he following plot shows a typical titration curve for the titration of diprotic

Question

he following plot shows a typical titration curve for the titration of diprotic acid H,A -1.2 x10 K-2.1 x 10-10) with NaO1H. Given that the principal A-containing species at H:Aat the first equivalence point is HA pH Moles of A buffer region is indicated by which of these point(s) a-d in the titration curve? B) points a andc C) point b and c D) points b and d E) points e and d A) point a and b Answer: (II) Problems 34) The following equilibrium constants have been determined for oxalic acid at 25°C: K-6.1x 10 Calculate the equilibrium constant for the following reaction at the same temperature: 35) Classify each of the following species as a Brensted acid or base, or both: () H:O, ) Or,(e) Ho.(a) 36) Arrange the oxides in each of the following groups in order of increasing basicity (a) K O, Al:Os, BaO, (b) CrOs, CrO, CrnO. a) CO,, (b) H20, (c) I, (d) SO:. (e) 37) Classify each of the following species as a Lewis acid or a Lewis base: NHs, (f OH , (g) H", (h) BCl. 38) Which would be considered a stronger Lewis acid: (o) BF, or BCl, (b) Fe"or Fer? Explain. 39) What is pH values? (a) 9.0 (b) 7.00 (c)-0.30 (d) 15.18 (e) 2.63 (0 10.756 40) Consider the following reacting system: the Hs0' concentration to the correct number of significant figures for solutions with the following What combination of temperature and pressure (high or low) would maximize the yield of nitrosyl chloride (NOCI)? [Hint. AHRNOC»-51.7 kJ/molAHJ (NO) = 90.4 kJ/mol]

Explanation / Answer

Q33

buffer is given when there are conjguate base + weak acid

these are points in which pH won't change drastically, as acid is added

from th egraph, only A and C are buffer area

Q34

Ktotal = K1*K2 = (6.5*10^-2)(6.1*0^-5) = 3.96*10^-6

Q35

First, let us define Bronsted Lowry acid/base:

Bronsted Lowry acid: any species that will donate H+ (protons) in solution, and makes pH lower (i.e HCl)

Bronsted Lowry base: any species that will accept H+ (protons) in solution, and makes pH higher (NH3 will accept H+ to form NH4+)

Typically, acid/bases are shown in the left (reactants)

then,

H2O = both, since OH- and H3O + can be formed

OH- = base only

H3O+ = acid only

NH3 = base only (and might be converted to NH2-) therefore, both

NH4+ = acid

NH2- = acid

NO3- = none, stron electrolye

CO3- = base, forms HCO#

HBr = acid

HCN = acid

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