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Lecture 213/16/05

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1) For the titration of 100 mL of 0.15 M HCl with 0.1 M NaOH, fill in the table.

2) Why does adding water to a buffer solution not change the pH?

Give the identity and concentration of the titrated sample (50 mL) represented by the blue line.

- Describe the effect on the pH of
- Adding sodium acetate to 0.1 M acetic acid
- Adding NaNO3 to 0.1 M HNO3
- Why are the effects not the same?

In lab, you titrate a 25-mL sample of HCN with 0.075 M NaOH. If it takes 37.5 mL to reach the equivalence point, what is the concentration of the HCN?

- Which of these combinations would be the best to buffer the pH at approximately 9?
- CH3COOH (Ka = 1.8 x 10-5) / NaCH3COO
- HCl (Ka = very large) / HCl
- NH3 (Kb = 1.8 x 10-5) / NH4+

Each of the solutions given in the table has an equal volume and the same concentration (0.1 M)

Which solution requires the greatest volume of 0.1 M NaOH to titrate? Explain.

The solubility of Ca(OH)2 is 7.9 x 10-6.

What is the pH of a saturated solution of calcium hydroxide?

- A 25-mL sample of 0.085 M pyridine (Kb = 1.5 x 10-9) is titrated with 0.102 M HCl. What is the pH when 5.5 mL of the acid has been added?