18 If a titration used 23.75mL of a 0.100M NaOH solution to reach the endpoint, then how many moles of NaOH were consumed? How many moles of ascorbic acid reacted from Q#2?
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.
![**Titration Calculations**
1. **Calculation of Moles of NaOH Consumed**
If a titration used 23.75 mL of a 0.100 M NaOH solution to reach the endpoint, then how many moles of NaOH were consumed?
2. **Calculation of Moles of Ascorbic Acid**
How many moles of ascorbic acid reacted from Q#2?
3. **Calculation of Moles of KIO₃ Consumed**
If a titration used 8.50 mL of a 0.0300 M KIO₃ solution to reach the endpoint, then how many moles of KIO₃ were consumed?
- **Explanation:**
For each calculation, use the molarity formula:
\( \text{Moles} = \text{Volume (L)} \times \text{Molarity (M)} \)
This relationship helps determine the number of moles of the titrant used in the titration process.
- For NaOH:
Given Volume \( = 23.75 \text{ mL} \) (convert to Liters: \( 23.75 \text{ mL} = 0.02375 \text{ L} \))
Given Molarity \( = 0.100 \text{ M} \)
\[
\text{Moles of NaOH} = 0.02375 \text{ L} \times 0.100 \text{ M} = 0.002375 \text{ moles}
\]
- For ascorbic acid:
This value typically is derived from a previous calculation or information provided in a preceding problem (Q#2). Assuming a 1:1 molar ratio in the reaction:
\[
\text{Moles of Ascorbic Acid} = \text{Moles of NaOH} = 0.002375 \text{ moles}
\]
- For KIO₃:
Given Volume \( = 8.50 \text{ mL} \) (convert to Liters: \( 8.50 \text{ mL} = 0.00850 \text{ L} \))
Given Molarity \( = 0.0300 \text{ M} \)
\[
\text{Moles of](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F85d00984-ae34-4416-a50e-e3da2d4d22d5%2F92fa68c8-6dc4-49fe-a489-2be96b87b451%2Fs6rrgjx_processed.jpeg&w=3840&q=75)
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