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?

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?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

please see attached
Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HNO2 (aq) + OH" (aq)NO, (aq) + H2O (1) K =
The solubility of salts that contain the conjugates of weak acids increase in acidic solution. Given the reaction of CUCN (Ksp = 3.47 x 10-20) with an acid in the form H3O+ shown below, find the equilibrium constant for this reaction given that Ka HCN = 4.9 x 10-10. CUCN(s) + H:O*(aq) = Cu"(aq) + HCN(aq) + H2O(1)
6. (I) HCOj(aq)+ H2O(0) = co(ag)+H3O*(g) (II) HCO3(aq) + H₂O(1) H₂CO3(aq) +OH(aq) In which of the following reactions, H₂O acts as an acid? (III) HPO (aq) + H₂O(l) H₂PO4 (aq) + OH¯(aq) PO (aq)+ H3O*(aq) (IV) HPO (aq) + H₂O(l) (A) I and II (B) None (C) II and III (D) I and IV (E) III and IV
The molar solubility of zinc carbonate in a water solution is M.
Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NH3 (aq) + H2O(1) =NH,* (aq) + OH(aq) K=-
Complete the following solubility constant expression for Ag2CrO4. Ksp = ☐ == ✗
What is the molar solubility (in mols/L)of silver chloride in 2.00 M NH3(aq) given that Ksp of AgCl = 1.77x10-10 and Kf of Ag(NH3)2* is 1.70x107? Express your answer in decimal notation rounded to three significant figures.
g.135.
A1) Estimate the solubility of CaF2(aq) [in units of MICROmolar] in the presence of 0.156 molar CaCl2(aq). A2) Estimate the solubility of CaF2(aq) [in units of PICOmolar] in the presence of 0.831 molar AlF3(aq). [This is a bit fictitious - I don't think aluminum fluoride is soluble, but I want you to think carefully about the fluoride concentration.]
Calculate the solubility of CaSO4 (in g·L-1) in the following media. The solubility product of CaSO4 is 4.9×10-5. Assume ideal behavi (a) water I-7.6 (b) a 7.8x10-5 M SrSO4 solution g•L-1
Consider the table of equilibrium constant values given below for a given set of conditions. What will be the concentration of [HCO3-] in water that is in equilibrium with both CaCO3 (s) and 225 ppm CO2 (g) under these conditions? Equation Type Value CO2 (g) H2CO3 (aq) KH 1.7 x 102 H2CO3 (aq)=HCO3(aq) + H (aq) Kat 6.44 x 107 HCO3 (aq) CO32 (aq) + H* (aq) Ka2 8.43 x 10-11 CaCO3 (s) Ca2+ (aq) + CO2 (aq) Ksp 8.4 x 10-9 H₂O (1) H(aq) + OH (aq) Kw 7.6 x 10-14 O 1.6 x 103 M O 8.1 x 10-3 M O 5.6 x 104 M O 3.9 x 104 M O 7.9 x 104 M