Multiple Choice
The equilibrium constant for the reaction below has the value Ka = 3.5 x 10^-4. In this reaction, the stronger Brønsted-Lowry acid is ________ and the weaker Brønsted-Lowry acid is ________. HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq)
17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What is the formula for the conjugate acid of the Brønsted-Lowry base CH3NH2?
A
CH3NH-
B
CH3NH2+
C
CH3NH3-
D
CH3NH3+
Verified step by step guidance1
Identify the Brønsted-Lowry base in the problem, which is CH3NH2. A Brønsted-Lowry base is a substance that can accept a proton (H+).
To find the conjugate acid of a base, add a proton (H+) to the base. This is because a conjugate acid is formed when a base gains a proton.
Add a proton (H+) to the base CH3NH2. This involves adding an H+ ion to the nitrogen atom, which is the site of protonation in amines.
The addition of a proton to CH3NH2 results in the formation of CH3NH3+. This is because the nitrogen atom in CH3NH2 accepts the proton, forming a positively charged ion.
Verify the charge and structure: The original base CH3NH2 is neutral, and by adding a proton (H+), the resulting conjugate acid CH3NH3+ carries a positive charge, which is consistent with the formation of a conjugate acid.
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