2. What is the hydronium-ion concentration in a solution formed by combining 750. mL of 0.10 M NaOH with 250. mL of 0.30 M HCI at 25.0°C? NaOH(aq) + HCl(aq) ->> NaCl(aq) + H₂O(l)
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.
![**Problem 2: Calculation of Hydronium-Ion Concentration**
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**Question:**
What is the hydronium-ion concentration in a solution formed by combining 750. mL of 0.10 M NaOH with 250. mL of 0.30 M HCl at 25.0°C?
**Relevant Chemical Reaction:**
\[ \text{NaOH(aq)} + \text{HCl(aq)} \rightarrow \text{NaCl(aq)} + \text{H}_2\text{O(l)} \]
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**Solution Steps:**
To solve this problem, we follow these steps:
1. **Calculate the moles of NaOH and HCl:**
- Moles of NaOH = \( 0.10 \, M \times 0.750 \, L = 0.075 \text{ mol} \)
- Moles of HCl = \( 0.30 \, M \times 0.250 \, L = 0.075 \text{ mol} \)
2. **Determine the limiting reagent:**
- Both NaOH and HCl have the same number of moles (0.075 mol), so they will completely neutralize each other.
3. **Calculate the resulting moles of excess H\(_3\text{O}^+\) or OH\(^-\):**
- Since both reactants neutralize completely, there will be no excess H\(_3\text{O}^+\) or OH\(^-\) in the solution.
4. **Determine the total volume of the solution:**
- Total volume = 750 mL + 250 mL = 1000 mL = 1.00 L
5. **Calculate the hydronium-ion concentration:**
Since the solution is neutral (neither H\(_3\text{O}^+\) nor OH\(^-\) is in excess), the concentration of H\(_3\text{O}^+\) is equal to that of pure water at 25.0°C, which is \( 1.00 \times 10^{-7} \, M \).
\[ [\text{H}_3\text{O}^+] = 1.00 \times 10^{-7} \, M \]
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**Conclusion:**
The hydronium-ion concentration \](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb99220ad-d702-4943-b904-ec3abe399c73%2Fff912bfe-10a1-469f-a8af-37c20c80e6f0%2Fqo62ft9_processed.jpeg&w=3840&q=75)
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