Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices: (1) Both members of a Bronsted-Lowry conjugate acid-base pair must contain the element hydrogen.
(2) The larger the value of the acid ionization constant for an acid, the weaker the acid is.
(3) Weak acids cannot completely neutralize strong bases.
A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question

Quizplus · Accepted Answer

1) False - A Bronsted-Lowry conjugate acid-base pair involves a molecule/ion donating a proton (H+) and the corresponding molecule/ion receiving that proton. The base in the pair does not need to contain hydrogen initially; it gains a hydrogen atom after accepting a proton.2) False - The larger the value of the acid ionization constant (Ka), the stronger the acid is, because it indicates a greater tendency of the acid to donate protons.3) False - Weak acids can completely neutralize strong bases, given appropriate stoichiometric ratios. The strength of an acid or base does not prevent neutralization; it only affects the equilibrium position of the reaction.

Characterize EACH of the Three Given Statements as Being TRUE