Chapter 17: Problem 106
Cacodylic acid is
Short Answer
Expert verified
(a) pH = 3.10
(b) Calculate pH using conjugate base concentration.
(c) Combine solutions and apply Henderson-Hasselbalch.
Step by step solution
01
Understand the Acid Dissociation in Part (a)
Cacodylic acid dissociates as . We have the initial concentration of the acid as . Let's consider and make an ICE table to find .
02
Set Up ICE Table for Cacodylic Acid
Initial: Change: Equilibrium: \.
03
Calculate Using Ionization Constant
The ionization constant . Using the equilibrium values, . Assuming , .
04
Solve for in Part (a)
Solve the equation . Thus, and .
05
Calculate the pH for Part (a)
06
Determine Concentration for Part (b)
07
Calculate pH for Part (b)
Since is a salt of a weak acid and strong base, it hydrolyzes to form and , followed by . Calculate .
08
Mix Both Solutions for Part (c)
Total moles of from part (a) and total moles of from (b) are determined. Then, find new concentrations in the combined solution volume.
09
Calculate pH of Final Mixture
Using concentrations from step above, apply Henderson-Hasselbalch equation: \(\text{pH} = \text{pK}_a + \log\left(\frac{[\mathrm{A}^{-}]}{[\mathrm{HA}]\right)\). Calculate .
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Ionization Constant
The ionization constant, or acid dissociation constant ( ), is a measure of the strength of an acid in solution. It provides insight into how well an acid molecule sheds its hydrogen ions, , in a given reaction. A higher value suggests a stronger acid that ionizes more completely in solution.
In the exercise involving cacodylic acid ( ), the ionization constant is given as . This implies that it is a weak acid since the value is far less than 1. is used in equilibrium calculations to determine , essential for later calculations. By setting up an equilibrium concentration expression, this small can be used to find the rate at which the acid dissociates into its ions. This is crucial for predicting and calculating solution behaviors like acidity.
In the exercise involving cacodylic acid (
Acid Dissociation
Acid dissociation refers to the process by which an acid reacts with water to release hydrogen ions ( ) into the solution, forming its conjugate base. As seen in the example of cacodylic acid, .
Every acid dissociation involves an equilibrium between the non-dissociated acid molecule and the ions produced. The initial concentration of the acid, changes due to dissociation, and equilibrium concentrations can be calculated using an ICE table (Initial, Change, Equilibrium).
levels.
Every acid dissociation involves an equilibrium between the non-dissociated acid molecule and the ions produced. The initial concentration of the acid, changes due to dissociation, and equilibrium concentrations can be calculated using an ICE table (Initial, Change, Equilibrium).
- Initial: Start with the full concentration set as the acid form, for example,
and zero for products. - Change: As dissociation occurs, the concentration of
decreases by , and and increase by . - Equilibrium: Calculate new concentrations using these changes, which allows for solving
, equating needed for .
pH Calculation
The of a solution signals its acidity or basicity, mathematically defined as . For weak acids such as cacodylic acid, once is calculated from the expression, can be directly derived from its concentration.
For example, using , . This value is typical for weak acids, indicating a slightly acidic solution.
In addition, for basic solutions such as in the presence of a salt of a weak acid, calculate the instead, followed by using and . Such calculations are foundational for students to master the manipulation of logarithmic expressions essential in chemistry.
For example, using
In addition, for basic solutions such as in the presence of a salt of a weak acid, calculate the
Henderson-Hasselbalch Equation
The Henderson-Hasselbalch Equation is a pivotal tool in buffer solutions, formulated as: This formula directly links an acid's with the ratio of its conjugate base ( ) to the acid ( ) concentrations.
In the final exercise part where two solutions combine, creating a buffer, the Henderson-Hasselbalch equation becomes crucial. It bypasses more complex calculations to swiftly ascertain the final of a buffer solution. Here, knowing both initial concentrations and total solution volumes enables rapid calculation through this log-based equation.
In the final exercise part where two solutions combine, creating a buffer, the Henderson-Hasselbalch equation becomes crucial. It bypasses more complex calculations to swiftly ascertain the final
-
is determined from as . - Calculate the molar concentrations of
and in the new mixed solution volume. - Insert these values into the equation to find the resulting
.