You want to adjust the pH of a liter of strong acid from 2.93 to 3.43. Part 1 of 2 Which ion must be added to the solution to adjust it's pH? Select the single best answer. OH H₂O* Part: 1/2 Part 2 of 2 How many moles of OH must you add to achieve this change? Round your answer to 2 significant figures. moles 0.8 X
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.
![**Adjusting the pH of a Strong Acid Solution**
*Objective:*
To adjust the pH of 1 liter of a strong acid solution from 2.93 to 3.43.
**Part 1 of 2: Ion Selection**
To adjust the solution's pH, determine which ion needs to be added. Choose the best answer from the options given:
- \( \text{OH}^- \)
- \( \text{H}_3\text{O}^+ \)
**Selection Process:**
Identify which ion will increase the pH, thereby reducing the solution’s acidity.
**Progress Indicator:**
[Progress Bar Image: Part 1 / 2 completed]
**Part 2 of 2: Calculating Moles of Ion**
Calculate the number of moles of \( \text{OH}^- \) required to achieve this pH adjustment. The answer should be rounded to 2 significant figures.
- Input Box: [ ] moles
- Additional Functions:
- Reset Button (x)
- Submit/Confirm Button (circular arrow)
*Note: Ensure to perform the calculation taking into account the properties of the strong acid and the nature of \( \text{OH}^- \) as a strong base.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Feb2e15ef-8640-49b0-a75f-b139085238e1%2F0171260c-ff8f-4753-94b2-f7f3ce8d90e3%2F83b5rio_processed.png&w=3840&q=75)
Step by step
Solved in 3 steps with 21 images
