A beaker holds a mixture of 0.40 M HIO3 and 1.0 M HCOOH. Ka(HIO3) = 1.6 x 10-1 Ка(нсоон) = 1.77 × 10-4 What is the pH of the mixture of acids? pH = [?]
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.
![## Determining the pH of a Mixture of Acids
### Problem Statement:
A beaker holds a mixture of 0.40 M HIO₃ and 1.0 M HCOOH.
### Given:
- The acid dissociation constant for HIO₃, \( K_a(HIO₃) = 1.6 \times 10^{-1} \)
- The acid dissociation constant for HCOOH, \( K_a(HCOOH) = 1.77 \times 10^{-4} \)
### Question:
What is the pH of the mixture of acids?
### Calculation:
To determine the pH of the mixture, you need to consider the contributions of both HIO₃ and HCOOH to the concentration of hydrogen ions [H⁺] in the solution. Generally, if one of the acids is significantly stronger than the other (i.e., has a larger \( K_a \)), it will contribute more significantly to the [H⁺] and, thus, the pH of the solution.
In this case, HIO₃ is the stronger acid as it has a larger \( K_a \):
\[ K_a(HIO₃)=1.6 \times 10^{-1} \]
\[ K_a(HCOOH)=1.77 \times 10^{-4} \]
Therefore, the stronger acid HIO₃ will primarily determine the pH.
To estimate the pH:
1. Calculate the H⁺ concentration for the stronger acid HIO₃.
2. Determine the pH from the H⁺ concentration.
### Input Field:
Below, you can enter the calculated pH of the mixture:
#### pH of Mixture:
```
[ ________________ ] [Enter]
```
Enter your solution to check if it matches with the calculated value of pH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa4c65346-a6bd-47be-a891-a239e86f6fd1%2F95ac785a-ed4d-4490-919b-a3f9edf9e630%2Fnyv73v_processed.jpeg&w=3840&q=75)
Step by step
Solved in 2 steps with 2 images
