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How do you prepare 0.45 percent sls in 0.05 m acetate buffer pH 4.5?
Wiki User
∙ 13y ago
In general:
pHbuffer = pKa - log10 [ (acid) / (base) ]Legend:- pHbuffer = 4.5
- acid = acetic acid, amount in mmoles, unknown = A(mmol) = Volume(L)*conc(mmol/L)
- base= acetate, amount in mmoles = 50.0 mmol = 1.00(L)*50(mmol/L)
- to be known from table: pKa = 4.77 for acetic acid
Calculation:
Rearranging to: pKa - pHbuffer = log10[ acid / base ]
Inverting log to exponent:
[ acid / base ] = 10[ pKa - pH ] = INVlog[ pKa - pH ] = INVlog[ 4.77 - 4.5 ] = INVlog[0.27] = 100.27 = 1.86 (a/b ratio)
So if base (acetate) is to be 50.0 mmol (present in 1.00 L) then acid (acetic) has to be 93.0 mmol (because a/b ratio has to be 1.86 whence 93.0/50.0= 1.86).
Wiki User
∙ 13y ago
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