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Having some problems with the following question:

Trimethylacetic acid [tex]C_4 H_{11} COOH[/tex]is a weak monoprotic acid. When 0.0010 mol of Trimethylacetic acid was dissolved in 100mL of water, the concentration of trimethylacetic ion was found to be [tex]3.0 \times 10^{ - 4} mol.L^{ - 1} [/tex]

a) What is monoprotic acid?

An Acid that donates only one proton.

b) Use the above data to work out [tex]pK_a [/tex] for Trimethylacetic acid.

now pKa = -log[Ka] think? How would I go about working Ka out?

c) What volume of 0.2M KOH would be required to neutralise this solution of trimethylacetic acid?

For this I would just work out how many moles are in the 100mL solution, and then use that to work out how how much volume of KOH I would need to add.

However I'm unsure how to work out how many mols are in the 100mL solution, It's an easy units conversion problem im sure, but I suck at it :(

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# Acid concentration Q's

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