Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
Why is it that the Bronsted Acid equation for hcl consists of a single error and a bronsted base consists of equilibrium errors?
Accepted Answer
The Brønsted-Lowry definition of acids and bases does not involve 'equilibrium errors' for either. Acids are proton (H+) donors, and bases are proton acceptors. HCl, a strong acid, dissociates completely in water, meaning it
always
donates its proton. Therefore, there's no equilibrium to speak of in terms of proton donation. Likewise, bases like ammonia (NH3) can accept protons in an equilibrium reaction, but the term 'equilibrium errors' doesn't apply to the Brønsted-Lowry definition.
Articles you might like