/L and g/L.Chloride in a brine solution is determined using Volhard method. A 10.00 mL aliquot of the solution is treated with 25.00 mL standard 0.1182 M AgNO3 solution. The excess silver is titrated with standard 0.1010 M KSCN solution, requiring 12.38 mL to reach the red Fe(SCN)2+ end point. Identify the (a) indicator (b) end point color (c) molarity of the Cl- in sample.Chloride in a brine solution is determined by the Volhard method. A 10.00 mL aliquot of the solution is treated with 15.00 mL standard 0.1182 M AgNO3 solution. The excess silver is titrated with standard 0.1010 M KCNS solution, requiring 2.38 mL to reach the endpoint. Calculate the concentration of chloride in g NaCl/liter.
- 1.0 g of a solid sample known to contain a mixture of NaOH and Na2CO3 is dissolved with distilled water and completed to 25 mL. By adding 2 drops of phenolphthalein (pT = 9.0) to the solution obtained, it was titrated with 0.107 M calibrated HCl solution, and the consumption was determined as 10.6 mL. Subsequently, 2 drops of methyl red (pT = 4.4) were added onto the same solution and titrated, the consumption was determined as 6.1 mL. Accordingly, calculate the amount of NaOH and Na2CO3 in the sample solution as% (a/a) by writing the related reactions. (Na: 23, C: 12, O: 16, H: 1 g / mol)Chromel is an alloy composed of nickel, iron and chromium. A 0.6553-g sample was dissolved and diluted to 250.0 mL. When a 50.00-mL aliquot of 0.05173 M EDTA was mixed with an equal volume of the diluted sample, all three ions were chelated, and a 5.34-mL back titration with 0.06139 M copper (II) was required.The chromium in a second 50.0-mL aliquot was masked through the addition of hexamethylenetetramine; titration of the Fe and Ni required 36.98 mL of 0.05173M EDTA. Iron and chromium were masked with pyrophosphate in a third 50.00-mL aliquot, and the nickel was titrated with 24.53 mL of the EDTA solution. Calculate the percentage of Cr in the alloy. Express your answer in 2 decimal places.The phosphate in a 3.000-g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and filtrate, upon addition of 1.00 mL of 0.01 M fecl3, required 18.23 mL of 0.1377 M KSCN for titration to the end point. (a) what type of precipitation titrimetry was used. (b) which served as the indicator (c) the color at the endpoint (d) the weight percent of phosphate in the detergent.
- After solubilization, 150 mg of a silver sample is titrated with 25 mL of a solution containing 48.5 mg KCNS in 10 mL in the presence of Fe3+. Calculate the purity of Ag in the sample.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.A weighed sample of sodium nitrite was treated with 0.05 mol of ceric sulfate in solution, in air-free conditions. The resulting solution was titrated with standard Fe(II) solution and 0.01 mol of Fe(II) were required. Determine the moles of sodium nitrite present in the weighed sample. NO2– + 2 Ce4+ + H2O → NO3– + 2 Ce3+ + 2 H+ Fe2+ + Ce4+→ Fe3+ + Ce3+
