6. A strong brine (mostly NaCl) is contacted with the exhausted resin to replace Ca with Na. The composition of the brine (regenerant) after equilibrating with the exhausted resin is: Nacl = 1.9 eq/L and CaCl2 = 0.28 eq/L. Most of the Ca is from the spent column. Na in the fresh brine would have been slightly higher than 2 eq/L. For this resin. C = 2.2 e9/L KCa2+ Na+ = 3.9 Calculate percentage of regeneration that can be accomplished with this regenerant ! alculate percentage of regeneration that can be accomplished with this

6. A strong brine (mostly NaCl) is contacted with the exhausted resin to replace Ca with Na. The composition of the brine (regenerant) after equilibrating with the exhausted resin is: Nacl = 1.9 eq/L and CaCl2 = 0.28 eq/L. Most of the Ca is from the spent column. Na in the fresh brine would have been slightly higher than 2 eq/L. For this resin. C = 2.2 e9/L KCa2+ Na+ = 3.9 Calculate percentage of regeneration that can be accomplished with this regenerant ! alculate percentage of regeneration that can be accomplished with this

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

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According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
The CO in a 20.3-L sample of gas was converted to CO2 by passing the gas overiodine pentoxide heated to 150℃, and I2 was distilled and collected to 8.25 mL of 0.01101 M Na2S2O3, then back titration with 2.16 mL of 0.00947 M I2 solution.Calculate the mg of CO (28.01 g/mol) per liter of sample.a. I2O5(s) + 5CO (g) → 5CO2(g) + I2 (g)b. I2(aq) + 2S2O32- (aq) → 2I-(aq) + S4O62- (aq)
Toxie chromate can be removed from solution uning the following reaction 2 Cro, lag) + 3SO4H'(ag)- Cry(SOls) + 2HyOA 5o, Is bubbled through 3.0x 10Lofa solution. All of the chromate is removed and 2.94 x 10 kg of the precipitate is formed. Calculate the initial concentration (in units of mM) of chromate in solution. Write only the numerical value below (without units) using the correct number of signihcant hpares. Type your answer Nest
A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.
A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.3172-g sample is dissolved in 50 mL of water and titrated to the Ag,CrO4 end point, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.
1. Determine the mass of CaCl2·2H2O (MW 147.02 g/mole) to weigh out using a four- place analytical balance to prepare 100 mL of a 0.1005 M solution of Ca2+. 2. Determine the mass of KCI to weigh out using a four-place analytical balance to prepare 100 mL of a 1 M solution of KCI (MW 74.5513 g/mole). 3. Record the solubility of calcium carbonate in water (mg/L) in your notebook. 4. Calculate the amount of calcium carbonate (mg) not in solution if a tablet is dissolved in 250 mL of water and the tablet's label claim is 600 mg calcium / tablet.
Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of commercial bleaching solution titrated ?
Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Mass of NaOCl in the diluted bleach titrated. ?
A 0.6560 g mixture of KCN (MW=65.116 g/mol) and NaCN (MW=49.005 g/mol) was dissolved in water. AgNO3 was added to the solution, precipitating all of the CN− in solution as AgCN (MW=133.886 g/mol). The dried precipitate weighed 1.505 g. Calculate the weight percent of KCN and NaCN in the original sample. KCN wt% = ~ 66.01 NaCN wt% = ?
TOPIC: GRAVIMETRY SHOW THE SOLUTION The mercury in a 0.7152-g sample was precipitated with an excess of paraperiodic acid, H5IO6, according to the following reactions:5 Hg+2 + 2 H5IO6 ---> Hg5(IO6)2(s) + 10 H+The precipitate was filtered, washed free of precipitating agent, dried and found to weigh 0.3408-g. Calculate the percentage of Hg2Cl2 in the sample. Molar Masses: Hg5(IO6)2 = 1448.75 Hg2Cl2 = 472.09 Answer: 38.82% Hg2Cl2 An iron ore was analyzed by dissolving a 1.1324-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron (III) was precipitated as the hydrous oxide Fe2O3·xH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe2O3. Calculate (a) % Fe, and (b) % Fe3O4 in the sampleMolar Masses: Fe2O3 = 159.69 Fe = 55.847 Fe3O4 = 231.54 Answer: 33.32% Fe and 46.04% Fe3O4
A 4.932-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 3% H2 O2. Reaction: SO2 (9) + H2 O2 → H2SO4 A 28.00-mL portion of 0.00878 M NaOH was introduced into the solution of H2SO4, following which the excess base was back-titrated with 15.27 mL of 0.01160 M HCI. Calculate the sulfur concentration in the sample in parts per million. Concentration = ppm
Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)