Calcualte PH and POh of an aqueous solution that is 0.050 M in HCL and 0.085 M in HBr at 25 degrees C
To calculate the pH and pOH of an aqueous solution, you need to know the concentration of the acid or base in the solution and apply the appropriate formulas. In this case, you have a solution that contains two different acids, HCl and HBr.
Step 1: Calculate the pH of the solution
The pH of an acidic solution is calculated using the formula:
pH = -log[H+]
For HCl:
[HCl] = 0.050 M
[H+] = 0.050 M (because HCl fully dissociates in water)
pH = -log(0.050) = 1.30
For HBr:
[HBr] = 0.085 M
[H+] = 0.085 M (because HBr fully dissociates in water)
pH = -log(0.085) = 1.07
Step 2: Calculate the pOH of the solution
The pOH of a solution is calculated using the formula:
pOH = -log[OH-]
Since HCl and HBr are acids, they don't produce hydroxide ions (OH-) in water. Therefore, the pOH of the solution is 0, as there are no hydroxide ions present.
So, the calculated values are:
pH = 1.30
pOH = 0
Please note that the pH and pOH values are temperature-dependent, and the calculations are assuming a temperature of 25 degrees Celsius.