Show how would you prepare a solution of 500 ml of a 0.15 M acetate buffer....

Show how would you prepare a solution of 500 ml of a 0.15 M acetate buffer. You have available the following: 6M HCl, 4 M acetic, solid sodium acetate, solid sodium hydroxide

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Expert Solution

in the question, pH = 4.6

pH of acidic buffer = pka + log(sodiumacetate/acetic acid)

pka of aceticacid = 4.76

pH = 4.6

no of mol of buffer = 500*0.15/1000 = 0.075 mol

4.6 = 4.76+log(x/(0.075-x))

x = 0.03067 mol

no of mole of sodium acetate = x = 0.03067 mol

mass of sodium acetate must take = x*Mwt

                                   = 0.03067*82

                   = 2.515 g

no of mole of aceticacid = 0.075-x

= 0.075-0.03067

= 0.0443 mol

volume of aceticacid = n/M = 0.0443/6*1000 = 7.383 ml

so that, take 7.383 ml of 6M aceticacid and 2.515 grams of sodium acetate and dissolve it in minimum water,then add water up to 500 ml.

queen_honey_blossom answered 1 year ago

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