(b) Which have a molecular dipole moment? (Select all that apply.)

CF₄

BF₃

PF₃

OF₂

F₂

Experimental Organic Chemistry 1

HPLC Questions

- What's the difference between single point calibrations and five point calibrations?

- How could you improve your resolution on a chromatograph?

- What's the difference between isocratic runs and gradient runs?

Contrast the reaction to form biodiesel with the reaction to form soap. Why do they form different products given that both reactions start out with a base and a fat or oil?

Use Slater's Rules to calculate Z* for

A. 3p electron in the element P

B. 4s electron in Co

C. 3d electron in Mn

Part A MX (Ksp = 3.97×10−36)

S = _____ M

Part B Ag2CrO4 (Ksp = 1.12×10−12) Express your answer in moles per liter.

S = _____ M

Part C Ni(OH)2 (Ksp = 5.48×10−16) Express your answer in moles per liter.

S = _____ M

A 19.57 g mixture of sugar (C12H22O11) and table salt (NaCl) is dissolved in 223 g of water. The freezing point of the solution was measured as -3.85 °C. Calculate the mass percent of sugar in the mixture. A list of Kf values can be found here.

Experimental Organic Chemistry 1

-How do you know when you should use GC or HPLC?

-What's the difference between Reverse Phase HPLC and Normal Phase HPLC?

10) . Use the principles that you learned in Part ii to calculate the standard reduction potentials for each half-cell, given that the E° for Cu2+ + 2e-  Cu (s) is 0.34 V.Note that E° for a half-reaction is not dependent on the coefficients, provided of course that the reaction is balanced, i.e., E° for Ag+ + e- Ag (s) is the same as E° for Ag+ + 2e- 2 Ag (s)

Refers to Procedures Part III Step 9

* Pb results are most unreliable

Define the followings.
(a) collision flux
(b) Stokes law
(c) Fick's second law
(d) Einstein-Smoluchowski equation
(e) half-life of a first-order reaction
(f) Forster theory of resonance energy transfer
(g) Mechaelis-Menten mechanism

Consider the titration of 40.0 mL of 0.200 M HClO4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL d. 80.0 mL b. 10.0 mL e. 100.0 mL c. 40.0 mL

answers are A) 0.699 B) 0.854 C) 1.301 D) 7.00 E) 12.15 I would just like to know how to do the work please and tbank you

A bottle filled with 0.5 L of an aqueous solution is at equilibrium with the gas containing 70 % (mole fraction) of nitrogen, N2, and 30 % of oxygen, O2. The temperature is 25 oC and the total pressure of the gas is 10 atm. The Henry’s Law constants for nitrogen and for oxygen in the solution are 6.1 × 10-4 mol L-1 atm-1 and 1.3 × 10-3 mol L-1 atm-1 .

(i) Calculate the partial pressure of oxygen and of nitrogen in the gas.

(ii) Calculate the molarity of nitrogen and oxygen dissolved in the solution.

(iii) Calculate the mass of nitrogen and the mass of oxygen released from the solution when the pressure in the gas was decreased to 1 atm at temperature 25 oC.

(iv) Calculate the volume of the gas released from the solution at pressure 1 atm and temperature 25 oC.

Iron reacts with chlorine gas according to the following balanced chemical equation:

2Fe(s)+3Cl2(g)→2FeCl3(s)

A) What mass of iron(III) chloride is produced when 101.08 g iron reacts with 185.42 g chlorine gas?

B) What is the percent yield of iron(III) chloride if 139.13 g of iron(III) chloride is actually obtained?

Using Excel, calculate a titration curve for a weak acid with a pKa of 3.57 with a
standardized NaOH solution of 0.1138 M. This curve should have a minimum of 20
calculated points; 15 before equivalence, equivalence, and 4 after equivalence. It is
STRONGLY recommended that you use the referencing features within excel to perform
these calculations. They may be done by hand, but will be extremely tedious! Submit
your (printed) results with an appropriately labeled figure and ALL calculations shown in
the immediately adjacent cell.

Formal concentration is 0.1000 M

Assume a 25.00 mL aliquot

Please show all work and the formulas you typed into excel

Which of the following is likely to have the greatest exothermic hydration enthalpy? A) Sr2+ B) Na+ C) Mg2+ D) Ca2+ E) K+

Which pair of aqueous solutions is given in order of increasing freezing point?

(1) 0.010m Na3PO4 < 0.030m NaCl

(2) 0.020m NaI < 0.030m glucose

(3) 0.010m CaCl2 < 0.020m KCl

(4) 0.010m Na3PO4 < 0.020m Na3PO4

(5) 0.020m glucose < 0.010m CaCl2