Calculate the pH of the following solutions.

0.060 M in sodium formate, NaCHO2, and 0.350 M in formic acid, HCHO2. The Ka for formic acid is 1.8x10-4

0.0575 M in pyridine, C5H5N, and 0.0720 M in pyridinium chloride, C5H5NHCl The Kb for pyradine is 1.7x10-9

I'm basically lost on both so an explanation would be helpful as well! Thanks.

pH = pKa + log([salt]/[acid])
pKa = -log(Ka) = 3.74
pH = 3.74 + log(0.06 / 0.35) = 2.98

pKb = -logKb = 8.77
pOH = pKb + log([salt]/[base])
pOH = 8.77 + log(0.072 / 0.0575) = 8.87
pH = 14 - pOH = 5.13