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Chemical equations- the Ka and Henderson Hasselbalch equation

Please help, I'm really stuck on the following:-

A weak acid has a PKa of 7.713. Calculate the pH of a solution in which the ratio of the concentrations of undissociated acid to acid anion ([HA]/[A-]) equals 8.441

also

Calculate the PKa of a weak acid given the information that a 0.652 M solution has a pH of 2.882

and

Calculate the pH of a 0.24 M solution made from a weak acid whose PKa is 4.271

Hope you can help or at least point me in the right direction.

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