Talking about Chromatography using kool aid, 70% isopropanol, 25% isopropanol and 5% isopropanol what is the answer to the questions?

1. Describe h0w you think the separation is occurring. What is the mechanism of the separation?

2. Why do you think the consistency of the solution added to the column was changed throughout the separation? This process is called gradient elution.

3. All chromatography systems consist of a mobile phase and a stationary phase. Define the system: what is/are the stationary phase(s), mobile phase(s), sample(s), analyte(s)?

4. Rank each colored component from least polar to most polar. Justify your ranking based on the order of elution.

Use chemfinder to find the chemical structures of the dyes. Draw the structures and justify your ranking based on their structures.

5. Many analytical procedures require a separation (chromatography) step prior to the analysis. Why?

6. This lab is a “qualitative” lab. It could easily be modified to be a “quantitative” lab. Briefly describe how you could make this a quantitative lab, i.e., how could you determine the concentration of the dyes in the Kool-Aid sample?

7. Compounds need not be colored to be analyzed using chromatography. How could colorless compounds be detected in a chromatography system?

How could you dissociate a diatomic molecule, at equilibrium, without changing the temperature of the system? [Suggested key words: equilibrium constant, concentration, ratio, volume...]

This is a P-Chem problem

The haf reaction occuring in the standard hydrogen electrode "SHE" is
2H⁺ (aq) +2e- <=> H₂ (g)

a) What is the EMF for this half-cell?
b) How is the EMF value listed in part (a) above for the standard ydrogen electrode measured?
c) Why do we need a "standard reference electrode" like this hydrogen half-cell?
d) How is SHE used to determine unknown half-cell voltages?

A 100.0 mL solution containing 0.756 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.217 M KOH. Calculate the pH of the solution after the addition of 60.0 mL of the KOH solution. Maleic acid has pKa values of 1.92 and 6.27.

At this pH (pH = 9.48), calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated H2M, HM–, and M2–, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively.

1. A loam-textured soil has from 50 to 100 square meters of surface area per gram of soil. Assume you had 100 grams of a loam-textured soil, and its S.A. was 75 m2/g. If this S.A. could be projected on one flat surface, How many football fields of area would this equal? ( Note: A football field is 120 yards long and 160 feet in width) Show your calculations.

A student starts with   4.586 g   of unknown mixture of Na₂CO₃ and CaCl₂•2H₂O. They collect   1.356 g   of precipitate. They identified Na₂CO₃ as their limiting reagent.

How many grams of CaCl₂•2H₂O did the unknown mixture originally contain?

ive tried 3.230 and 2.898 but were both wrong.

thanks

IF₅

Polar Bonds

1. Yes
2. No

Dipole Moment

1. Yes
2. No

TeBr₄

Polar Bonds

1. Yes
2. No

Dipole Moment

1. Yes
2. No

NH₂⁻

Polar Bonds

1. Yes
2. No

Dipole Moment

1. Yes
2. No

PBr₃

Polar Bonds

1. Yes
2. No

Dipole Moment

1. Yes
2. No

IO₂⁻

Polar Bonds

1. Yes
2. No

Dipole Moment

1. Yes
2. No

The following reactions are important ones in catalytic converters in automobiles. Calculate ΔG∘ for each at 298 K. Predict the effect of increasing temperature on the magnitude of ΔG∘.

A. 2CO(g)+2NO(g)→N2(g)+2CO2(g)

B. 5H2(g)+2NO(g)→2NH3(g)+2H2O(g)

C. 5H2(g)+2NO(g)→2NH3(g)+2H2O(g)

D. 2H2(g)+2NO(g)→N2(g)+2H2O(g)

E. 2NH3(g)+2O2(g)→N2O(g)+3H2O(g)

Given the following atomic weights, that the density of acetic acid is 1.05, and that 5.3 g of isoamyl alcohol, 7.6 mL of acetic acid, and 0.5 mL of sulfuric acid make 3.8 g of isoamyl acetate, what is the % yield of isoamyl acetate from its limiting reagent? Give at least two significant figures. C = 12, H = 1, O =16

Derive Clapeyron equation and Clausius modification for liquid-vapor equilibrium conditions.

When 22.0 mL of a 3.68×10-4 M silver nitrate solution is combined with 25.0 mL of a 1.80×10-5 M sodium sulfate solution does a precipitate form? (yes or no)

For these conditions the Reaction Quotient, Q, is equal to ____?

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 MKOH.

A.)Calculate the pH at 0 mL of added base.

B.)Calculate the pH at 5 mL of added base.

C.)Calculate the pH at 10 mL of added base.

D.)Calculate the pH at the equivalence point.

E.)Calculate the pH at one-half of the equivalence point.

F.)Calculate the pH at 20 mL of added base.

G.)Calculate the pH at 25 mL of added base.

Consider the following reaction between sulfur trioxide and water:

SO3(g)+H2O(l)=H2SO4(aq)

A chemist allows 61.5 g fo SO3 and 11.2 g of H2O to react. When the reaction is finished, the chemist collects 51.0g of H2SO4.

1) Determine the theoretical yield for the reaction.

2) Determine the percent yield for the reaction.