1). Two 20.0 mL samples, one 0.200 MKOH and the other 0.200 MCH3NH2, were titrated with 0.100 MHI. Answer each of the followingquestions regarding these two titrations.
a). What is the volume of added acid at the equivalence pointfor KOH?
b). What is the volume of added acid at the equivalence pointfor CH3NH2?
c). Predict whether the pH at the equivalence point for eachtitration will be acidic, basic, or neutral.
d). Predict which titration curve will have the lowest initialpH.
2). Potassium hydroxide is used to precipitate each of thecations from their respective solution. Determine the minimumconcentration of KOH required for precipitation to begin in eachcase.
a). 1.2×10−2M CaCl2
3). Use theHenderson–Hasselbalch equation to calculate the pH of eachsolution:
a). a solution that contains 1.31% C2H5NH2 by mass and 1.20%C2H5NH3Br by mass
b). a solution that is 11.5 g of HC2H3O2 and 11.5 g of NaC2H3O2in 150.0 mL of solution
