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.
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The calculation doesn't match the multiple-choice. is there a step that was missed?
![### Calculating the Solubility Product Constant (Ksp) of PbBr₂
The molar solubility of PbBr₂ is given as 2.17 x 10⁻³ M at a certain temperature. Given this information, you are required to calculate the Ksp for PbBr₂. Below are multiple-choice options you can choose from:
1. 6.4 x 10⁻⁶
2. 3.4 x 10⁻⁶
3. 3.4 x 10⁻⁷
4. 6.4 x 10⁻⁷
To solve this, you can follow these steps:
1. **Write the Dissociation Equation**:
\[ \text{PbBr}_2 (s) \leftrightarrow \text{Pb}^{2+} (aq) + 2\text{Br}^- (aq) \]
2. **Express the Solubility Product Constant (Ksp)**:
\[ K_{sp} = [\text{Pb}^{2+}][\text{Br}^-]^2 \]
3. **Determine the Ionic Concentrations**:
- Given: \[ \text{Solubility of PbBr}_2 = 2.17 \times 10^{-3} \text{ M} \]
- Therefore:
\[ [\text{Pb}^{2+}] = 2.17 \times 10^{-3} \text{ M} \]
\[ [\text{Br}^-] = 2 \times 2.17 \times 10^{-3} \text{ M} = 4.34 \times 10^{-3} \text{ M} \]
4. **Plug the Values into the Ksp Expression**:
\[ K_{sp} = [2.17 \times 10^{-3}][4.34 \times 10^{-3}]^2 \]
\[ K_{sp} = (2.17 \times 10^{-3})(4.34 \times 10^{-3})^2 \]
\[ K_{sp} = (2.17 \times 10^{-3})(1.88 \times 10^{-5}) \]
\[ K_{sp} \approx 4.08 \times 10^{-8](https://content.bartleby.com/qna-images/question/f3c22a28-8e9a-42a1-ac26-114f2e495bee/1c9eb53f-3962-4a61-b9e2-1ed11935e6b0/67b0kxq_processed.png)
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