# 10.3: Water - Both an Acid and a Base

Learning Objectives

• To write chemical equations for water acting as an acid and as a base.

Water (H2O) is an interesting compound in many respects. Here, we will consider its ability to behave as an acid or a base.

In some circumstances, a water molecule will accept a proton and thus act as a Brønsted-Lowry base. We saw an example in the dissolving of HCl in H2O:

$\rm{HCl + H_2O_{(ℓ)} \rightarrow H_3O^+_{(aq)} + Cl^−_{(aq)}} \label{Eq1}$

In other circumstances, a water molecule can donate a proton and thus act as a Brønsted-Lowry acid. For example, in the presence of the amide ion (see Example 4 in Section 10.2), a water molecule donates a proton, making ammonia as a product:

$H_2O_{(ℓ)} + NH^−_{2(aq)} \rightarrow OH^−_{(aq)} + NH_{3(aq)} \label{Eq2}$

In this case, NH2 is a Brønsted-Lowry base (the proton acceptor).

So, depending on the circumstances, H2O can act as either a Brønsted-Lowry acid or a Brønsted-Lowry base. Water is not the only substance that can react as an acid in some cases or a base in others, but it is certainly the most common example—and the most important one. A substance that can either donate or accept a proton, depending on the circumstances, is called an amphiprotic compound.

A water molecule can act as an acid or a base even in a sample of pure water. About 6 in every 100 million (6 in 108) water molecules undergo the following reaction:

$H_2O_{(ℓ)} + H_2O_{(ℓ)} \rightarrow H_3O^+_{(aq)} + OH^−_{(aq)} \label{Eq3}$

This process is called the autoionization of water (Figure $$\PageIndex{1}$$) and occurs in every sample of water, whether it is pure or part of a solution. Autoionization occurs to some extent in any amphiprotic liquid. (For comparison, liquid ammonia undergoes autoionization as well, but only about 1 molecule in a million billion (1 in 1015) reacts with another ammonia molecule.) Figure $$\PageIndex{1}$$ Autoionization. A small fraction of water molecules—approximately 6 in 100 million—ionize spontaneously into hydronium ions and hydroxide ions. This picture necessarily overrepresents the amount of autoionization that really occurs in pure water.

Example $$\PageIndex{1}$$

Identify water as either a Brønsted-Lowry acid or a Brønsted-Lowry base.

1. H2O(ℓ) + NO2(aq) → HNO2(aq) + OH(aq)
2. HC2H3O2(aq) + H2O(ℓ) → H3O+(aq) + C2H3O2(aq)

SOLUTION

1. In this reaction, the water molecule donates a proton to the NO2 ion, making OH(aq). As the proton donor, H2O acts as a Brønsted-Lowry acid.
2. In this reaction, the water molecule accepts a proton from HC2H3O2, becoming H3O+(aq). As the proton acceptor, H2O is a Brønsted-Lowry base.

Exercise $$\PageIndex{2}$$

Identify water as either a Brønsted-Lowry acid or a Brønsted-Lowry base.

1. HCOOH(aq) + H2O(ℓ) → H3O+(aq) + HCOO(aq)
2. H2O(ℓ) + PO43−(aq) → OH(aq) + HPO42−(aq)

## Concept Review Exercises

1. Explain how water can act as an acid.
2. Explain how water can act as a base.