a. 0.180 M sodium chloroacetate (Ka (CICH₂COOH) = 1.36 × 10 °)? [H₂O+]-[ = M -3 b. 3.90 × 10-³ M aniline hydrochloride (Kü (C6H5NH₂) = 3.98 × 10−¹⁰ )? [H₂O+] =[ c. 0.210 M HIO3 (K₁ (HIO3) = 0.17)? [H₂O+]=[ M M
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.
![### Acidity and Basicity of Solutions
1. **Sodium Chloroacetate Solution**
- **Concentration:** \(0.180 \, \text{M}\)
- **Acid Dissociation Constant (\(K_a\))** of Chloroacetic Acid (\(\text{CICH}_2\text{COOH}\)): \(1.36 \times 10^{-3}\)
- **Hydronium Ion Concentration \([\text{H}_3\text{O}^+]\):** \( \boxed{\,}\) M
2. **Aniline Hydrochloride Solution**
- **Concentration:** \(3.90 \times 10^{-3} \, \text{M}\)
- **Base Dissociation Constant (\(K_b\))** of Aniline (\(\text{C}_6\text{H}_5\text{NH}_2\)): \(3.98 \times 10^{-10}\)
- **Hydronium Ion Concentration \([\text{H}_3\text{O}^+]\):** \( \boxed{\,}\) M
3. **Iodic Acid Solution**
- **Concentration:** \(0.210 \, \text{M}\)
- **Acid Dissociation Constant (\(K_a\))** of Iodic Acid (\(\text{HIO}_3\)): \(0.17\)
- **Hydronium Ion Concentration \([\text{H}_3\text{O}^+]\):** \( \boxed{\,}\) M
### Explanation
This section provides exercises for calculating the hydronium ion concentration \([\text{H}_3\text{O}^+]\) in solutions of varying strengths and chemical properties. Understanding such calculations is crucial in determining the acidity or basicity of a solution.
- **Part (a)** deals with a weak acid salt (sodium chloroacetate) whose \([\text{H}_3\text{O}^+]\) is determined by its \(K_a\).
- **Part (b)** requires converting a weak base constant (\(K_b\)) into its corresponding acid constant to find \([\text{H}_3\text{O}^+]\).
- **Part (c)** involves a strong acid (\(K_a\)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F68a9b3d6-216d-4727-afb3-4b2a53419445%2Fd63780c4-64a9-4d8a-a6db-956599dcc803%2Fezvtsyd_processed.png&w=3840&q=75)
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