 Acetic Acid (HC 2 H 3 O 2 ) has 0.767% dissociation in a 0.300M solution at 25°C. Find the Ka for acetic acid at 25°C and the solution’s pH

 Acids that can give up MORE than one H + ion  Diprotic—2 H + ions capable of ionizing  Triprotic—3 H + ions capable of ionizing  **Each H + dissociates separately and in a separate step--- Specific Ka value for each step.

 Ka 1 >>> Ka 2 generally for these acids  Most of the H + dissociates in the 1 st dissociation.  **Use Ka from the 1 st dissociation to calculate [H + ] and pH

 2H 2 CO 3  H + + HCO 3 - (Ka 1 =4.3x10 -7 )  HCO 3 -  H + + CO 3 2- (Ka 2 =4.7x )

 Calculate the pH of a 0.125M maleic acid solution. HOOCCH=CHCOOH + H 2 O  H 3 O + + HOOCCH=CHCOO - (Ka = 1.2 x ) HOOCCH=CHCOO - + H 2 O  H 3 O OOCCH=CHCOO - (Ka = 4.7 x )

 Finish Weak Acid/Base Problems—Friday  Read over lab procedure