Unit 4-5: Acids and Bases 3 Buffered Solutions. What is the pH of our 1.2M acetic acid solution if 10.0 mL of 1.0 M NaOH is added to it
{"Image DocumentName": "Unit 4-5: Acids and Bases 3Buffered Solutions. What is the pH of our 1.2M acetic acid solution if 10.0 mL of 1.0 M NaOH is added to it?", "Image ImageDescription": "CH3COOH CH3COO-(aq) + H+(aq) initial: ( )/0.260 M 0.010/0.260 M 0 M. change: - x M + x M +x M. equilibrium: x M x M x M. Ka = [CH3COO-][H+] = ( x)x = 1.8 x [CH3COOH] ( x) (assume x<<0.0385) x x x10-5 = 0 x = 5.2 x 10-4 M (x<<0.0385) pH = -log(5.2 x 10-4) = verify your assumption.", "Image XResolution": "37", "Image YResolution": "37", "Image ResolutionUnit": "Pixels/Centimeter", "Image Software": "SlidePlayer", "Image YCbCrPositioning": "Centered"}