You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka = 1.8

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please help with these 3 questions

Show by a balanced equation how each of the following salts, if any, is hydrolyzed by water, then tell which salt would give an acidic, basic, or neutral solution:

(i) Na₂CO3 (ii) Al(NO₃)₃ (iv) HCOONa

5. Calculate the pH of a buffer solution prepared by mixing 20.0 mL of 0.20 M acetic acid with 10.0 mL of sodium acetate. Ka for acetic acid = 1.8 x 10-5

6. Calculate the pH of a buffer solution prepared by mixing 20.0 mL of 0.20 M in ammonia and

15. 0 mL of 0.30 M in ammonium chloride? Assume the total volume is 35.0 mL. Kb for ammonia is 1.8 x 10-5.

(a) Suppose you have two stock solutions 0.50 M CH3COOH and 0.50 M CH3COONa. Is these were mixed together would this be a buffer? How many milliliters of sodium acetate do you need to add to obtain a pH of 5.45 if you start with 100 mL of acetic acid? Ka = 1.8 X 10-5

A biochemist needs 750 mL of an acetic acid–sodium acetate buffer with pH 4.50. Solid sodium acetate (CH₃COONa) and glacial acetic acid (CH₃COOH) are available. Glacial acetic acid is 99% CH₃COOH by mass and has a density of 1.05 g/mL. If the buffer is to be 0.15 M in CH₃COOH, how many grams of CH₃COONa and how many milliliters of glacial acetic acid must be used?