Write the chemical equation and the Ka expression for the ionization of each of the following acids in aqueous solution. First, show the reaction with H+(aq) as a product and then with the hydronium ion: (a) HBrO2 (b) C2H5COOH.

Name: Chemistry: The Central Science
Author: Brown
ISBN: 9780137542970

Verified step by step guidance

Step 1: Identify the acid and its ionization in water. For HBrO2, the ionization reaction with H+(aq) as a product is: \[ \text{HBrO}_2 (aq) \rightleftharpoons \text{H}^+ (aq) + \text{BrO}_2^- (aq) \].

Step 2: Write the Ka expression for the ionization of HBrO2. The expression is: \[ K_a = \frac{[\text{H}^+][\text{BrO}_2^-]}{[\text{HBrO}_2]} \].

Step 3: Show the ionization of HBrO2 with the hydronium ion as a product: \[ \text{HBrO}_2 (aq) + \text{H}_2\text{O} (l) \rightleftharpoons \text{H}_3\text{O}^+ (aq) + \text{BrO}_2^- (aq) \].

Step 4: Identify the acid and its ionization in water for C2H5COOH. The ionization reaction with H+(aq) as a product is: \[ \text{C}_2\text{H}_5\text{COOH} (aq) \rightleftharpoons \text{H}^+ (aq) + \text{C}_2\text{H}_5\text{COO}^- (aq) \].

Step 5: Write the Ka expression for the ionization of C2H5COOH. The expression is: \[ K_a = \frac{[\text{H}^+][\text{C}_2\text{H}_5\text{COO}^-]}{[\text{C}_2\text{H}_5\text{COOH}]} \].

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid Ionization

Acid ionization refers to the process by which an acid donates a proton (H+) to water, resulting in the formation of its conjugate base and hydronium ions (H3O+). This process is fundamental in understanding the behavior of acids in aqueous solutions and is represented by a chemical equation that shows the reactants and products involved.

Ka Expression

The acid dissociation constant (Ka) is a quantitative measure of the strength of an acid in solution. It is defined as the ratio of the concentration of the products (the conjugate base and hydronium ion) to the concentration of the reactants (the undissociated acid) at equilibrium. The Ka expression provides insight into how readily an acid donates protons and is crucial for calculating pH and understanding acid-base equilibria.

Hydronium Ion

The hydronium ion (H3O+) is formed when an acid donates a proton to a water molecule. It is a key species in acid-base chemistry, representing the presence of acidity in a solution. Understanding the role of the hydronium ion is essential for writing accurate chemical equations and Ka expressions, as it directly relates to the ionization of acids in aqueous environments.

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