9. Given the pka's indicated, determine the net charge on the molecule shown below when it is in aqueous solution at pH 2.3, 7.6 and 14. pka = 5 O pH 2.3 7.6 14 H NH₂ H net pK₂ = 11 charge H pka: = 10
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- Given that pKb for iodate ion (IO-3) is 13.83, find the quotient [HIO3]/[IO-3] in a solution of sodium iodate at (a) pH 7.00; (b) pH 1.00.What is the salt and acid concentration for 1 Molar phosphoric acid solution at pH 7.0 when pKa is 7.21? Salt is: Na2HPO4 Acid is: NaH2PO4 (antilogy of 0.21 is 1.6281)The value of Ksp for Mg3(AsO4)2 is 2.1 x 10-20. TheAsO43 - ion is derived from the weak acid H3AsO4 (pKa1 =2.22; pKa2 = 6.98; pKa3 = 11.50). (a) Calculate the molarsolubility of Mg3(AsO4)2 in water. (b) Calculate the pH of asaturated solution of Mg3(AsO4)2 in water.
- Histidine has ionizable groups with pKa values of 1.8, 6.0, and 9.2, as shown below (His 5 imidazole group). A biochemist makes up 100 mL of a 0.100 M solution of histidine at a pH of 5.40. She then adds 40 mL of 0.10 M HCl. What is the pH of the resulting solution?Using the reagents, prepare 100mL solution with a concentration of 25.0 mM Tris buffer at a final pH of 7.70. •Solid Tris, FW = 121.1• Solid Tris-C1, the conjugate acid of Tris. It has a pKa of 8.30 (at 25° C) and a FW of 157.6. •deionized waterCalculate (to the nearest 0.1%) the proportion of a dose of ebastine (pKa of conjugate acid = 10.3) that will be ionised at pH 7.7. You do not need to include "%" in your answer.
- What is the pKa of the conjugate acid of a base that has a Kb value equal to 2.1 × 10-7? Report your answer to the hundredths place. Assume the temperature is 25ºC.If the concentration of an acid in solution is 2.2 times larger than the concentration of its conjugate base, and the pH of the solution is 3.5, what is the pKa of the acid? Include the answer to 3 significant figuresI was given an excellent explanation to the following question, but I don't understand one part of the expert answer. Why is the concentration ratio the same for the calculation of pKa2? "The pKa values of a compound with two ionizable groups are pK1 =4.10 and pK2 between 7 and 10. A biochemist has 10 mL of a 1.0 M solution of this compound at a pH of 8.00. She adds 10.0 mL of1.00 M HCl, which changes the pH to 3.20. What is pK2?" I included the original answer. Thank you very much for your help.
- Why is the equilibrium between the acid NaH2PO4, and its conjugate base Na2HPO4, a suitable buffer for maintaining intracellular pH (pH 6.9-7.3)? Justify your answer using your titration curve from part A.3 Sketch a titration curve for the amino acid lysine and indicate the pKa values for all titratable groups. Also indicate the pH at which this amino acid has no net charge.Use the Goal Seek spreadsheet at the end of the chapter to find the pH of 1.00 L of solution containing 0.030 mol HA (pKa = 2.50) and 0.015 mol NaA. What would the pH be with the approximations [HA] = 0.030 and [A-] = 0.015?