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.
![**Question:**
What volume (in mL) of 15.8 M HNO₃ would be required to make 500.0 mL of a solution with a pH of 3.20?
**Calculator Interface:**
- A calculator is displayed with buttons numbered from 0 to 9 and additional buttons for operations such as +/- and scientific notation (x 10^□).
- There is a text box labeled "mL" for entering or displaying the result.
**Solution Steps:**
To solve the problem, follow these steps:
1. **Determine the Hydronium Ion Concentration ([H⁺]):**
\[ \text{pH} = -\log [\text{H}⁺] \]
\[ 3.20 = -\log [\text{H}⁺] \]
\[ [\text{H}⁺] = 10^{-3.20} \approx 6.31 \times 10^{-4} \, \text{M} \]
2. **Use the Dilution Formula:**
\[ C_1V_1 = C_2V_2 \]
Where:
- \( C_1 = 15.8 \, \text{M} \) (concentration of HNO₃)
- \( V_1 \) = volume of HNO₃ needed (unknown)
- \( C_2 = 6.31 \times 10^{-4} \, \text{M} \) (target concentration)
- \( V_2 = 500.0 \, \text{mL} \)
3. **Solve for \( V_1 \):**
\[ V_1 = \frac{C_2 \times V_2}{C_1} \]
Substitute the known values:
\[ V_1 = \frac{(6.31 \times 10^{-4} \, \text{M}) \times (500.0 \, \text{mL})}{15.8 \, \text{M}} \]
\[ V_1 = \frac{0.3155}{15.8} \]
\[ V_1 \approx 0.01996 \, \text{mL} \]
Therefore, approximately 0.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F88c4a12b-1ea9-44c1-9400-53c8c9c9bde6%2F9ad971eb-69b0-41f3-a1dc-c1003fc0f628%2Fnru6yzb_processed.png&w=3840&q=75)
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