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- State the fact below ? An acid can be deprotonated by the conjugate base of any acid havinga higher pKa.How did you know the molecules were weak or strong acid? Please give the pKa if that's the method you used. Please explain in detail.Consider a diprotic acid with pKa values of 1.60 and 4.50, that is colorless when fully protonated, deep blue when singly deprotonated, and bright red when doubly deprotonated. Assuming that both colored forms have large and approximately equal molar absorptivities, what can be inferred from a solution of the compound that has a faint blue color?
- The pKa of the conjugate acid of guanidine is 13.6, making it one of thestrongest neutral organic bases. Offer an explanation.At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated as H2M,H2M, HM−,HM−, and M2−,M2−, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively.A solution was prepared at 25°C in which the ratio of methylamine (CH3NH2) to the salt methylammonium chloride (CH3NH3Cl) was two to one, and resulted in a pH = 11.00. Calculate Ka for the weak acid methylammonium (CH3NH3+) at 25°C.
- The Kb of carbonate is 1.8×10−4. Calculate the Ka of its conjugate acid.A 0.119 M solution of Covidenol, a weak acid, has a measured pH of 3.45. Determine the pKa of Covidenol.To what category of basicity does CrO42- belong? Select one: a. strongly or very strongly basic b. feebly basic c. nonbasic d. moderately basic e. weakly basic
- Look up the theoretical value for the Ka of CH3COOH to calculate what the pH should have been for the 5% CH3COOH.LiF has a pKsp of 2.77. HF has a pKa of 3.17. LiF is dissolved at 0.250 F after addition of strong acid. What is the pH of the 0.250 F LiF solution?What is the FORMULA and NAME of the conjugate acid of bisulfite ion?