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.
![### Calculating pH from Hydrogen Ion Concentration
Understanding the pH scale and how to calculate the pH of a solution given its hydrogen ion concentration, [H⁺], is fundamental in chemistry. Here we have several problems where you will need to calculate the pH from given hydrogen ion concentrations.
#### Problems:
1. **[H⁺] = 10⁻⁹.³ moles/L; pH = ?**
2. **[H⁺] = 10⁻¹³.²³ moles/L; pH = ?**
3. **[H⁺] = 0.000001 moles/L; pH = ?**
4. **[H⁺] = 0.00000302 moles/L; pH = ?**
5. **[H⁺] = 9.1 x 10⁻⁷ moles/L; pH = ?**
6. **[H⁺] = 0.05μE/L; pH = ?**
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### Explanation:
To calculate the pH of a solution, use the formula:
\[ \text{pH} = -\log_{10} [\text{H}^+] \]
For each problem:
1. For [H⁺] = 10⁻⁹.³ moles/L:
\[ \text{pH} = -\log_{10} (10^{-9.3}) = 9.3 \]
2. For [H⁺] = 10⁻¹³.²³ moles/L:
\[ \text{pH} = -\log_{10} (10^{-13.23}) = 13.23 \]
3. For [H⁺] = 0.000001 moles/L:
\[ \text{pH} = -\log_{10} (0.000001) = 6 \]
4. For [H⁺] = 0.00000302 moles/L:
\[ \text{pH} = -\log_{10} (0.00000302) \approx 5.52 \]
5. For [H⁺] = 9.1 x 10⁻⁷ moles/L:
\[ \text{pH} = -\log_{10](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2c3da103-2d04-47ed-aa8d-fc15d595c069%2Faf3c98bf-d6da-4e77-a685-4efbc617404c%2Fx61gq4_processed.jpeg&w=3840&q=75)
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