chemistry buffer question

A chemist needs Ph 4 of a buffer solution of HNO2 and NaNO2, Ka for HNO2 = 4x10^-4, conc for both are 0.25 moldm-3, what volumes would you use for both in a 250cm3 buffer?

Got this question on a past paper and just cant figure it out...

(answer is 200cm3 NaNO2, 50cm3 HNO2)

How do you get ka / [H+]? ahh exams tmr super stressed also cheers for your help

What exam board is this??? Please not AQA...

i get everything apart from the rearranging.. If you have the normal equation, then do ka x [HA], you get:

[H+] x [A-] = ka x [HA]

Then how do you get [A-] / [HA]??

A chemist needs Ph 4 of a buffer solution of HNO2 and NaNO2, Ka for HNO2 = 4x10^-4, conc for both are 0.25 moldm-3, what volumes would you use for both in a 250cm3 buffer?

Got this question on a past paper and just cant figure it out...

(answer is 200cm3 NaNO2, 50cm3 HNO2)

I understand how you work out the ratio of NO2- concentration and HNO2 concentration using your ka and H+ concentration. But, why do you divide the 250cm3 by 5? Isn't five parts the total concentration so why would you divide the volume by the total concentration?!
This is so mathsy its so confusingggg I thought you have to work out moles since they gave cocentration to then work out volume.

So you just need to work out the ratio of moles of each needed in the buffer.

ka = [H+][A-]/[HA]

ka/[H+] = [A-]/[HA]

this means salt/weak acid ratio

pH 4: [H+] = 1 x 10^-4
ka = 4 x 10^-4

hence ka/[H+] = 4 = [A-]/[HA] = [salt] /[weak acid]

so the salt concentration has to be 4 x the weak acid concentration. As the two solutions are the same concentration then you have to mix four volumes of salt with 1 volume of acid.