ding the Consider the following data on some weak acids and weak bases: name acetic acid acid hydrofluoric acid solution 0.1 M CsHsNHBr 0.1 M NaCH3CO₂ 0.1 M NaCl 0.1 M KF K₁ formula HCH₂CO₂ 1.8 x 105 HF 6.8 x 104 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. PH choose one choose one choose one base ✓ choose one 1 (lowest) 2 3 4 (highest) K₂ name ammonia NH3 1.8 × 10 5 pyridine CHN 1.7×10 ⁹ -9 formula
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.
![**Consider the following data on some weak acids and weak bases:**
| **Acid** | **Formula** | **Kₐ** |
|--------------------|-------------|--------------|
| Acetic acid | CH₃CO₂H | 1.8 × 10⁻⁵ |
| Hydrofluoric acid | HF | 6.8 × 10⁻⁴ |
| **Base** | **Formula** | **Kᵦ** |
|--------------------|-------------|--------------|
| Ammonia | NH₃ | 1.8 × 10⁻⁵ |
| Pyridine | C₅H₅N | 1.7 × 10⁻⁹ |
Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on.
**Solution** | **pH**
|-------------|--------
| 0.1 M C₅H₅NHBr | [dropdown] choose one (1 lowest to 4 highest)
| 0.1 M NaCH₃CO₂| [dropdown] choose one (1 lowest to 4 highest)
| 0.1 M NaCl | [dropdown] choose one (1 lowest to 4 highest)
| 0.1 M KF | [dropdown] choose one (1 lowest to 4 highest)
**Explanation**: Click the "Explanation" button to learn more about how to determine the pH of these solutions based on the ionization constants (Kₐ and Kᵦ) of their components.
**Check**: After selecting the relative pH order, click "Check" to verify your choices.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe03ae0e4-1943-4b04-991c-bc8a9e9b7172%2Fd52498c6-b748-4dcf-a067-4b465fdb70dc%2Fslvuhh_processed.jpeg&w=3840&q=75)
The question is based on the concept of pH of the solution. It is defined as a negative logarithm of hydrogen ion concentration present in a solution.
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