Answer:
pH= 12.52
Step-by-step explanation:
First, calculate the moles of acid in the solution:
(0.050 L)(0.10molL)=0.0050 mol acid
Next, calculate the moles of base:
(0.100 L)(0.100molL)=0.0100 mol base
The strong acid and strong base will dissociate completely to generate the same number of moles of hydronium and hydroxide, respectively. The amount of base exceeds the amount of acid, so all of the hydronium will be neutralized, leaving an excess of hydroxide. To find the remaining amount of hydroxide, we subtract the moles of hydronium added (equal to the moles of hydroxide neutralized) from the moles of hydroxide added:
0.0100 mol OH−−0.0050 mol H3O+=0.0050 mol OH−
To find the concentration of hydroxide, we must divide this number of moles by the total volume of solution, being sure to add the volumes of acid and base added together:
0.0050 mol OH−0.150 L=0.033 M OH−
Take the negative logarithm of this concentration to obtain the pOH:
-log(0.033)=1.48
Finally, to obtain the corresponding pH, subtract this number from 14.00:
14.00−1.48=12.52