Question #350208

calculate the pH of a solution prepared by dissolving 2.05 g of sodium acetate, CH3COONa, in 78.0 mL of 0.25 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. ka of CH3COOH is 1.75 x 10-5

1
Expert's answer
2022-06-13T22:52:03-0400

Moles of CH3COONa= 2.0582.0= 0.025 molMoles~ of~ CH3COONa= ~\cfrac{2.05}{82.0} = ~0.025 ~mol


Volume V=78.0 mL=0.078 LVolume~ V = 78.0 ~mL = 0.078~ L


 [CH3COONa]= 0.0250.078= 0.32 M[CH_3COONa]=~ \cfrac{0.025}{0.078} = ~0.32~M


[CH3COOH]=0.25 M[CH_3COOH] = 0.25~ M




pH= log(Ka)+ log([CH3COONa][CH3COOH])pH =~ -log(K_a) +~ log\bigg(\cfrac{[CH_3COONa]}{[CH_3COOH]}\bigg)



pH= log(1.75 105)+ log(0.320.25)pH =~ -log(1.75 *~10^{-5}) + ~log\bigg(\cfrac{0.32}{0.25}\bigg) \\



pH=4.757+0.079=4.836pH= 4.757 + 0.079 = 4.836



Answer: pH = 4,836





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