- #1
Qube
Gold Member
- 468
- 1
Homework Statement
You mix the below two solutions. What is the resulting pH?
200 mL solution with [itex]H_{3}O^{+} = 1 * 10^{-4}[/itex]
100 mL solution with [itex]H_{3}O^{+} = 2 * 10^{-11}[/itex]
Homework Equations
[itex]pH = -log[H_{3}O^{+}][/itex]
[itex]N_{H_{3}O^{+}} = M * L[/itex]
The Attempt at a Solution
I first found the number of moles of hydronium ion on each of the two solutions by multiplying volume in liters by the molarity of the solution. For the first solution, the number of moles of hydronium ion is [itex]2 * 10^{-5}[/itex]. The second solution has [itex]2 * 10^{-12}[/itex] moles of hydronium ion.
I added the number of moles of hydronium ion and divided by the volume of the mixture - 300 mL or 0.3 L. This yields the new hydronium ion molarity.
I then took the negative logarithm of the hydronium ion molarity and found the pH to be approximately 4.
However, the key says the pH is instead approximately 10, which I noticed to be 14 - 4 ([itex]pK_{w} = 14 = pH + pHO[/itex]).
Why is the solution basic instead of acidic?