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?

Dear student acc to bartleby guidelines I can solve only first three subparts of the posted…

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?..

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.20QAP

See similar textbooks

Similar questions

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 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?
A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample. Please use the factor label method in answering.
A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample.
Calcium fluoride is considered as a relatively insoluble compound and therefore lime or slakedlime has been considered as a possible material to remove excess fluoride in water of boreholesin certain parts of the country. The solubility product of CaF2 is Ksp = 3 x 10 – 11 and that ofCa(OH)2 isKsp =8x10-61. How much lime can be added to the water to remove 10 mg of F- ion per litre ofborehole water?(The atomic masses are Ca: 40.08; F: 19.00; O: 16; H: 1)
Calculate Qsp for calcium fluoride (Ksp = 3.9 ×10–11) when 180.0 mL of a 6.05×10-3 M solution of Ca(NO3)2 is added to 260.0 mL of a 7.65×10-3 Msolution of KF.
Construct a titration curve (pCl^- vs. Vtitrant) for the titration of 25.0 mL of 0.100 M Cl^– solution with 0.100 M AgNO3. MS Excel® can be used. Titrant volumes: 0.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL.AgCl: Ksp = 1.82 x 10^-10
What is the mole ratio of sodium acetate to acetic acid (Ka=1.8 x 10^-5) in a buffer with the pH of 4.00? Report to 3 sig figs
A 0.500-g sample containing BaBr2 (FM = 297.14) is dissolved in 50 mL of distilled water. Titrating with 0.0400 M AgNO3 requires 25.00 mL to reach the Mohr endpoint. A blank titration requires 0.50 mL to reach the same endpoint. Calculate the %w/w BaBr2 in the sample. Please provide a complete solution.
A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.5072-g sample is dissolved in 50 mL of water and titrated to the Ag2CrO4 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.KCl = 74.551 NaBr = 102.89
10mL of a 10% by weight MgCl2 solution (density = 1.1 g / mL) is precipitated as magnesium ammonium phosphate after necessary processes, filtered and washed. The precipitate is dissolved in 50mL 1M HCl and excess acid is titrated with 2.0M NaOH solution in the presence of methyl orange. Find the NaOH consumption (Mg = 24,3g / mol, Cl = 35,5g / mol)
A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.2125-g sample is dissolved in 25 mL of water and titrated to the Ag2CrO4 endpoint, requiring 25.63 mL of 0.1110 M AgNO3. A blank titration requires 1.15 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample. KCl = 74.551 NaBr = 102.89