Identify the Bronsted-Lowry acid and base on the left side of the equation and the conjugate acid and conjugate base on the right side. HBRO (aq) + H20 (1) H30* (aq) + BrO` (aq) HSO,'(aq) + HC0, (aq) - so, (aq) + H2CO; (aq) HSO; (aq) + H30* (aq) H,SO3 (aq) + H,0 (1)
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-Lowry Acid-Base Reactions**
Learn how to identify Bronsted-Lowry acids and bases with the following examples. Each equation shows reactants on the left side and the products on the right side. Identify which chemical species act as acids and bases in each reaction. Remember, acids donate protons (H^+), and bases accept protons.
### Reaction 1
**Equation:**
\[ \text{HBrO (aq) + H}_2\text{O (l)} \rightleftharpoons \text{H}_3\text{O}^+ \text{(aq) + BrO}^- \text{(aq)} \]
- **HBrO (aq)**: Acts as the Bronsted-Lowry acid, donating a proton to H₂O.
- **H₂O (l)**: Acts as a Bronsted-Lowry base, accepting a proton from HBrO.
- **H₃O⁺ (aq)**: The conjugate acid formed by H₂O after gaining a proton.
- **BrO⁻ (aq)**: The conjugate base formed by HBrO after losing a proton.
### Reaction 2
**Equation:**
\[ \text{HSO}_4^- \text{(aq) + HCO}_3^- \text{(aq)} \rightleftharpoons \text{SO}_4^{2-} \text{(aq) + H}_2\text{CO}_3 \text{(aq)} \]
- **HSO₄⁻ (aq)**: Acts as the Bronsted-Lowry acid, donating a proton to HCO₃⁻.
- **HCO₃⁻ (aq)**: Acts as a Bronsted-Lowry base, accepting a proton from HSO₄⁻.
- **SO₄²⁻ (aq)**: The conjugate base formed by HSO₄⁻ after losing a proton.
- **H₂CO₃ (aq)**: The conjugate acid formed by HCO₃⁻ after gaining a proton.
### Reaction 3
**Equation:**
\[ \text{HSO}_3^- \text{(aq) + H}_3\text{O}^+ \text{(aq)} \rightleftharpoons \text{H}_2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa9e8573f-552b-4431-b931-fec80f931989%2Fcd768480-81d1-4e6d-b8e7-55a90bc53428%2F5f4igi_processed.png&w=3840&q=75)
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