Chemistry, 10.03.2020 00:07 laurabwhiddon
Calculate the pH of a solution that is 0.239 M acetic acid and 0.190 M sodium acetate. The Ka of acetic acid is 1.76×10–5 at 25°C. What is the pH of this mixture at 0°C? (At 0°C, Ka = 1.64x10-5)
Answers: 3
![pH=pK_a+\log(\frac{[salt]}{[acid]})](/tpl/images/0539/1827/e4eea.png)
![pH=pK_a+\log(\frac{[CH_3COONa]}{[CH_3COOH]})](/tpl/images/0539/1827/05ea7.png)
= negative logarithm of acid dissociation constant of acetic acid at 0°C = 4.78![[CH_3COONa]=0.190M](/tpl/images/0539/1827/29d58.png)
![[CH_3COOH]=0.239M](/tpl/images/0539/1827/577dd.png)
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Calculate the pH of a solution that is 0.239 M acetic acid and 0.190 M sodium acetate. The Ka of ace...
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