Answer questions a-c about the Bronsted acid-base reaction below using the identifying letters A-D below each structure. The pka's for the acids of interest are: acetic acid (pka = 4.8), and hydrogen bromide (pka = -9). CH₂- OH A acetic acid Br B bromide + H-Br 12 C acetate CH₂- D hydrogen bromide a) The stronger base is b) Its conjugate acid is c) The species that predominate at equilibrium are (two letters, e.g. ac)
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![**Bronsted Acid-Base Reaction Analysis**
In this educational exercise, analyze the Bronsted acid-base reaction using the identifying letters A-D below each molecular structure. The pKa values for the acids of interest are given as follows:
- Acetic acid (\( \text{pKa} = 4.8 \))
- Hydrogen bromide (\( \text{pKa} = -9 \))
**Structures:**
- **A. Acetic acid:** \( \text{CH}_3\text{COOH} \)
- **B. Bromide:** \( \text{Br}^- \)
- **C. Acetate:** \( \text{CH}_3\text{COO}^- \)
- **D. Hydrogen bromide:** \( \text{HBr} \)
**Reaction Equation:**
\[ \text{A (acetic acid)} + \text{B (bromide)} \rightleftharpoons \text{C (acetate)} + \text{D (hydrogen bromide)} \]
**Questions:**
a) **The stronger base** is: [Answer box]
b) **Its conjugate acid** is: [Answer box]
c) **The species that predominate at equilibrium** are: (two letters, e.g., ac) [Answer box]
The above questions help in understanding the nature of the reactants and products in terms of acid-base chemistry and their equilibrium states.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe6799157-c37b-4be1-addf-af520cc69330%2F92b168c0-5d06-459a-9541-fbb104cb3ada%2Fotcmq8l_processed.jpeg&w=3840&q=75)
The negative base-10 logarithm of a solution's acid dissociation constant (Ka) is pKa.
pKa = -log10Ka
The stronger the acid, the lower the pKa value. Acetic acid, for example, has a pKa of 4.8, and hydrogen bromide has -9
Now -9 is the smaller value, so, HBr is a strong acid.
Step by step
Solved in 3 steps with 1 images
