THERMODYNAMICS
You have a phosphate buffer at pH 7.8. What ionic constituents are present in the buffer?
What are the fractions of each ionic constituent present at pH 7.8?
A buffer solution is combination of a weak acid and its conjucate base or a weak base and its conjucate acid
phosphate buffer is combination of Weak acid H2PO4- and its conjucate base HPO42-
H2PO4- <------> HPO42- + H+
Henderson - Hasselbalch equation is used to calculate the fracrion of weak acid and conjucate base
pH = pKa + log([A-]/[HA])
where, A- and HA are conjucate base and weak acid respectively
pKa of H2PO4- = 7.20
required pH = 7.8
7.8 = 7.20 + log([HPO42-]/[H2PO4-])
log([HPO42-]/[H2PO4-]) = 0.60
[HPO42-]/[H2PO4-] = 3.981
[HPO42-] = 3.981×[HPO4-]
if total buffer concentration = 1M
[H2PO4- ] + 3.981[H2PO4-] = 1M
4.981[H2PO4- ] = 1M
[H2PO4-] = 0.2008M
[HPO42-] = 0.1 - 0.2008M = 0.7992
Therefore,
Fraction of H2PO4- = 0.2008
Fraction of HPO42- = 0.7992
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