HF and NaF - If the right concentrations of aqueous solutions are present, they can produce a buffer solution.
<h3>What are buffer solutions and how do they differ?</h3>
- The two main categories of buffers are acidic buffer solutions and alkaline buffer solutions.
- Acidic buffers are solutions that contain a weak acid and one of its salts and have a pH below 7.
- For instance, a buffer solution with a pH of roughly 4.75 is made of acetic acid and sodium acetate.
<h3>Describe buffer solution via an example.</h3>
- When a weak acid or a weak base is applied in modest amounts, buffer solutions withstand the pH shift.
- A buffer made of a weak acid and its salt is an example.
- It is a solution of acetic acid and sodium acetate CH3COOH + CH3COONa.
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3.25 C because I said so and energy is green
Aqueous nitric acid and aqueous ammonia reacts to form ammonium nitrate
HNO₃(aq)+NH₃(aq) = NH₄NO₃(aq)
HNO₃ +NH3 = NH₄ (+) + NO₃ (-)
Therefore the net ionic equation will be;
H⁺(aq) + NH₃ = NH₄⁺ (aq)
The awnser would be c i got you fam
Answer:
pH 4
Explanation:
Firstly, we define pH as the negative logarithm to base 10 of the concentration of hydrogen ions.
Mathematically, we express this as:
pH = -log[H+]
Now let’s us calculate the concentration of hydrogen in each of the pH
For pH 4, we have:
4 = -log[H+]
[H+] = -Antilog(4)
[H+] = 0.0001M
For pH 5,
[H+] = -Antilog(5)
[H+] = 0.00001M
We can see that 0.0001 is greater than 0.00001 and thus it has a greater concentration of hydrogen ions