Concept explainers
Label the acid in the reactants and the conjugate acid in the products in each reaction. Use the data in Tables 9.2 and 9.3 to determine whether the reactants or products are favored at equilibrium. Explain your reasoning.
a.
b.
c.
Table 9.2 Relative Strength of Acids and Their Conjugate Bases
Table 9.3 Acid Dissociation Constants
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Chapter 9 Solutions
General, Organic, and Biological Chemistry - 4th edition
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- Consider the following acidic equilibrium: H₂CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + H₃O⁺(aq). If you add NaHCO₃ to this solution, which of the following will occur? A) The reaction quotient will decrease. B) The reaction will shift in the reverse direction. C) The equilibrium constant will increase. D) No changes to the equilibrium positions will take place.arrow_forwardCH3CH2COOH Draw the Lewis structure of the acid and mark the acidic hydrogen with an asterisk (*). Draw a Lewis structure of the conjugate base of the acid. Suppose the acid is neutralized with a strong base. a) Which of the two structures you drew in 6 and 7 would be the predominant form of the species at a pH well above that at the equivalence point? b) Which of the two structures would be the predominant form of the species at a very low pH, well below that at the equivalence point and similar to the pH near the start of the titration? c) At what point in the titration, if any, would there be equal amounts of the two forms?arrow_forward1. The odor of spoiled butter is due in part to butanoic acid (HC4H7O2) which results from the breakdown of the fat in butter. A 0.100M solution of butanoic acid is 1.23% ionized. a. Write the chemical equation for the ionization of this acid in water. b. Write the Ka expression for this acid. c. What is the equilibrium concentration of each product and the reactant?arrow_forward
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