Q2. Calculate the pH of a 6.73 x 10 M H3PO4 (phosphoric acid) solution. Molar mass H3PO4 = 97.994 pH = -log[H¹] Poy-3H+ трой mol PH=-lug CHT? Density H3PO4 = 1.88 -105 [ 20.19 × 10 -47=-=-109(20.145+4109 | ml
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.
![**Transcription for Educational Website**
---
**Title: Understanding pH and Concentration Calculations**
**Question 2: Calculate the pH of a 6.73 x 10^-4 M H3PO4 (phosphoric acid) solution.**
- **Formula:** pH = -log[H+]
- **Molar mass of H3PO4:** 97.994 g/mol
- **Density of H3PO4:** 1.88 g/mL
**Solution:**
The dissociation of phosphoric acid is shown as:
\[ 3 \times 6.73 \times 10^{-4} \rightarrow 3H^+ + PO_4^{3-} \]
This implies:
\[ \text{pH} = -\log[ \text{H}^+] = -\log(2.019 \times 10^{-3}) \]
The calculated pH is 2.69.
**Question 3: Calculate the [H+] (concentration of the H+) of an HCl solution when the pH = 2.88.**
- **Hint to solve Q3:** Use the antilog function (inverse log).
- **Molar mass of HCl:** 36.458 g/mol
- **Density of HCl:** 1.18 g/mL
For HCl, when pH = 2.88:
\[ \text{[H}^+\text{]} = 10^{-\text{pH}} = 10^{-2.88} \]
The calculated concentration \([H^+]\) is approximately:
\[ 1.318 \times 10^{-3} \, \text{M} \approx 1.3 \times 10^{-3} \, \text{M} \]
The values calculated show important applications of the logarithmic and exponential functions in chemistry, specifically in calculating the acidity of solutions. Understanding these concepts is crucial for accurately gauging the properties of acidic or basic solutions.
---
End of Transcription](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F21c9e2c1-3922-4190-983a-755fc6e01f0b%2F4ddc8b50-225e-40a4-9ddc-3359c9020683%2Fjq68soo_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 2 images
