pH = 7 @ 25 C / 298 K 14 always!! increasing/decreasing concentrations of buffer components, but keeping the ratios constant (if you don't it'll change the buffer capacity for either acid or base respectively) pH = pKa

1.0 x 10^-14 at 25 C or 298 K solution that is resistant to a small pH change, it has to contain a weak acid or base pared with its conjugate salt(Na+, H3O-, etc...) and it creates neutral compounds, keeping pH relatively stable HA(aq) + OH- --> A-(aq) + H2O(L) if weak acid is in excess --> a buffer --> Hendeson Hasselbalch equaiton if strong base is in excess, the moles of excess hydroxide ions is used for pH if acid and base are equimolar then the equilibrium concentr if weak base is in excess --> a buffer --> Hendeson Hasselbalch equaiton if strong acid is in excess, the moles of excess acid are used to determine pH if acid and base are equimolar then the equilibrium concentrations are used to determine pH

maximum buffering capacity weak acid-strong base reaction how to increase/decrease buffering capacity pH + pOH =

weak acid-strong base reaction weak acid-strong base reaction what is a buffer in what range are buffers effective

in what range are buffers effective how to increase/decrease buffering capacity maximum buffering capacity maximum buffering capacity