This should be an easy one for some of you, but it's difficult to me because of my lack of chemistry knowledge. This is not a homework problem, but a calculation I need to do for my research. I need to calculate the pH of a 1 Liter solution containing 0.000077 M HCl and 0.03 M Na-HCO3. (not necessary to read --->) I started with 10 mL of 25% HCl, which has a concentration of 7.7 M HCl. I diluted this in 1 Liter of water bringing the concentration of HCl down to 0.077 M. I then take 1 mL of this solution and dilute it again in 1 L bringing the concentration of HCl down to 0.000077 M. To this solution I add 2.52 grams of sodium bicarbonate. This has a concentration of 0.03 M (2.52 g) x (1 mol / 84 g) x (1/L). The pKa for bicarbonate/carbonic acid, or HCO3 / H2CO3 is 6.4. The pKa for carbonate/bicarbonate, or CO3/HCO3 is 10.3. Bicarbonate, a buffer, reacts with HCl, as follows: NaHCO3 + HCl <--> H2CO3 + NaCl If you don't want to do calculations, could you tell from just looking at the concentrations that I will have a near neutral pH? I'm growing microorganisms.