A buffer solution is made that is 0.329 M in HF and 0.329 M in KF. If K. for HF is 7.20 x 104, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.093 mol KOH is added to 1.00 L of the buffer solution.
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.
![**Buffer Solution Problem**
A buffer solution is made that is 0.329 M in HF and 0.329 M in KF.
If \( K_a \) for HF is \( 7.20 \times 10^{-4} \), what is the pH of the buffer solution?
**pH =** [Enter answer here]
**Net Ionic Equation Problem**
Write the net ionic equation for the reaction that occurs when 0.093 mol KOH is added to 1.00 L of the buffer solution.
*(Use the lowest possible coefficients. Omit states of matter.)*
[Reactant 1] + [Reactant 2] → [Product 1] + [Product 2]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F00585539-79e1-42a7-8a75-95bc6de8d9d5%2F6960dc69-c285-4136-878b-999d7c1bd803%2Fo5yhbua_processed.jpeg&w=3840&q=75)
![**Buffer Solution Design**
*Objective: Design a buffer with a pH of 5.65 using one of the weak base/conjugate acid systems.*
**Data Table:**
| Weak Base | \( K_b \) | Conjugate Acid | \( K_a \) | \( pK_a \) |
|---------------|-----------------|-----------------|------------------|-----------|
| \( \text{CH}_3\text{NH}_2 \) | \( 4.2 \times 10^{-4} \) | \( \text{CH}_3\text{NH}_3^+ \) | \( 2.4 \times 10^{-11} \) | 10.62 |
| \( \text{C}_6\text{H}_{15}\text{O}_3\text{N} \) | \( 5.9 \times 10^{-7} \) | \( \text{C}_6\text{H}_{15}\text{O}_3\text{NH}^+ \) | \( 1.7 \times 10^{-8} \) | 7.77 |
| \( \text{C}_5\text{H}_5\text{N} \) | \( 1.5 \times 10^{-9} \) | \( \text{C}_5\text{H}_5\text{NH}^+ \) | \( 6.7 \times 10^{-6} \) | 5.17 |
**Problem Statement:**
Determine the mass of the bromide salt of the conjugate acid that must be combined with the corresponding mass of the weak base to prepare 1.00 L of a buffer that is 1.00 M in the weak base.
**Required Inputs:**
- Grams of bromide salt of the conjugate acid = [Input field]
- Grams of weak base = [Input field]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F00585539-79e1-42a7-8a75-95bc6de8d9d5%2F6960dc69-c285-4136-878b-999d7c1bd803%2Fwy14x0g_processed.jpeg&w=3840&q=75)
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