Please help me, stuck on this a2 chem question!!!
At 25 °C, the acid dissociation constant Ka for ethanoic acid has the value 1.75 × 10–5 mol dm–3.
(c) (i) Calculate the pH of the solution formed when 10.0 cm3 of 0.154 mol dm–3 potassiumhydroxide are added to 20.0 cm3 of 0.154 mol dm–3 ethanoic acid at 25 °C.(4 marks)
(c) (i) Calculate the pH of the solution formed when 10.0 cm3 of 0.154 mol dm–3 potassiumhydroxide are added to 20.0 cm3 of 0.154 mol dm–3 ethanoic acid at 25 °C.(4 marks)
Original post by chhhhelsie
not sure but thats how i would do it. Is answer wrong or right?
It's much easier than that.
After reaction moles of acid = moles of salt
Therefore pH = pKa = 4.75
Original post by charco
It's much easier than that.
After reaction moles of acid = moles of salt
Therefore pH = pKa = 4.75
After reaction moles of acid = moles of salt
Therefore pH = pKa = 4.75
Thanks a lot! I am glad i doubted myself
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