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1.8.2. Bronsted-Lowry Acids and Bases

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    In 1923, chemists Johannes Nicolaus Brønsted and Thomas Martin Lowry independently developed definitions of acids and bases based on the compounds' abilities to either donate or accept protons (\(H^+\) ions). In this theory, acids are defined as proton donors; whereas bases are defined as proton acceptors. A compound that acts as both a Brønsted-Lowry acid and base together is called amphoteric.

    The Brønsted-Lowry Theory of Acids and Bases

    Brønsted-Lowry theory of acid and bases took the Arrhenius definition one step further, as a substance no longer needed to be composed of hydrogen (H+) or hydroxide (OH-) ions in order to be classified as an acid or base. For example , consider the following chemical equation:

    \[ HCl \; (aq) + NH_3 \; (aq) \rightarrow NH_4^+ \; (aq) + Cl^- \; (aq) \]

    Here, hydrochloric acid (HCl) "donates" a proton (H+) to ammonia (NH3) which "accepts" it , forming a positively charged ammonium ion (NH4+) and a negatively charged chloride ion (Cl-). Therefore, HCl is a Brønsted-Lowry acid (donates a proton) while the ammonia is a Brønsted-Lowry base (accepts a proton). Also, Cl- is called the conjugate base of the acid HCl and NH4+ is called the conjugate acid of the base NH3.

    • A Brønsted-Lowry acid is a proton (hydrogen ion) donor.
    • A Brønsted-Lowry base is a proton (hydrogen ion) acceptor.

    In this theory, an acid is a substance that can release a proton (like in the Arrhenius theory) and a base is a substance that can accept a proton. A basic salt, such as Na+F-, generates OH- ions in water by taking protons from water itself (to make HF):

    \[F^-_{(aq)} + H_2O_{(l)} \rightleftharpoons HF_{(aq)} + OH^-\]

    When a Brønsted acid dissociates, it increases the concentration of hydrogen ions in the solution, \([H^+]\); conversely, Brønsted bases dissociate by taking a proton from the solvent (water) to generate \([OH^-]\).

    • Acid dissociation

    \[HA_{(aq)} \rightleftharpoons A^-_{(aq)} + H^+_{(aq)}\]

    • Acid Ionization Constant:


    • Base dissociation:

    \[B_{(aq)} + H_2O_{(l)} \rightleftharpoons HB^+_{(aq)} + OH^-_{(aq)}\]

    • Base Ionization Constant

    \[K_b = \dfrac{[HB^+][OH^-]}{[B]}\]

    The determination of a substance as a Brønsted-Lowery acid or base can only be done by observing the reaction. In the case of the HOH it is a base in the first case and an acid in the second case.


    To determine whether a substance is an acid or a base, count the hydrogens on each substance before and after the reaction. If the number of hydrogens has decreased that substance is the acid (donates hydrogen ions). If the number of hydrogens has increased that substance is the base (accepts hydrogen ions). These definitions are normally applied to the reactants on the left. If the reaction is viewed in reverse a new acid and base can be identified. The substances on the right side of the equation are called conjugate acid and conjugate base compared to those on the left. Also note that the original acid turns in the conjugate base after the reaction is over.


    Acids are Proton Donors and Bases are Proton Acceptors

    For a reaction to be in equilibrium a transfer of electrons needs to occur. The acid will give an electron away and the base will receive the electron. Acids and Bases that work together in this fashion are called a conjugate pair made up of conjugate acids and conjugate bases.

    \[ HA + Z \rightleftharpoons A^- + HZ^+ \]

    A stands for an Acidic compound and Z stands for a Basic compound

    • A Donates H to form HZ+.
    • Z Accepts H from A which forms HZ+
    • A- becomes conjugate base of HA and in the reverse reaction it accepts a H from HZ to recreate HA in order to remain in equilibrium
    • HZ+ becomes a conjugate acid of Z and in the reverse reaction it donates a H to A- recreating Z in order to remain in equilibrium


    1. Why is \(HA\) an Acid?
    2. Why is \(Z^-\) a Base?
    3. How can A- be a base when HA was and Acid?
    4. How can HZ+ be an acid when Z used to be a Base?
    5. Now that we understand the concept, let's look at an an example with actual compounds! \[ HCl + H_2O \rightleftharpoons H_3O^+ + Cl^¯ \]
    • HCL is the acid because it is donating a proton to H2O
    • H2O is the base because H2O is accepting a proton from HCL
    • H3O+ is the conjugate acid because it is donating an acid to CL turn into it's conjugate acid H2O
    • Cl¯ is the conjugate base because it accepts an H from H3O to return to it's conjugate acid HCl

    How can H2O be a base? I thought it was neutral?


    1. It has a proton that can be transferred
    2. It receives a proton from HA
    3. A- is a conjugate base because it is in need of a H in order to remain in equilibrium and return to HA
    4. HZ+ is a conjugate acid because it needs to donate or give away its proton in order to return to it's previous state of Z
    5. In the Brønsted-Lowry Theory what makes a compound an element or a base is whether or not it donates or accepts protons. If the H2O was in a different problem and was instead donating an H rather than accepting an H it would be an acid!

    Contributors and Attributions

    • Sarah Rundle (UCD), Charles Ophardt, Professor Emeritus, Elmhurst College; Virtual Chembook

    Additional Resources

    Michigan State Virtual Textbook of Organic Chemistry

    Brønsted Acids and Bases


    Carey 4th Edition On-Line Activity

    Khan Academy


    Balancing Acid/Base Reactions

    Cliffs Notes

    Brønsted-Lowry Acids and Bases

    1.8.2. Bronsted-Lowry Acids and Bases is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts.

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