Think of three ways you could safely distinguish between a strong acid and a strong base.

--Acid is the substance when dissolved in water, increases the concentration of H+ ions.

--Such compound whose chemical formula begins with H, for example HCl (Hydrochloric acid), H3BO3 (Boric acid), CH2O3 (Carbonic

acid). Although CH3COOH (Acetic acid) is an exception.

--Its less than 7.

--Bases are the proton acceptor.

--Such compounds whose chemical formula ends with OH, for example KOH (Potassium hydroxide), NaOH (Sodium hydroxide).

--Its greater than 7.

Explanation:

Molarity of sodium acetate you will need to add is 0.0324M

Explanation:

Assuming volume of the buffer is 1L.

The pH of a buffer can be determined using Henderson-Hasselbalch equation:

pH = pKa + log [A⁻] / [HA]

Where pKa is pKa of the weak acid,  [A⁻] molar concentration of conjugate base and [HA] molar concentration of weak acid

Replacing for the acetic buffer (pKa = 4.76):

pH = 4.76 + log [Sodium Acetate] / [Acetic Acid]

As you have 0.010 moles of acetic acid in 1L:

[Acetic Acid] = 0.010mol / 1L = 0.010M

And you require a pH of 5.27:

5.27 = 4.76 + log [Sodium Acetate] / [0.010M]

0.51 = log [Sodium Acetate] / [0.010M]

10^0.51 = [Sodium Acetate] / [0.010M]

3.236 =  [Sodium Acetate] / [0.010M]

3.236 [0.010M] = [Sodium Acetate]

0.0324M = [Sodium Acetate]