Caloulate tOH] at 25° C solutionwidh for a conentrahion of TH30*] equal to 4.5x 10°3 M and a a determine if the solution is acidio, basic, ar neutral
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.
![**Calculation of Hydroxide Ion Concentration ([OH⁻]) at 25°C**
**Problem Statement:**
Calculate [OH⁻] at 25°C for a solution with a concentration of [H₃O⁺] equal to 4.5 x 10⁻³ M and determine if the solution is acidic, basic, or neutral.
**Solution:**
To determine the hydroxide ion concentration, we can use the water dissociation constant (Kw) at 25°C:
\[ K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14} \]
Given:
\[ [H_3O^+] = 4.5 \times 10^{-3} \, M \]
We can rearrange the formula to solve for [OH⁻]:
\[ [OH^-] = \frac{K_w}{[H_3O^+]} \]
Substituting the known values:
\[ [OH^-] = \frac{1.0 \times 10^{-14}}{4.5 \times 10^{-3}} \]
Perform the division:
\[ [OH^-] = 2.22 \times 10^{-12} \, M \]
**Determination of Solution Type (Acidic, Basic, or Neutral):**
- **Acidic Solution:** [H₃O⁺] > [OH⁻]
- **Neutral Solution:** [H₃O⁺] = [OH⁻]
- **Basic Solution:** [H₃O⁺] < [OH⁻]
Because:
\[ [H_3O^+] = 4.5 \times 10^{-3} \, M \]
\[ [OH^-] = 2.22 \times 10^{-12} \, M \]
Since [H₃O⁺] > [OH⁻], the solution is **acidic**.
**Conclusion:**
The solution, with a [H₃O⁺] concentration of 4.5 x 10⁻³ M, has a calculated [OH⁻] concentration of 2.22 x 10⁻¹² M and is determined to be acidic.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdabc7e8b-d42d-4c7a-8b8c-eac102cb510a%2F06d0cb0e-e5f2-4ac7-8d02-e74b821baf65%2Fv3i2p7n_processed.jpeg&w=3840&q=75)
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