Determine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. c. NO₃^–

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Identify the anion in question: \( \text{NO}_3^- \).

Recall that an anion is considered basic if it can accept a proton (\( \text{H}^+ \)) from water, forming \( \text{OH}^- \).

Consider the conjugate acid of \( \text{NO}_3^- \), which is \( \text{HNO}_3 \) (nitric acid).

Recognize that \( \text{HNO}_3 \) is a strong acid, meaning it completely dissociates in water, and its conjugate base, \( \text{NO}_3^- \), is very weak and does not accept protons.

Conclude that \( \text{NO}_3^- \) is a neutral anion and does not act as a base in water.

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Acid-Base Theory

Acid-base theory explains the behavior of substances in terms of proton (H+) transfer. According to the Brønsted-Lowry theory, acids donate protons while bases accept them. Understanding this concept is crucial for determining whether an anion acts as a base or is neutral in solution.

Properties of Anions

Anions are negatively charged ions that can influence the acidity or basicity of a solution. The nature of the anion, including its size and electronegativity, affects its ability to accept protons. For example, anions derived from strong acids, like NO3-, are typically neutral and do not exhibit basic properties.

Equilibrium and Reaction Equations

In acid-base reactions, equilibrium plays a key role in determining the direction of the reaction. Writing an equation to show how an anion acts as a base involves illustrating the proton transfer process. This requires understanding how to represent chemical species and their interactions in a balanced equation.

Determine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. c. NO3–