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What is the ph of a buffer prepared by adding 0.506 mol of the weak acid ha to 0.609 mol of naa in 2.00 l of solution? the dissociation constant ka of ha is 5.66×10−7. express the ph numerically to two decimal places?

Respuesta :

mixter17
Hello!

To solve this question, we first have to know the pKa of the acid:

[tex]pKa=-log(Ka)=-log(5,66*10^{-7})=6,25 [/tex]

Now, we can apply the Henderson-Hasselbach's equation to determine the pH of the buffer solution:

[tex]pH=pKa+ log( \frac{[NaA]}{[HA]} )= 6,25 + log(\frac{(0,609 mol/2L)}{(0,506 mol/2L)})=6,33 [/tex]

So, the pH of this buffer solution is 6,33

Have a nice day!

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