Question

Consider the titration of 50.0 ml of 0.314 m weak base b ( kb =7.5*; 10 ^ - 6 ) with 0.340 mhn*o_{3} what is the ph of the solution after the addition of 30.0 ml of hn * o_{3}'

Answer 1

To calculate the pH of the solution after the addition of 30.0 ml of HNO3 to the weak base B, you would need to determine the moles of HNO3 and the weak base B, and then calculate the concentration of OH- ions in the solution. Finally, you can determine the pH from the pOH using the equation pH = 14 - pOH.

Step-by-step explanation:

Calculating the pH during the Titration of a Weak Acid

To calculate the pH of the solution after the addition of 30.0 ml of HNO3, we need to consider the reaction between the weak base B and HNO3.

First, determine the moles of HNO3 added:

1. Convert the volume of HNO3 added (30.0 ml) to moles using the molarity of HNO3 (0.340 M).
2. Calculate the moles of OH- ions that react with the HNO3 based on the stoichiometry of the reaction.

Next, determine the moles of weak base B:

1. Convert the volume of weak base B (50.0 ml) to moles using the molarity of B (0.314 M).

Combine the moles of HNO3 and weak base B to determine the moles of the resulting species.

Finally, calculate the concentration of OH- ions in the solution and use this to determine the pH of the solution using the pOH equation:

1. Calculate the concentration of OH- ions using the combined moles of reactants and products.
2. Calculate the pOH using the equation: pOH = -log[OH-].
3. Calculate the pH using the equation: pH = 14 - pOH.