What’s the answer for #9
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Hello!
A solution of a weak acid and its conjugate base is called a buffer solution. It can resist the addition of bases and acids while maintaining the pH approximately constant.
To calculate the pH of a buffer solution, we'll use the famous Henderson-Hasselbach equation, applying the pKa value of the Benzoic Acid (4,20). In this equation, [A⁻] represents the concentration of the Conjugate Base and [HA] the concentration of the acid.
![pH=pKa + log( \frac{ [A^{-}]}{[HA]} ) \\ \\ pH=4,20 + log ( \frac{0,170 M}{0,245} ) \\ \\ pH=4,04](https://tex.z-dn.net/?f=pH%3DpKa%20%2B%20log%28%20%5Cfrac%7B%20%5BA%5E%7B-%7D%5D%7D%7B%5BHA%5D%7D%20%29%20%5C%5C%20%20%5C%5C%20pH%3D4%2C20%20%2B%20log%20%28%20%5Cfrac%7B0%2C170%20M%7D%7B0%2C245%7D%20%29%20%5C%5C%20%20%5C%5C%20pH%3D4%2C04%20)
So, the pH of the solution would be 4,04.
Have a nice day!
A solution of a weak acid and its conjugate base is called a buffer solution. It can resist the addition of bases and acids while maintaining the pH approximately constant.
To calculate the pH of a buffer solution, we'll use the famous Henderson-Hasselbach equation, applying the pKa value of the Benzoic Acid (4,20). In this equation, [A⁻] represents the concentration of the Conjugate Base and [HA] the concentration of the acid.
So, the pH of the solution would be 4,04.
Have a nice day!