[ 2nd ] Instructions: Kindly provide the complete and correct solutions. (There are some questions that needs to be based in a periodic table, kindly base it on the one I provided below) I won't like it if it is incomplete and incorrect. 2. A river water sample was titrated against 0.0250 M EDTA totest its hardness of 0.0250 M EDTA. A 50.00-mL aliquot,prepared with NaOH, was titrated with 14.53 mL of the sameEDTA titrant. Another 50.00 mL aliquot was prepared andbuffered to pH 10.0, it required 23.55 mL Calculate thefollowing.a. Total hardness (ppm Caco).b. Calcium hardness (ppm CaCO3).c. Magnesium hardness (ppm MgCO3).[Identify which titration values corresponds to which hardness analysis. Use the titrationvalues and metal + EDTA stoichiometric relationship to find the amount of metal, use thisvalue to find the ppm.] PERIODIC TABLE OF THE ELEMENTSIA1HHABANAVIA16VIIA171.012VA15713143568LIBeс12.019.016.9411B108113Al Si26.98 28.09N14.0115O16.0016F19.001712HIBIVBVBV16VIIBV48n18118Na22.9919Mg24.313456789101112202122232425262029CaScTiVMnFe55.8540.0830Cu Zn63.55 65.394744.9647.87K39.1037Rb85.4750.9454.94CI35.4535Br79.90531Ni58.694627Co58.9345RhPdAgCd102.91 106.42 107.87 112.4130.97 32.073134Ga GeSe69.72 72.6478.96495052In Sn Sb Te11482 118.71 121.76 127.60 126.90As74.925138Cr52.0042Mo95.9474394048SrY88.91Zr91.2287.6256Nb92.9173Tc(98)7571727980818555CsBa Lu132.91 137.33 173.04HfTaWReRu101.07767776Os Ir Pt190.23 192.22 195.08108109110HsMt Ds(269) (278) (281)82Au Hg TI Pb196.97 200.59 204.38 207.2011111211311483Bi208.98115178.49180.95183.84 186.2184Po(209)116LV Uus(293) (294)At(210)1171031041051061078788Fr RaLrRfSg BhDb(268)UupRg Cn(280)Uut FI(286) (289)(223) (226) (262)(267)(269)(270)(285)(288)57585960616266CeLanthanideSeriesLa138.91 140.12Pr Nd140.91 144.24Pm(145)9363Sm Eu150.36 151.96676869Dy Ho Er Tm162.50 164.93 167.26 168.9370Yb173.046465Gd Tb157.25 158.93969798Cm Bk Cf(247) (247) (251) (252)90921001011028991Ac Th Pa(227) 232.04 231.04 238.03Actinide95Np PuAm(237) (244) (243)99EsFmMdNoSenes(257)(258)(259)CF182He4.0010Ne20.1818Ar39.9536Kr83.8054Xe131.2996Rn(222)118Uuo(294)

Answered: Image /qna-images/answer/d287f733-910c-4067-a7c6-608ae2d664e9.jpg

2. A river water sample was titrated against 0.0250 M EDTA to test its hardness of 0.0250 M EDTA. A 50.00-mL aliquot, prepared with NaOH, was titrated with 14.53 mL of the same EDTA titrant. Another 50.00 mL aliquot was prepared and buffered to pH 10.0, it required 23.55 mL Calculate the following. a. Total hardness (ppm Caco). b. Calcium hardness (ppm CaCO₂). c. Magnesium hardness (ppm MgCO3).

2. A river water sample was titrated against 0.0250 M EDTA to test its hardness of 0.0250 M EDTA. A 50.00-mL aliquot, prepared with NaOH, was titrated with 14.53 mL of the same EDTA titrant. Another 50.00 mL aliquot was prepared and buffered to pH 10.0, it required 23.55 mL Calculate the following. a. Total hardness (ppm Caco). b. Calcium hardness (ppm CaCO₂). c. Magnesium hardness (ppm MgCO3).

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.31QAP

See similar textbooks

Similar questions

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.
A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0493 M EDTA. The endpoint volume was 42.15 ml. A second aliquot of the same mixture was made strongly basic by the addition of NaOH – this causes the Mg2+ to precipitate as Mg(OH)2. The solution was then titrated with the 0.0493 M EDTA and the endpoint volume was found to be 35.65 ml. Calculate the molar concentration of Mg
A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0499 M EDTA. The endpoint volume was 40.17 ml. A second aliquot of the same mixture was made strongly basic by the addition of NaOH – this causes the Mg2+ to precipitate as Mg(OH)2. The solution was then titrated with the 0.0499 M EDTA and the endpoint volume was found to be 34.70 ml.
Use the following atomic masses (in g/mol): Ca = 40.08; C = 12.01; O = 16; Na = 23; Cl = 35.45 1.) Calculate the CaCO3 content of a chalk sample weighing 0.2545g, consuming 16.67mL of 0.1150M Disodium EDTA in titration.
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.
3. An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation. After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask, and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation ofthe end point was equal to 13.03 mL. Based on this information,a) Outline the two steps involved, representing the related reactions./5b) Calculate the concentrations of CaCO3 and MgCO3 present in the initialsolution./6c) Calculate the masses of CaCO3 and MgCO3 present in the pellet./6d) Calculate the…
A solution was prepared by dissolving about 30.00m g of EDTA in approximately 1 L of water and standardizing against 50.00-mL aliquots of 0.004356 M Mg2+. An average titration of 32.65 mL was required. Calculate the molar concentration of the EDTA.
Volhard titration. A 30.00-mL solution of unknown I2 was treated with 50.00 mL of 0.365 0 M AgNO3. The precipitated AgI was filtered off, and the filtrate (plus Fe31) was titrated with 0.287 0 M KSCN. When 37.60 mL had been added, the solution turned red. How many milligrams of I2 were present in the original solution?
An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask. and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, (a) Outline the two steps involved, representing the related reactions. (b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution. (c) Calculate the masses of CaCO3 and MgCO3 present in the pellet. (d) Calculate the…
. An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation. After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask, and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, a) Outline the two steps involved, representing the related reactions./5 b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution./6 c) Calculate the masses of CaCO3 and MgCO3 present in the pellet./6 d) Calculate…
A 30-mL portion of a solution containing Ca2+ and Mg2+ was titrated with 28.19 mL of 0.213 M EDTA at pH 10. Another 30-mL aliquot of the same Ca-Mg mixture was treated with NaOH to make the solution strongly alkaline and precipitate Mg(OH)2. This solution was then titrated with the same EDTA solution. What would be the required EDTA volume (in mL) to reach the endpoint of the second aliquot if it was found that there was 0.061 M of Mg2+ in the sample?
What is the ppm Zn in the orginal foor powder sample, after dissolving 50.0 ml of good water, the zinc in a 0.3232 gram sample of foot powder was titrated at a pH=11.0 with 19.67 ml of a 0.01222M EDTA solution