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- Molecule A is C6H9O2F and an aqueous solution of 0.0130 M of molecule A has a pH of 1.0 . Calculate the pKa. Use at least 2 sig figs and no scientific notation.What is the conjugate acid of HBO32-Consider the following compounds that vary from nearly nonacidic to strongly acidic. Draw the conjugate bases of these compounds, and explain why the acidity increases so dramatically with substitution by nitro groups.CH4 CH3NO2 CH2(NO2)2 CH(NO2)3 pKa ≅ 50 pKa = 10.2 pKa = 3.6 pKa = 0.17
- To what final concentration of NH3 must a solution be adjusted to just dissolve 0.035 mol of NiC2O4 (Ksp = 4×10−10) in 1.0 L of solution? (Hint: You can neglect the hydrolysis of C2O42− because the solution will be quite basic.) Express your answer using one significant figure.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.15.What would be the pH of a 0.25 M solutionof phenylamine (C6H5NH2) at room temperature? The Kb of phenylamine is 4 × 10^−10. 1. 132. 10.5 3. 94. 15. 5
- Dicarboxylic acids have two dissociation constants, one for the initial dissociation into a monoanion and one for the second dissociation into a dianion. For oxalic acid, HO2C—CO2H, the first ionization constant is pKal = 1.2 and the second ionization constant is pKa2 = 4.2. Why is the second carboxyl group far less acidic than the first?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 figuresBecause phenol (C6H5OH) is less acidic than a carboxylic acid, it can be deprotonated by NaOH but not by the weaker base NaHCO3. Using this information, write out an extraction sequence that can be used to separate C6H5OH, benzoic acid, and cyclohexanol. Show what compound is present in each layer at each stage of the process, and if it is present in its neutral or ionic form.
- The pKa values of the conjugate acids of 2-aminopyridine (6.71) and 4- aminopyridine (9.11) are as shown. Which nitrogen is the more basic in these structures and why?Calculate the [H3O+] of 3.0M H3PO4 solution, given the acid dissociation constant for H3PO4:Ka1 = 7.2x10−3 Ka2 = 6.3x10−8 Ka3 = 4.2x10−131b) Suppose you decreased the pH of the biotin solution from 7.0 to 3.0 - what would happen to the ionizable group on a molecule of biotin as the pH shifted from 7.0 to 3.0? Briefly explain why you would expect that to happen