An aqueous solution with a pH of 3.00 is diluted from 2.0 L to 4.0 L. Wht is the pH of the diluted solution?
pH = -log(H^+).
Plug in 3.00 for pH and calculate (H^+).
Since the solution is diluted by a factor of two, then (H^+) in the diluted solution will be 1/2 of the initial value. Plug in the new (H^+) and solve for the new pH. Hint: it will NOT be 1/2 of 3.00.
To find the pH of the diluted solution, we can use the fact that the pH scale is logarithmic.
The dilution equation is given as: M1V1 = M2V2
Given:
Initial volume (V1) = 2.0 L
Final volume (V2) = 4.0 L
Initial pH (pH1) = 3.00
Since we are diluting the solution by doubling the volume, the final concentration (M2) will be halved.
Now, let's solve for the final concentration (M2):
M1V1 = M2V2
M2 = (M1V1) / V2
M2 = (10^-pH1)(V1 / V2)
Substituting the given values:
M2 = (10^-3.00)(2.0 L / 4.0 L)
M2 = (0.001)(0.5)
M2 = 0.0005
Now, we can calculate the pH of the diluted solution using the concentration (M2):
pH2 = -log(M2)
pH2 = -log(0.0005)
pH2 ≈ 3.3
Therefore, the pH of the diluted solution is approximately 3.3.
To find the pH of the diluted solution, we need to use the concept of dilution. Dilution refers to the process of lowering the concentration of a solute in a solution by adding more solvent.
In this case, we are given an aqueous solution with a pH of 3.00 that is diluted from 2.0 L to 4.0 L. Since pH is a measure of the hydrogen ion concentration ([H+]), we can assume that the dilution process will not affect the concentration of hydrogen ions.
To understand this, we can use the equation for pH:
pH = -log[H+]
Since the dilution does not affect the concentration of hydrogen ions, the value of [H+] remains unchanged. Therefore, the pH of the diluted solution will be the same as the original solution, which is 3.00.
Hence, the pH of the diluted solution is also 3.00.