SaltMgCO3Mg(OH)2Theoretical Ksp3.5 x 10-81.8 x 10-11For the standardization of the HCI titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint.After isolating and precipitating the magnesium salt A, a portion was dissolved in distilledwater in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquotof the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthaleinendpoint.Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgCl2 required 1.51mL of the same HCl titrant to titrate a 100.0-mL solution.a. What is the molarity of the HCI titrant?b. Comparing the data in distilled water with the two possible solids, which is the mostlikely identity of the magnesium salt? Show your full solutions in getting yourconclusion.Note: Don't forget to factor in stoichiometryc.What is the average experimental Ksp for both solvents (distilled water and 0.0200M MgCl2) and individual solubility in each solvent of the magnesium salt?d. What is the percent error in the obtained Ksp value?

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Salt MgCO3 Mg(OH)2 Theoretical Ksp 3.5 x 10-8 1.8 x 10-11 For the standardization of the HCI titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99 g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint. After isolating and precipitating the magnesium salt A, a portion was dissolved in distilled water in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquot of the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthalein endpoint. Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgCl₂ required 1.51 mL of the same HCl titrant to titrate a 100.0-ml solution. a. What is the molarity of the HCI titrant? b. Comparing the data in distilled water with the two possible solids, which is the most likely identity of the magnesium salt? Show your full solutions in getting your conclusion. Note: Don't forget to factor in stoichiometry c. What is the average experimental Ksp for both solvents (distilled water and 0.0200 M MgCl2) and individual solubility in each solvent of the magnesium salt? d. What is the percent error in the obtained Ksp value?..

Salt MgCO3 Mg(OH)2 Theoretical Ksp 3.5 x 10-8 1.8 x 10-11 For the standardization of the HCI titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99 g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint. After isolating and precipitating the magnesium salt A, a portion was dissolved in distilled water in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquot of the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthalein endpoint. Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgCl₂ required 1.51 mL of the same HCl titrant to titrate a 100.0-ml solution. a. What is the molarity of the HCI titrant? b. Comparing the data in distilled water with the two possible solids, which is the most likely identity of the magnesium salt? Show your full solutions in getting your conclusion. Note: Don't forget to factor in stoichiometry c. What is the average experimental Ksp for both solvents (distilled water and 0.0200 M MgCl2) and individual solubility in each solvent of the magnesium salt? d. What is the percent error in the obtained Ksp value?..

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter12: Spectrochemical Methods

Section: Chapter Questions

Problem 15P

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
Salt Theoretical Ksp MgCO3 3.5 x 10-8 Mg(OH)2 1.8 x 10-11 For the standardization of the HCl titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99 g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint. After isolating and precipitating the magnesium salt A, a portion was dissolved in distilled water in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquot of the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthalein endpoint. Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgClz required 1.51 mL of the same HCI titrant to titrate a 100.0-mL solution. 1.) Comparing the data in distilled water with the two possible solids, which is the most likely identity of the magnesium salt? Show your full solutions in getting your conclusion. Note:Don't forget to factorin stoichiometry
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A 370.00 mL solution of 0.00190 M AB5 is added to a 200.00 mL solution of 0.00165 M CD2. What is pQsp for AD5?
What is the solubility of CuCO3 in 0.1892 M Na2CO3? Ksp(CuCO3) = 1.400e-10.
The Merck Index indicates that 10 mg of guanidine,CH5N3, may be administered for each kilogram of bodymass in the treatment of myasthenia gravis. The nitrogenin a 4-tablet sample that had a total mass of 7.50 g wasconverted to ammonia by a Kjeldahl digestion, followedby distillation into 100.0 mL of 0.1750 M HCl. Theanalysis was completed by titrating the excess acid with11.37 mL of 0.1080 M NaOH. How many of thesetablets represent a proper dose for a patient who weighs(a) 100 lb, (b) 150 lb, and (c) 275 lb?
[TITRIMETRY] Complete the table below.
1. What is the molar solubility of PbCl2 in a solution of 0.23 M CaCl2? Ksp = 1.6 ✕ 10-5 for PbCl2. 2. What is the Qsp when 32.0 mL of 6.50 ✕ 10-7 M Na3PO4 are mixed with 41.4 mL of 5.50 ✕ 10-5 M CaCl2? Assume the volumes are additive. Ksp = 2.0 ✕ 10-29. 3. What is the Qsp when 61.0 mL of 1.50 ✕ 10-4 M AgNO3 are mixed with 80.0 mL of 5.20 ✕ 10-3 M CaCl2? Assume the volumes are additive. Ksp = 1.6 ✕ 10-10. 4. What [I-1] is needed to start the precipitation of AgI from a saturated solution of AgCl? Ksp = 2.9 ✕ 10-16 for AgI and Ksp = 1.2 ✕ 10-10 for AgCl.
A 0.5131-g sample that contains KBr (MM: 119.0023) is dissolved in 50 mL of distilled water. Titrating with 0.04614 M AgNO3 requires 25.13 mL to reach the Mohr end point. A blank titration requires 0.65 mL to reach the same end point. Report the %w/w KBr in the sample.
If 250.0 mL of 0.0010 M Sr(NO3)2 were added to 50.0 mL of 0.0000010 M Na2CO3 would a precipitate of SrCO3 form? (Assume that all the Sr(NO3)2 and Na2CO3 have completely dissolved). The Ksp of SrCO3 is 5.60 x 10-10.