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Calculate the pH of a solution prepared by dissolving 2.05g of sodium acetate, CH3COONa, in 57.0 ml of 0.10 M acetic, CH3COOH(aq) . Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x10-5

Calculate the pH of a solution prepared by dissolving 205g of sodium acetate CH3COONa in 570 ml of 010 M acetic CH3COOHaq Assume the volume change upon dissolvi class=

Respuesta :

The first step is to find the concentration of acetate in the solution, to do it, convert the given mass to moles using sodium acetate molar mass:

[tex]2.05gCH_3COONa\cdot\frac{1molCH_3COONa}{82.0343gCH_3COONa}=0.025molCH_3COONa[/tex]

Now, divide the amount of moles by the volume in liters:

[tex]\frac{0.025molCH_3COONa}{0.057L}=0.44M[/tex]

Finally use the equation of Henderson-Hasselbach to calculate the pH

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