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.
![**Problem Statement:**
Find the [H₃O⁺] of a 0.100 M HCN solution. The Ka for HCN is 4.9 × 10⁻¹⁰.
---
**Explanation:**
This problem involves calculating the hydronium ion concentration [H₃O⁺] of a hydrocyanic acid (HCN) solution using its dissociation constant (Ka).
1. **Write the dissociation equation for HCN:**
\[
\text{HCN} \leftrightarrow \text{H⁺} + \text{CN⁻}
\]
In water, H⁺ is equivalent to H₃O⁺, so the equation can be written as:
\[
\text{HCN} + \text{H₂O} \leftrightarrow \text{H₃O⁺} + \text{CN⁻}
\]
2. **Write the expression for Ka:**
\[
\text{Ka} = \frac{[\text{H₃O⁺}][\text{CN⁻}]}{[\text{HCN}]}
\]
3. **Assume initial concentrations and change:**
- Initial [HCN] = 0.100 M
- Initial [H₃O⁺] = 0
- Change: [HCN] decreases by x, [H₃O⁺] and [CN⁻] increase by x
Therefore:
- [HCN] = 0.100 - x
- [H₃O⁺] = x
- [CN⁻] = x
4. **Substitute into the Ka expression:**
\[
\text{Ka} = \frac{x \times x}{0.100 - x} = \frac{x^2}{0.100 - x}
\]
Assume x is small compared to 0.100 (since HCN is a weak acid), then:
\[
\text{Ka} \approx \frac{x^2}{0.100}
\]
5. **Solve for x:**
\[
4.9 \times 10^{-10} = \frac{x^2}{0.100}
\]
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