Rank the following salts in order of increasing pH of 0.1 M aqueous solutions. (Hint: write out the reactions of the salts + water and then look up the relevant Ka or Kb values) e) KNO3 K2SO4 K₂S f) NH4NO3 NaHSO4 NaHCO3 Na2CO3
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.
![**Rank the following salts in order of increasing pH of 0.1 M aqueous solutions. (Hint: write out the reactions of the salts + water and then look up the relevant Ka or Kb values)**
**e)**
- KNO3
- K2SO4
- K2S
**f)**
- NH4NO3
- NaHSO4
- NaHCO3
- Na2CO3
**Notes for Ranking:**
1. **Identify the Nature of Ions:**
- Determine if the ions from the salts will react with water to produce acidic or basic solutions.
- For example, KNO3 (potassium nitrate) will dissociate into \( K^+ \) and \( NO_3^- \) ions. Both \( K^+ \) and \( NO_3^- \) ions do not hydrolyze in water, so the solution remains neutral.
- On the other hand, Na2CO3 (sodium carbonate) dissociates into \( Na^+ \) and \( CO_3^{2-} \). The \( CO_3^{2-} \) ion hydrolyzes to produce \( OH^- \), making the solution basic.
2. **Review Reactions with Water:**
- Write the hydrolysis reactions for the anions and cations:
- For example, \( Na_2CO_3 \):
\[
CO_3^{2-} + H_2O \leftrightharpoons HCO_3^- + OH^-
\]
- Examine the resulting \( H_3O^+ \) or \( OH^- \) concentrations to infer acidity or basicity.
3. **Use \( K_a \) or \( K_b \) Values:**
- Review the dissociation constants of the conjugate acids/bases to accurately rank the pH of the solutions.
By following these steps, you will be able to rank the salts in order of increasing pH from the most acidic to the most basic.
**Illustrative Calculations:**
1. **KNO3:**
- \( KNO_3 \rightarrow K^+ + NO_3^- \)
- Both ions are neutral in solution (pH ≈ 7).
2. **K2SO4:**
- \( K_2SO_4 \rightarrow 2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fad29c243-17bc-495f-9a75-f51d725c2e92%2F6e89985c-197d-450e-a71b-e43f156f9a06%2F1nu3ox_processed.png&w=3840&q=75)
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