6. (a) Aspirin is a weak acid with a pKa of 3.6 and MW 180 g/mol. The saturation solubility (S) of aspirin in water is 3.3 g/L and a saturated solution has pH equal to your answer to question 4(b) above. What is the solubility of the unionisedform (So) of aspirin at this pH using units of mol/L and g/L. (b) Use the So value (just obtained) to calculate thesaturation solubility (S) of aspirin in water at pH 6.6 using units of mol/L and g/L. (c) If you modified the aspirinsuspension APF12 formula by replacing the purified water with pH 6.6 buffer, would the product be a suspension orsolution?

The objective of the question is to calculate the solubility of the unionised form of aspirin at a…

Answered: 6. (a) Aspirin is a weak acid with a…

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter79: Solubility

Section: Chapter Questions

Problem 1P

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Distinguish between the terms slightly soluble and weak. electrolyte.
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?
6. (a) Aspirin is a weak acid with a pKa of 3.6 and MW 180 g/mol. The saturation solubility (S) of aspirin in water is 3.3 g /L and a saturated solution has pH equal to your answer to question 4(b) above. What is the solubility of the unionised form (So) of aspirin at this pH using units of mol/L and g/L. (b) Use the So value (just obtained) to calculate the saturation solubility (S) of aspirin in water at pH 6.6 using units of mol/L and g/L. (c) If you modified the aspirin suspension APF12 formula by replacing the purified water with pH 6.6 buffer, would the product be a suspension or solution?
(a) If the molar solubility of YF3 at 25 °C is 4.23e-06 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 0.00100 g of BaCO3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility-product constant for BaCO3. Ksp = (c) The Ksp of ZnCO3 at 25 °C is 1.46e-10. What is the molar solubility of ZnCO3? solubility = mol/L
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The thermodynamic solubility product of AGCN is 6.0x10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.7e-9 X mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.8e-15 X mol·L-1
The thermodynamic solubility product of A9CN is 6.0×10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.75e-9 mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.81e-16 X mol·L-1
Benzoic acid, C6H5COOH, is much more soluble in NaOH(aq) than it is in pure water. Can you suggest a reason for this? of HO,
Q2) a) Explain the titration curve (variation of pH with respect to addition of titrant) with suitable diagram and reactions involved when a strong base is added as titrant to a weak acid as analyte. (b) The saline water discharged from a thermal desalination plant was analyzed and it has following composition.(i) If the discharged water sample contains 4.2 g of potassiumchloride (KCl) per 500 mL of solution, determine its molarity.(ii) The sample contains CaCl2 and its concentration was found to be 0.04M. Calculate grams of CaCl2 present in 100 mL of the sample. (c) In complexometric titration, explain why a constant pH need to be maintained during estimation of metal ions using EDTA.

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