Chapter 17:Calculating pH ChangesSupplemental InstructionIowa State UniversityLeader: KelseyCourse: Chemistry 178Instructor: VerkadeDate: 10/12/20101. Consider the following buffer:−¿H(aq)+¿←→+F(aq)¿HF(aq)¿ Why is this a buffer and what do buffers do? If a strong base is added to the buffer what will happen? If a strong acid is added to the buffer what will happen?2. Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: a) NaHCO3 titrated with NaOH, b) NH3 titrated with HCl, c) KOH titrated with HBr. (Problem 17.35 on page 760 of BLBM textbook).3. Calculate the pH when the following quantities of 0.100M NaOH solution have been added to 50.0mL of 0.100M HCl solution: a) 49.0 mL, b) 51.0mL. (Sample Exercise 17.6on page 731 of BLBM textbook).Supplemental Instruction1060 Hixson-Lied Student Success Center v 294-6624 v www.si.iastate.edu4. A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: a) 15.0 mL, b) 19.9 mL c) 20.0 mL, d) 20.1 mL, e) 35.0 mL. (Problem 17.41 on page 761 ofBLBM
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