Question

Question: In the space below, discuss tour observations and compare the use of a buffered versus a non-buffered solution (DI water) with the addition of a strong acid or base.

Part C: K, Acid Dissociation Constant Acetic Acid pH | [H] | K Calculation Concentration (2.83 x 10 2.82 104 7.95 x 10-6 0.010 M 3.55 0.10 M (8.71 * 10-4) (0.1) 7.59x10-6 3.00 18.71x10 *M 1.0 M 2.71 (1.95 x 10-5) (1.03 1.95 x 10-3M 3.80 x 10-6 LHO PHS Average K for acetic acid: 6.45x10-6 ke for acetic acid. 6. ka [H][*] [HA] Part D: Buffers pH of acetic acid/sodium acetate buffer solution (HOAc/NaOAc) pH of acetic acid/sodium acetate buffer solution - 3 drops of 1 M HCI pH of acetic acid/sodium acetate buffer solution - 3 drops of 1 M NaOH 4 .5 4.3 4.8 pH of deionized water pH of water + 3 drops of 1 M HCI pH of water + 3 drops of 1 M NAOH 11.0 In the space below, discuss your observations and compare the use of a buffered versus a non-buffered solution (DI water) with the addition of a strong acid or base. Chapter 18 w Study 241

Answer 1

In acetic acid, sodium acetate buffer, upon addition of 3 drops of im Hee, pH decreases by 0.2 but it decreases by 14.1-1.8=2-3 in case of deionized water undergoing the same change Again, up on the addition of strong base NaOH, PH increases by 0.3 in buffered solution, where as an increase of (11.0-4.1)=6.9 in PH was seen in case of non-buffered deionized water. In conclusion, o we can say the buffered solution sustains (negligible change in pH) the addition of small amount of mong acid or base, whereas non buffered solutions are unable to sustain such change upon the addition of gt acid or base. - strong