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12 Dec 2019

Suppose one mixes 100 mL of 0.150 M potassium hydrogen phthalate with 100 mL of 0.0800 M NaOH. write the balanced chemical equation showing the chemistry of the salt. then upon addition of NaOH to the salt solution write the balanced chemical equation for the chemistry that occurs. finally calculate the solution pH. I understand that to find the pH you will use HP + OH -----> P2- + H2O but why?

can this solution be considered a buffer?

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Question 5

A. How many mL of 0.1 M CH3COONa must you add to 35.0 mL of 0.50 M CH3COOH to make a buffer of pH 4.7? [pKa of H3COONa is 4.75]

B. Use the Henderson-Hasselbalch equation to calculate how many mL of 0.1 M HCl must you add to 100 mL of 0.10 M Tris base to make a buffer of pH 8.8? [pka of Tris Base is 8.08]

C. What is the pH when 25.0 mL of 0.200 M of H3COONa has been titrated with 35.0 mL of 0.100 M NaOH? Write out the balanced chemical equation.

D. You need to produce a buffer solution that has a pH of 4.68. You already have solution that contains 15.0 mmol of H3COONa. How many millimoles of H3COONa should you add to this solution?

âWhen a strong base is gradually added dropwise to a weak acid, the pH changes at each addition. When the appropriate quantity of base has been added to react with all of the acid, the pH changes sharply, indicating the endpoint of the titration. A plot of pH versus volume of base added gives what is known as a titration curveâ.

Consider the titration of 25.00 mL of 0.1000 M benzoic acid with 0.1000 M NaOH,.

Write a balanced chemical equation for the titration reaction using C6H5COOH for benzoic acidâs formula.

Determine the volume of NaOH solution required to reach the endpoint.

The chart on the next page has entries for several steps along the titration curve. To calculate the pH at each step, you first must understand the chemistry at that step, and then you can decide the appropriate method to calculate the pH. For each volume listed, (i) list the major species in solution, (ii) determine whether the Ka equation, Kb equation, buffer equation, or solution equilibrium equation is appropriate for the calculation of the solution [H3O+] and pH, and (iii) complete the calculations.

Volume NaOH Added (mL)	Major Species	Appropriate Equation	[H3O+]	pH
0.00
5.00
12.50
20.00
25.00
30.00

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