Use the table below to answer the following questions:Table 1 - List of Weak AcidsAcidFormulaКаAcetic acidHC2H3O21.8x10-5Benzoic acidC6H5CO2H6.5x10:5Formic acidHCO2H1.8x10-4Hydrofluoric acidHF3.5x104Nitrous acidHNO24.5x10-4PhenolC6H5OH1.3x10-10Table 2 - List of Weak BasesBaseFormulaAmmoniaNH31.8x10-5C6H5NH24.3x10 10AnilineMethylamineCH3NH24.4x10-4Weakest acid[ Choose]Strongest acid[Choose ]Acid with lowest pH (same concentration)[Choose ]Acid with highest pH (same concentration)[Choose ]Base with lowest pH (same concentration)[Choose ]Base with highest pH (same concentration)[ Choose]

According to Bronsted Lowry concept bases accept protonH+ and acids donate protonH+. Recall the…

Answered: Use the table below to answer the…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 85AP

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Classify each of the following statements as true or false: aAll Brnsted-Lowry acids are Arrhenius acids. bAll Arrhenius bases are Brnsted-Lowry bases, but not all Brnsted-Lowry bases are Arrhenius bases. c HCO3 is capable of being amphoteric. d HS is the conjugate base of S2. eIf the species on the right side of an ionization equilibrium are present in greater abundance than those on the left, the equilibrium is favored in the forward direction. f NH4+ cannot act as a Lewis base. gWeak bases have a weak attraction for protons. hThe stronger acid and the stronger base are always on the same side of a proton transfer reaction equation. iA proton transfer reaction is always favored in the direction that yields the stronger acid. jA solution with pH=9 is more acidic than one with pH=4. kA solution with pH=3 is twice as acidic as one with pH=6. lA pOH of 4.65 expresses the hydroxide ion concentration of a solution in three significant figures.
Each box represents an acid solution at equilibrium. Squares represent H+ ions, and circles represent the anion. Water molecules are not shown. Which figure represents a strong acid? Which figure is a weak acid?
. The following figures are molecular-level representations of acid solutions. Label each as a strong acid or a weak acid.
Write equations to illustrate the acid-base reaction when each of the following pairs of Brnsted acids and bases are combined: Acid Base a.HOCl H2O b.HClO4 NH3 c.H2O NH2 d.H2O OCl e.HC2O4 H2O
. Write a chemical equation showing how each of the following species can behave as indicated when dissolved in water. a. HSO3as an acid b. CO32as a base c. H2PO4as an acid d. C2H3O2as a base
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.

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