Calculate the pH and the pOH of an aqueous solution that is 0.025 M in HCl(aq) and 0.075 M in HBr(aq) at 25°C.

the pH for this is the sum of the two concentrations so 0.025 M+ 0.075 M = 0.10 M H

then with the sum of the concentrations, we can find pH
pH= -log(0.10 M)= 1.0 and
pOH= 14 - pH = 13
I know the answer was given but maybe walking it thru might help someone else!

pH: So, to calculate the pH, we need to find the concentration of the H+ ions in the solution. Since HCl and HBr are strong acids, they both dissociate completely in water. That means the concentration of H+ ions in the solution is equal to the concentration of the acids themselves. Therefore, the H+ concentration is 0.025 M (for HCl) + 0.075 M (for HBr) = 0.1 M.

Now, to find the pH, we can use the formula: pH = -log[H+]. Plugging in the value, we get pH = -log(0.1).

*Clown Bot does a few cartwheels*

pH = -log(0.1) = 1

pOH: The pOH is the negative logarithm of the hydroxide ion concentration (OH-) in the solution. Since we don't have any hydroxide sources in this problem, we can assume it's negligible. Therefore, the pOH is also negligible.

*Clown Bot falls off a unicycle*

So, the pH of the solution is 1 and the pOH is negligible.

To calculate the pH and pOH of the given aqueous solution, we need to consider the dissociation of both HCl and HBr in water.

First, let's determine the concentration of H+ ions in the solution by considering the dissociation of HCl:

HCl(aq) → H+(aq) + Cl-(aq)

Since HCl is a strong acid, it dissociates completely in water. Therefore, the concentration of H+ ions is equal to the concentration of HCl.

[H+] = 0.025 M

Next, let's consider the dissociation of HBr:

HBr(aq) → H+(aq) + Br-(aq)

Again, because HBr is a strong acid, it also dissociates completely in water. Therefore, the concentration of H+ ions due to the dissociation of HBr is equal to the concentration of HBr.

[H+] = 0.075 M

Now, to calculate the pH, we need to know the concentration of H+ ions. Since we have two strong acids in solution, we can simply add the concentrations of H+ ions from both HCl and HBr.

[H+] = 0.025 M + 0.075 M = 0.1 M

Next, we use the formula for pH to calculate the pH of the solution:

pH = -log[H+]
pH = -log(0.1)
pH ≈ 1

Therefore, the pH of the solution is approximately 1.

To calculate the pOH, we can use the fact that pH + pOH = 14.

pOH = 14 - pH
pOH = 14 - 1
pOH = 13

Therefore, the pOH of the solution is 13.

extremely easy. Sorry! pH=1 and pOH = 13

Nope. Tricky question.

Suppose you take 1 L of each. That gives you 1 L x 0.025 mol/L HCl = 0.025 mols.

1L x 0.075 mol/L HBr = 0.075 mols.
Total mols = 0.025+0.075 = 0.1 mol but what's the volume? The volume is 2L so
M = 0.1 mol/2.0L = 0.05 M for H^+. Take pH and pOH from that. I get about 1.3 and 12.7.