Bronsted-Lowry Acid
Description
Two scientists came to a conclusion: an acidic solution behaves as proton donors, which is in the form of a hydrogen ion. This is what we call the Bronsted-Lowry definition of an acid, which is the main focus of this lesson.
!!!What is a Bronsted-Lowry Acid?
What makes a solution an acid? There are different definitions proposed by different scientists about what makes an acidic solution. Particularly, there were two scientists who independently proposed essentially the same theory about the definition of acids and bases.
In 1923, Johannes Nicolaus Bronsted and Thomas Martin Lowry, from Denmark and England, respectively, came up and published the same theory on how acidic and basic solutions behaved. According to Bronsted and Lowry, __acids__ are solutions that ‘’donate protons’’ and __bases__ are solutions that ‘’accept protons’’.
Johannes …show more content…
We do this by counting the hydrogen atoms for each substance in the chemical reaction. If a substance ‘’lost’’ hydrogen atoms, then this is our Bronsted-Lowry acid.
!!!Bronsted-Lowry Acid-Base Reactions
Let us go over a few Bronsted-Lowry acid-base reactions and practice identifying Bronsted-Lowry acids, as well as conjugate acids and bases.
First, let us look at the reaction between:
CH_3 COOH+H_2 O ⇌CH_3 COO^-+ H_3 O^+
Let us identify the substances. CH3COOH is the Bronsted-Lowry acid because it is the ‘’proton donor’’ – it donated its hydrogen atom to H2O. H2O is the Bronsted-Lowry base because it is the ‘’proton acceptor’’. The conjugate base is CH3COO- because it is the substance produced after the proton, hydrogen, is donated. The conjugate acid is H3O+ because this is the substance produced when H2O accepted the proton. The conjugate acid-base pairs are: CH3COOH/CH3COO- and H2O/H3O+. If we label the reaction accordingly, it will look like: Let us now look at this next reaction:
NH_3+HCl ⇌〖NH_4〗^++ 〖Cl〗^-
What happens here
Two scientists came to a conclusion: an acidic solution behaves as proton donors, which is in the form of a hydrogen ion. This is what we call the Bronsted-Lowry definition of an acid, which is the main focus of this lesson.
!!!What is a Bronsted-Lowry Acid?
What makes a solution an acid? There are different definitions proposed by different scientists about what makes an acidic solution. Particularly, there were two scientists who independently proposed essentially the same theory about the definition of acids and bases.
In 1923, Johannes Nicolaus Bronsted and Thomas Martin Lowry, from Denmark and England, respectively, came up and published the same theory on how acidic and basic solutions behaved. According to Bronsted and Lowry, __acids__ are solutions that ‘’donate protons’’ and __bases__ are solutions that ‘’accept protons’’.
Johannes …show more content…
We do this by counting the hydrogen atoms for each substance in the chemical reaction. If a substance ‘’lost’’ hydrogen atoms, then this is our Bronsted-Lowry acid.
!!!Bronsted-Lowry Acid-Base Reactions
Let us go over a few Bronsted-Lowry acid-base reactions and practice identifying Bronsted-Lowry acids, as well as conjugate acids and bases.
First, let us look at the reaction between:
CH_3 COOH+H_2 O ⇌CH_3 COO^-+ H_3 O^+
Let us identify the substances. CH3COOH is the Bronsted-Lowry acid because it is the ‘’proton donor’’ – it donated its hydrogen atom to H2O. H2O is the Bronsted-Lowry base because it is the ‘’proton acceptor’’. The conjugate base is CH3COO- because it is the substance produced after the proton, hydrogen, is donated. The conjugate acid is H3O+ because this is the substance produced when H2O accepted the proton. The conjugate acid-base pairs are: CH3COOH/CH3COO- and H2O/H3O+. If we label the reaction accordingly, it will look like: Let us now look at this next reaction:
NH_3+HCl ⇌〖NH_4〗^++ 〖Cl〗^-
What happens here