Question 29 Suppose that a distribution constant for an amine, B, is Kp = 4.50 and the acid dissociation constant of BH* is Ka=1.90 x 109. If 5.00x10¹ L of 5.10x101 M aqueous amine is extracted with 1.50x101 L of solvent, what will be the formal concentration remaining in the aqueous phase a) at pH 10.50? and b) at pH 4.00?
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- I 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.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.Give typed solution A compound has two carboxyls and one aminium group. The pKas of the groups are 2.1, 4.5, and 9.1, respectively. A biochemist has 100 mL of a 0.10 M solution of this compound at a pH of 5.2. She adds 29 mL of 0.1 M NaOH. To the nearest hundredth of a unit, what will be the pH of the solution after addition of the NaOH? (Assume full stirring to reach a new equilibrium.) (ANSWER IS 8.25, BUT UNSURE HOW TO GET THERE)
- If a water has a carbonate alkalinity of 120.00 mg/L as the ion and a pH of 10.30, what is the bicarbonate alkalinity in mg/L as the ion? The answer is HCO_3=130.686 or 130.7 mg/LPlease do explain the stepsWhat is the pH of 500mL of a buffer solution of HC3H5O3 0.0570M and C3H5O3Na 0.0275M? Ka of HC3H5O3 = 1.9x10^-5Question: calculate the pH of 50.0 mL H20 + 1.00 mL 0.6 M NaOH (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00
- ANSWER NUMBER FOUR ONLY A study of vaccines suggest that a higher pH, preferably near 7, is necessary for the faster formation of the antibodies. Because of this, a chemist proposed using a citric acid buffer. They were tasked to prepare a 500.0 mL, 0.25 M pH 5.00 buffer from 1.20M citric acid (H3C6H5O7; pKa1 = 3.13, pKa2 = 4.76, pKa3 = 6.40) and 0.90 M NaOH. Note: When adding a strong acid/base to a weak base/acid, the strong acid/base is fully consumed. What is the acid component and base component of the buffer solution? What are the moles of each component in the buffer solution? Calculate the amounts of reagents needed to prepare the buffer solution. What will be the pH of the buffer upon addition of 0.75 mL 2.00 M HNO3? What will be the pH of the buffer upon addition of 2.30 mL of 1.75 M NaOH?A 0.022 2 M solution of HA is 0.15% dissociated. Calculate pKa for this acid.2. The Ph of 0.40M solution of hypobromous acid [HOBr] is5.05. Calculate ka and % dissacosiation
- The normal pH of blood is 7.40± 0.05 and is controlled inpart by the H₂CO₃/HCO₃⁻ buffer system.(a) Assuming that the Kₐ value for carbonic acid at 25°C applies to blood, what is the [H₂CO₃]/[HCO₃⁻] ratio in normal blood?(b) In a condition called acidosis, the blood is too acidic. What is the [H₂CO₃]/[HCO₃⁻] ratio in a patient whose blood pH is 7.20?A physician wishes to prepare a buffer solution at pH = 3.82 that efficiently resists changes in pH yet contains only small concentrations of the buffering agents. Determine which one of the following weak acids, together with its sodium salt, would probably be best to use: m-chlorobenzoic acid, Ka= 1.04 × 10-4 ; p-chlorocinnamic acid, Ka=3.89 × 10-5 ; 2,5-dihydroxybenzoic acid, Ka = 1.08 ×10-3 ; or acetoacetic acid, Ka= 2.62 × 10-4 . Explain.2) Given silver oxalate (Ag2C2O4 KSP = 5.40 x10-12) and silver phosphate (Ag3PO4 KSP = 8.89 x10-17) whichsubstance has a greater concentration of the Ag+ ion?