In Comparing Two Acids, the Stronger Acid Will Have a ______Ka and a ______Pka
Total Page：16
File Type：pdf, Size：1020Kb
SI Chem 178 Ch 17 Leader: Emily Tuesday, March 5th, 2013
Review: In comparing two acids, the stronger acid will have a ______Ka and a ______pKa.
Amines are ______and behave as such because of their______. (Think Lewis)
HX acid strength is determined by SIZE / EN
Oxyacid strength is determined by SIZE / EN and gets STRONGER / WEAKER with the addition of more oxygens.
Write the equation that relates Kb Ka and Kw. What types of problems from Ch 17 will use this?
LARGE / SMALL pH changes are observed in buffered solutions.
Write the HH equation. What situations from Ch 17 will use this?
T/F Buffer capacity is greater as the molarity of the acid/salt mixture increases. (Ex: A 1M solution of acetic acid and 1M Sodium acetate versus 0.1M Acetic acid and 0.1M Sodium acetate. What would be the same in each of these cases?)
The common ion effect is observed with STRONG/ WEAK species and it INCREASES / DECREASES % ionization of the weaker electrolyte.
New Stuff:
Define equivalence point: Is this definition the same for strong and weak acids/bases? What is the difference between the equivalence environment when titrating a strong acid versus weak acid? Why?
Circle which is constant in a neutralization reaction:
Total Volume Moles of initial species Moles of titrant Initial species volume pH Ka and Kb of acid being neutralized Species present in solution What is the solution pH if I combine 200 mL of 0.12M HCl with 150mL of 0.20M KOH?
17.34 Comparing and contrasting titrating STRONG vs WEAK acid with a STRONG base (both at the same initial concentration in solution.) (Answer with: Same, Weak is higher/lower, Strong is higher/lower) a. Quantity of base required to reach equivalence point b. pH at the beginning of titration c. pH at equivalence point d. pH after EXCESS base is added e. Choice of indicator pH range
17.43 20mL of 0.20 HBr is being titrated against 0.20M NaOH, what is the pH of the solution after the following additions of NaOH: 15.0, 19.9, 20.0, 20.1, 35.0. mL HBr mL NaOH Total Vol Moles H+ Moles Molarity pH OH- of Excess Ion
17.45 35mL of 0.15M CH3COOH (Acetic acid) is being titrated with 0.15M NaOH, calculate the pH after the following additions of NaOH (in mL): 0, 17.5, 34.5, 35.0, 35.5, 50
17.46 Titration of 30mL of 0.05M NH3 with 0.025M HCl… calculate pH after the following additions of HCl (in mL): 0, 20.0, 59.0, 60.0, 61.0, 65.0.