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H2PO4 -1 has a pKa of 6.86. If the concentration of H2PO4 -1 is 0.422 mM and the concentration of H1PO4 -2 is 0.068 mM what is the pH of the solution?

Sagot :

Dejanrasidn

The pH of the solution is 6.07.

pKa = 6.86; the acid equilibrium constant

c(H₂PO₄⁻) = 0.422 mM; concentration of the acid

c(HPO₄²⁻) = 0.068 mM; concentration of the salt

Henderson–Hasselbalch equation for the buffer solution:

pH = pKa + log(c(HPO₄²⁻)/c(H₂PO₄⁻))

pH = 6.86+ log (0.068 mM/0.422 mM).

pH = 6.86 + log0.161.

pH = 6.86 - 0.79

pH = 6.07; potential of hydrogen

pH (potential of hydrogen) is a numeric scale used to specify the acidity or basicity an aqueous solution.

When pH is less than seven (pH<7), solution is acidic..

When is equal seven (pH = 7), solution is neutral.

When pH is greater than seven (pH > 7), solution is basic.

More about buffer: brainly.com/question/4177791

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