Determine the pH of a solution that contains 5.3*10^-2 M in HClO4 and 3.0*10^-2 M in HCl?
Add (H^+) from HClO4 and (H^+) from HCl but be careful. You may NOT add molarities most of the time; you can here. If you want to see how it works, we can take 1L of the solution.
Then we have M x L = 0.053 x 1L = 0.053moles HClO4.
And we have M x L = 0.030 x 1L = 0.030 moles HCl.
Total moles = 0.053 + 0.030 = 0.083 moles (you CAN add moles--always), then
M = moles/L = 0.083/1L = 0.083 M.
Then pH = -log(H^+)
Why did the acid go to the comedy club? It wanted to find its pH balance!
Now, let's figure out the pH of this solution. HClO4 and HCl are strong acids that fully dissociate in water. The dissociation of HClO4 gives H+ ions while HCl dissociates into H+ and Cl- ions. Since they are both strong acids, they will contribute to the overall acidity of the solution.
Since HClO4 is a stronger acid than HCl, it will donate more H+ ions to the solution. Therefore, we can consider only the HClO4 concentration to calculate the pH.
So, the pH of the solution that contains 5.3*10^-2 M in HClO4 will be acidic. However, in order to calculate the exact pH, we need to know the dissociation constant (Ka) of HClO4. Without that information, I'm afraid I can't provide you with a precise numerical value.
But hey, at least you now know that the solution will be...acid-larious!
To determine the pH of the solution, you need to find the concentration of H+ ions in the solution.
First, we'll calculate the concentration of H+ ions from HClO4:
HClO4 → H+ + ClO4-
Here, HClO4 is a strong acid, so it ionizes completely in water. Therefore, the concentration of H+ ions is equal to the concentration of HClO4.
[H+] = 5.3 × 10^-2 M
Next, we'll calculate the concentration of H+ ions from HCl:
HCl → H+ + Cl-
Again, HCl is a strong acid, so it ionizes completely in water. Therefore, the concentration of H+ ions is equal to the concentration of HCl.
[H+] = 3.0 × 10^-2 M
Now, we'll combine the concentrations of H+ ions from both acids to get the total concentration of H+ ions in the solution.
Total [H+] = [H+] from HClO4 + [H+] from HCl
= (5.3 × 10^-2) M + (3.0 × 10^-2) M
= 8.3 × 10^-2 M
Finally, we'll calculate the pH using the formula:
pH = -log[H+]
pH = -log(8.3 × 10^-2)
pH ≈ 1.08
Therefore, the pH of the solution is approximately 1.08.
To determine the pH of a solution, we need to use the concept of strong acids. Both HClO4 (perchloric acid) and HCl (hydrochloric acid) are strong acids, meaning they completely dissociate in water.
The dissociation reaction for HClO4 is:
HClO4 → H+ + ClO4-
The dissociation reaction for HCl is:
HCl → H+ + Cl-
Since both acids completely dissociate, the concentration of H+ ions in the solution will be equal to the concentration of the respective acid.
For HClO4: [H+] = 5.3 × 10^-2 M
For HCl: [H+] = 3.0 × 10^-2 M
The pH scale is a logarithmic scale that measures the concentration of H+ ions in a solution. The pH is given by the formula: pH = -log[H+].
To find the pH for each acid, we can take the negative logarithm of the H+ concentration.
For HClO4:
pH = -log(5.3 × 10^-2)
pH ≈ -log(5) - log(10^-2)
pH ≈ -log(5) - (-2) [using the property log(a^b) = b × log(a)]
pH ≈ -log(5) + 2
pH ≈ 2 - log(5)
pH ≈ 2 - 0.699
pH ≈ 1.301
For HCl:
pH = -log(3.0 × 10^-2)
pH ≈ -log(3) - log(10^-2)
pH ≈ -log(3) - (-2)
pH ≈ -log(3) + 2
pH ≈ 2 - log(3)
pH ≈ 2 - 0.477
pH ≈ 1.523
Therefore, the pH of the solution containing 5.3 × 10^-2 M HClO4 and 3.0 × 10^-2 M HCl is approximately 1.301 for HClO4 and 1.523 for HCl.