Textbook Question
Calculate [OH-] and pH for each of the following strong base solutions: (c) 10.0 mL of 0.0105 M Ca(OH)2 diluted to 500.0 mL
Ch.16 - Acid-Base Equilibria
Chapter 16, Problem 49
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.
Verified step by step guidance1
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.
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Calculating Percent Ionization of Weak Acids
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.
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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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Related Practice
Textbook Question
Calculate the concentration of an aqueous solution of Ca1OH22 that has a pH of 10.05.
Textbook Question
Write the chemical equation and the Ka expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H+(a)q as a product and then with the hydronium ion: (a) C6H5COOH (b) HCO3-
Textbook Question
Phenylacetic acid 1C6H5CH2COOH2 is one of the substances that accumulates in the blood of people with phenylketonuria, an inherited disorder that can cause mental retardation or even death. A 0.085 M solution of C6H5CH2COOH has a pH of 2.68. Calculate the Ka value for this acid.