A 14 mL solution of 0.01 M HC is titrated with 0.01 M NaOH to give the following

Question

A 14 mL solution of 0.01 M HC is titrated with 0.01 M NaOH to give the following titration curve. Determine the key features of this curve. (The titration curve is approximate and may not show all aspects adequately.) pH 14 12 10 Base Added (mL) 28 7 14 2 The titration curve has the following features (1) Before any base is added, the pH of the starting solution of 0.01 M HCl is gradually but remains in the --select... region. In this area, the solution contains an (2) When small amounts of base are added, up to about 12 mL, the pHct excess of H30+ ons. (3) At and around the equivalence point, the pH rises dramatically, going from the acidic region to the basic region. At the equivalence point, when [H30+1-OH1.the pH is

Explanation / Answer

In the first part , 14 mL of 0.01 M HCl is titrated with 0.01M NaOH.

Q1) of part one

the pH of the solution before any base is added

From the graph , the starating point corresponds to 2.0

Thus the pH of solution before addition of base = 2.0

From the concentration of acid

[H+] = 0.01 = 1.0x10-2 M

Thus pH =- log [H+]

= - log 0.01

= 2.0

Q3) of part one

At the equivalence point where [H+] = [OH-] the pH of the solution = 7.0.

This is becuase when there is no extra acid or base in solution , all the H+ or OH- come from water's self ionisation.

2 H2O --------------> H3O+ + OH-

in water , [H+] = [OH-] = 1.0x10-7 M

Thus pH = 7.0 at the equivalence point.

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