Question

A Brønsted-Lowry acid Question 9 options: A) has a lower pH than vinegar. B) is any species that donates a proton. C) is any species that accepts a proton. D) is limited to aqueous solutions.

Answer 1

B) is any species that donates a proton.

Answer 2

A Brønsted-Lowry acid is any substance (molecule or ion) that can donate a hydrogen ion (H+).

A Brønsted-Lowry base is any species that can accept a hydrogen ion (H+).

Explanation:

In short, acids have the ability to donate protons and bases have the ability to accept protons.

Take the following reaction for example:

H2SO4+NH3⇌NH+4+HSO−4

Sulfuric acid (H2SO4) is the Brønsted-Lowry acid because it donates a hydrogen ion. Ammonia (NH3) is the Brønsted-Lowry base because it accepts the hydrogen ion.

The Brønsted-Lowry theory also introduces the concept of conjugate acid-base pairs. A conjugate acid-base pair are two species that differ by a (H+) ion.

Based on the reaction above, the ammonium ion

(NH+4) is the conjugate acid of the base ammonia and the hydrogen sulfate ion (HSO−4) is the conjugate base of sulfuric acid.

Here's a tip to let you know which substance is the conjugate acid and which substance is the conjugate base:

A conjugate base has one less (H+) proton than the acid you started with.

A conjugate acid has one more (H+) proton than the base you started with.

So option c is correct

Is any spcies that denotes a proton

Step-by-step explanation: