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Hot Tip! Remember that to know if our problem is before equivalence we have to look at how much of our NaOH is being added to the solution. In this case, it is 13.96, and by calculating our V2=76.7752 we conclude that our problem is before equivalence.

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Hot Tip! Remember that to know if our problem is before equivalence we have to look at how much of our NaOH is being added to the solution. In this case, it is 13.96, and by calculating our V2=76.7752 we conclude that our problem is before equivalence.

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Let's just say for example if our NaOH solution that is being added is higher than our V2 than it is after equivalence, and if it is equal to it is at equivalence!

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You have successfully solved a titration problem! As long as you solve step by step titration problems are a piece of cake!

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You have successfully solved a titration problem! As long as you solve step by step titration problems are a piece of cake!

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Finally, we use the Henderson-Hasselbalch equation to find the pH.

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Finally, we use the Henderson-Hasselbalch equation to find the pH.

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Rounded to 2 decimal places the pH is 4.04!

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Next, we have to write the equation for the solution at equilibrium and create or BCA table.

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Next, we have to write the equation for the solution at equilibrium and create or BCA table.

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Then, we have to find moles of HCH3CO2 and NaOH.

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Then, we have to find moles of HCH3CO2 and NaOH.

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Next, we need to calculate the volume of NaOH needed for equivalence by using the M1V1=M2V2 formula.

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Next, we need to calculate the volume of NaOH needed for equivalence by using the M1V1=M2V2 formula.

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By finding V2 we see that our problem is before equivalence.

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So the first thing that should be done is to write out our balanced equation for acetic acid and NaOH.

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So the first thing that should be done is to write out our balanced equation for acetic acid and NaOH.

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A chemist titrates 241.7 mL of a 0.2700 M solution of acetic acid (HCH3CO2) with a 0.8500 M solution of NaOH. Calculate the pH of the acid solution after the chemist has added 13.96 mL of the NaOH solution to it. *The pKa of acetic acid is 4.70*

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A chemist titrates 241.7 mL of a 0.2700 M solution of acetic acid (HCH3CO2) with a 0.8500 M solution of NaOH. Calculate the pH of the acid solution after the chemist has added 13.96 mL of the NaOH solution to it. *The pKa of acetic acid is 4.70*

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First before starting the problem take a breather and have confidence that you can tackle this problem even if it feels like tackling you.

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First before starting the problem take a breather and have confidence that you can tackle this problem even if it feels like tackling you.

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Now that we've got that out of the way let us read and determine if our problem is before, at, or after equivalence.