A solution that is 0.17m in HCHO2 and 0.11 Min in NaCHO2
1 answer:
Hello!
(Missing Previous Enunciate) <span>Use the Henderson-Hasselbalch equation to find the pH of:
To solve this question we need the pKa of HCOOH, which is 3,75, now, we can apply the Henderson-Hasselbach equation:
</span>![pH=pKa+ log( \frac{[HCOONa]}{[HCOOH]} )=3,75 + log( \frac{0,11M}{0,17M} )=3,56](https://tex.z-dn.net/?f=pH%3DpKa%2B%20log%28%20%5Cfrac%7B%5BHCOONa%5D%7D%7B%5BHCOOH%5D%7D%20%29%3D3%2C75%20%2B%20log%28%20%5Cfrac%7B0%2C11M%7D%7B0%2C17M%7D%20%29%3D3%2C56)
<span>
So, the pH of a solution that is 0,17 M in HCHO</span>₂ and 0,11 M in NaCHO₂ is 3,56
Have a nice day!
(Missing Previous Enunciate) <span>Use the Henderson-Hasselbalch equation to find the pH of:
To solve this question we need the pKa of HCOOH, which is 3,75, now, we can apply the Henderson-Hasselbach equation:
</span>
<span>
So, the pH of a solution that is 0,17 M in HCHO</span>₂ and 0,11 M in NaCHO₂ is 3,56
Have a nice day!
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