If you started with an acetic acid solution of 2.0 mL of 0.84M Acetic acid and...

If you started with an acetic acid solution of 2.0 mL of 0.84M Acetic acid and shifted it with 0.2mL of 0.01M HCl (4 drops), what is the new pH?.

Initial pH
Final pH

Ka of acetic acid = 1.8 x 10^-50.3

Start by finding the equilibrium concentrations of the acetic acid solution. Calculate the Ph based on this initial concentration (initial Ph).

Calculate the moles of everything (compounds in the equilibrium AND the acid). Shift the equilibrium with the strong acid. Calculate the new molarities (new volume!). Now, re-establish the equilibrium and calculate the new Ph.

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

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