1) Build models for the PH₃ and PH₄⁺ species.

How do you compare the angles of H - P - H bonds in both species? If different, explain why.

How do you compare your electronic and molecular geometries?

2 )Build the models for the PH₃ and H₂S species.

How do you compare the binding angles in both species? If they are different, explain why.

How do you compare your electronic and molecular geometries?

17.27 Briefly describe the two techniques that are used for galvanic protection.

In this experiment, benzyl and dibenzyl ketone will produce tetraphenylcyclopentadienone via aldol condensation reaction.

1.) What is a condensation reaction? What is the small molecule lost in this reaction?

2.) In this reaction, all the reactants are ketone compounds. Can condensation reactions be extended to other carbonyl compounds than ketones?

3.) What is an enol? In a tautomerization equilibrium, will the enol or the keto isomer will be favored?

4.) What is the driving force for the enolization? (what causes the enolate ion to be formed?)

5.) The reaction goes through color change. Why the color change happens in this reaction and how can this information is associated with the (predicted) success of this reaction?

6.) Side Products Possibilities:. Assume that and enolized molecule of dibenzyl ketone attacks another dibenzyl ketone. Write the overall chemical reaction.

1a. When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter.
In the laboratory a general chemistry student finds that when 1.33 g of CaBr₂(s) are dissolved in 103.70 g of water, the temperature of the solution increases from 24.23 to 25.85 °C.
Based on the student's observation, calculate the enthalpy of dissolution of CaBr₂(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat of water.
ΔH_dissolution =  kJ/mol

1b. In the laboratory a general chemistry student finds that when 21.18 g of Cs₂SO₄(s) are dissolved in 112.90 g of water, the temperature of the solution drops from 24.64 to 21.92 °C.
Based on the student's observation, calculate the enthalpy of dissolution of Cs₂SO₄(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat of water.
ΔH_dissolution =  kJ/mol

This is all the information the question gives me.

how do adhesion and cohesion explain capillary action?

how does water dissolve a substance like NaCl? Draw a picture illustrating this

Choose one answer

A 400 mOsm/1 glucose solution is:

A) Hyposmotic to a 200 mM solution of KCl

B) isosmotic to a 600 mM solution of KCl

C) Isosmotic to a 0.18% solution of KCl

D) Hyperosmotic to a 200 mM solution of KCl

E) isomotic to a 200 mM solution of KCl.

Consider the reaction: NO₂ (g) + CO (g) ---> CO₂ (g) + NO (g)

The equilibrium constant is at 701 K and 895 K are 2.57 and 567 L mol^-1 s^-1 so,

A. Find the reaction order

B. Energy of Activation

C. Use part b to find the reaction rate constant at 200 ^C

Name the possible products of this reaction in the presence of ether and AlCl3: methylbenzene + 2-chlorobutane.
1. 1-ethyl-2-methylbenzene

2. 1-ethyl-3-methylbenzene

3. 1-ethyl-4-methylbenzene

What is the pH of a buffer solution that contains 0.350M pyruvic acid and 0.150M sodium pyruvate? Ka = 4.1x10^-3

Select one:

A. 4.72

B. 2.82

C. 2.02

D. 2.76

What is the pH of a 100.0mL buffer solution that contains 0.215M acetic acid and 0.255M sodium acetate after 0.055 mmol HCl is added. Assume no volume change. Ka = 1.8x10^-5.

Select one:

A. 4.61

B. 4.87

C. 5.03

D. 5.48

Calculate the change in pH after 0.010 mole HCl is added of 1L of pure water at 25 degrees Celsius? Assume no volume change.

Select one:

A. 7

B. 2

C. 5

D. 9

Calculate the change in pH of a buffer solution that originally contains 0.0500M ammonia and 0.0500M ammonium after 0.020 moles of NaOH is added to 1.0L. Assume no volume change. Kb = 1.8x10^-5 for ammonia. Hint you need pKa.

Select one:

A. 0.63

B. 0.18

C. 0.55

D. 0.37

NaHCO₃ + HCl reaction

a)From the P,V,T data calculate the ACTUAL moles of CO₂ produced in each trial

b) With your result from part a, calculate the molar mass of CO₂ for each trial.

I think I'm using the wrong pressure in my calculations when I try it. I'm not sure :(

Atomic absorption spectroscopy was used with the method of standard additions to determine the concentration of cadmium in a sample of an industrial waste stream. For the addition, 10.0 μL of a 1000.0 μg/mL Cd standard was added to 10.0 mL of the unknown solution. The results obtained are shown in the table. Absorbance Reagent blank 0.028 Sample 0.480 Sample plus addition 0.887 What is the concentration of the cadmium in the waste stream sample? c = μ g / mL Later, the analyst learned that the blank was not truly a reagent blank, but water. The absorbance of the actual reagent blank, is 0.062 . Calculate the cadmium concentration using the new information for the blank. c = μ g / mL Calculate the percent error caused by using water as the blank instead of the reagent blank. error: %

Consider the following reaction:
CO(g)+2H2(g)⇌CH3OH(g)
Kp=2.26×104 at 25 ∘C. Calculate ΔGrxn for the reaction at 25 ∘C under each of the following conditions.

A) Standard conditions

B) At equilibrium

C) PCH3OH= 1.5 atm ;
PCO=PH2= 1.5×10⁻² atm

Please make sure to display your thought process? It is imperative to be able to follow how the answer was deduced. Please be as thorough as possible. Please address all parts as they are critical to answering this question correctly:

Discuss the type of surface treatments that are applied to nanoclays in order to improve nanoclay dispersion in polymer matrices. What happens when untreated nanoclay is used to reinforce a polymer? What happens when a properly organically modified clay is used? List and discuss three techniques that are used to characterize the microstructure/nanostructure of nanoclay-filled polymers.

1. Manganese(II) (Mn²⁺) forms a complex with EDTA according to Mn²⁺ + Y^4- <-> MnY^2- with a formation constant K_f = 7.8 x 10¹³.

(a) 23.14 mL of 0.07893 M Mn²⁺ was titrated with 0.08130 M EDTA at pH 10.00. Calculate the endpoint volume for the titration.

(b) Calculate the conditional formation constant (K_f’) for Mn²⁺ at pH 10.00 where a_Y4- = 0.30.

(c) Calculate the concentration of free Mn²⁺ in solution at the endpoint of the titration at pH 10.00.

(d) Calculate the concentration of free Mn²⁺ in solution following the addition of 15.00 mL of 0.08130 M EDTA at pH 10.00.

(e) Calculate the concentration of free Mn²⁺ in solution following the addition of 25.00 mL of 0.08130 M EDTA at pH 10.00.