Part A
How many moles of HF (Ka=6.8

A 83.0 mL sample of 0.0200 M HIO4 is titrated with 0.0400 M CsOH solution. Calculate the pH after the following volumes of base have been added. (

a) 11.6 mL

pH =

(b) 40.7 mL

pH =

(c) 41.5 mL

pH =

(d) 43.6 mL

pH =

(e) 75.5 mL

pH =

Calculate the pH at the equivalence point in titrating 0.045 M solutions of each of the following with 0.061 M NaOH.

(a) hydrochloric acid (HCl) pH =

(b) acetic acid (HC2H3O2), Ka = 1.8e-05 pH =

(c) hypoiodous acid (HIO), Ka = 2.3e-11 pH =

which do you think has a greater effect on evaporation
rate: molar mass or the type of intermolecular force(s) present? Explain your answer

1. Colligative Properties:

What are the four colligative properties (module #4 pg 38)?

If you add NaCl to water, what happens to the boiling point?

Explain with a drawing why the freezing point of seawater is lower than the freezing point of freshwater

Determine the %(p/p) of CaCO3 of a 25 mg chalk sample dissolved in 25 mL water, 12.5 mL HCl 0.1 M, titrated with 8.6 mL NaOH 0.1 M.

which compound the greatest lattice energy?

AIP vs AIN

KCl vs KBr

NaCl vs NaBr

MgO vs MgS

NaCl vs KCL

Considering the ionic equilibrium of your artificial kidney stone, how could you manipulate the chemical environment to decrease the solubility of your stone? What would be the effect of the solubility of your kidney stones if you utilized a strong acid/base versus a weak acid/base?

The kidney stone my group and I used was a calcium phosphate stone.

Iodine-137 decays to give xenon-137, which decays to give cesium-137. What are the modes of decay in these two reactions?

Write the molecular equation, complete ionic equation and Net ionic equation for the following:



(a) NaC₂H₃O₂ +H₂SO_{4 =}

molecular equation----

Complete Ionic equation---

Net ionic Equation-----



(b) CuSO₄ + NH₃

Molecular equation---

Complete ionic equation---

Net ionic equation-----


(c) KI + AgNO₃ =

Molecular equation

Complete ionic equation

Net ionic equation


(d) KI + AgNO₃ +NH₃ =

Molecualar equation-----

Complete ionic equation----

Net ionic equation-----


(e) K₂CrO₄ + Pb(NO₃)₂

Molecular equation----

Complete ionic equation----

Net ionic equation-----

Write the IUPAC name for each of the following compounds:

a. [Cr(NH₃)₅Cl]²⁺

b.   [W(NH₃)₃(H₂O)₃]²⁺

c.   [Fe(H₂O)₆]³⁺

4)Calculate the E_cell of: Al(s) + Cu²⁺(aq)(0.010M) → Al³⁺(aq)(1.0M) + Cu(s) (is this balanced?)

A. 2.06 B. 1.94 C. -2.06

5)Calculate the E^ocell for: Fe(s) + Br₂(g) →   Fe²⁺(aq) +Br^-(aq) ; is this electrolytic or voltaic?

A.-1.52V ; voltaic B.1.52V ; electrolytic C.1.52V ; voltaic D.-1.52V ; electrolytic

6)Calculate the E_cell of: Au(s) ; Au³⁺(aq) // Sn²⁺(aq) ; Sn(s)    is this electrolytic or voltaic?

A.1.64 ; electrolytic B.1.64 ; voltaic C.-1.64 ; voltaic D.-1.64 ; electrolytic

Identify the most likely transition metal M:

a)   K3[M(CN)6], in which M is a first-series transition metal and the complex has 3 unpaired electrons.

b)   [M(H2O)6]3+, in which M is a second-series transition metal and LFSE = –2.4 Do.

c)   Tetrahedral [MCl4]–, which has 5 unpaired electrons and M is a first-series transition metal.

d)   Square planar [MCl2(NH3)2], in which M is a d8 third-series transition metal.

1. Much like the CO ligands, cyanide (CN^-) ligands have IR stretching frequencies that are distinctive and therefore often particularly useful. Consult an appropriate character table, and give a reducible representation for the cyanide stretching vibrations in the square-planar tetracyanoplatinate(II) ion, Pt(CN)₄^2-.