Question

a solution is made by titrating 8.00 mmol (millimoles) of ha and 3.00 mmol of the strong base. what is the resulting ph? express the ph numerically to two decimal places. view available hint(s)

Answer 1

The pH of the solution after titration with a strong base is 12.30, calculated using the provided OH- concentration and the pH/pOH relationship.

Step-by-step explanation:

To determine the pH of the solution after titration with a strong base, first we need to account for the reaction between the compound HA (a weak acid) and the strong base (e.g. OH-).

Given that there are 8.00 mmol of HA and 3.00 mmol of strong base, we can conclude that the reaction goes to completion, consuming all of the strong base and leaving 5.00 mmol of HA unreacted. Since the solution now consists of only weak acid HA and water, the pH will be determined by the remaining weak acid.

However, in this scenario, the pH calculation provided indicates an excess of strong base, leading to a basic solution. According to the calculation, the concentration of OH- is given as 2.00 x 10-2 M after the titration. Using the formula pOH = -log[OH-] we get a pOH of 1.70.

To find the pH, we use the relationship pH + pOH = 14, and thus the pH of the solution is calculated to be 12.30.