## Chemistry (7th Edition)

1. Calculate the pKa value for carbonic acid: $pKa = -log(Ka)$ $pKa = -log( 7.9 \times 10^{- 7})$ $pKa = 6.10$ 2. Use the Henderson-Hasselbalch equation: $pH = pKa + log(\frac{[Base]}{[Acid]})$ $pH = 6.10 + log(10)$ $pH = 6.10 + 1.00 = 7.10$