Are all Bronsted-Lowry acids and bases Lewis acids and bases? Please discuss.
Yes, they are. Bronsted-Lowry acids are proton donors that can be thought of as electron pair acceptors because the H+ is transferred to the electron pair on a base. Bronsted-Lowry bases are proton acceptors. In order to accept a proton, the base must donate an electron pair to the proton, so Bronsted-Lowry bases are also Lewis bases. It is important to note that the converse is not true--all Lewis acids and bases are not Bronsted-Lowry acids and bases.
What is the [H+] of a solution prepared by the dissolution of 26.0 g HF (g) in 1.00 L of water? The Ka of HF is 6.6 x 10-4.
Note the use of the equilibrium constant to solve the problem and the assumption that the amount of dissociation for weak acids is quite small. That assumption is only valid for a weak acid in a solution where the weak acid concentration is much larger than the value of x. If x is greater than 5% of the initial concentration of the acid, then you must solve the quadratic equation because the assumption becomes invalid.
Given that the Kb of NH3 is 1.8 x 10- 5, calculate the Ka of the ammonium ion, NH4.
Note the important relationships between Kw, Ka, and Kb necessary for solving this problem.