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.

1.921 g of the weak base trimethylamine, (CH₃)₃N (MW = 59.11g/mol) (K_b = 6.3 x 10^-5), is diluted in water to give 50.0 mL of solution. This solution is titrated with 0.10 M HCl. (assume all solutions at 25⁰C)

(a) What is the pH of the original amine solution?

(b) What is the pH of the solution after 162.5 ml of HCl is titrated?

(c) What is the pH after 325ml of HCl is titrated?

a. Calculate the moles of H2 produced from each trial

b. Vol of gas was not at standard temp and pressure. Convert the volume at the pressure and temperature of the experiment to a volume at standard temperature and pressure. (STP = 273. 15K, P = 1.00atm)

c. Using your answers from part a and b, calculate the molar volume of H2(g) (L/mol) at STP for each trial.

(For what ever reason, I am only able to put in a good value for mols of H2 into the computer, it keeps saying my calculations are incorrect for the rest. Trying to figure out what I am doing wrong)

h nmr for 2,4-Dimethoxybenzoicacid

Balance the equations or write the balanced chemical for the following:
A) C7H8O2(l) + O2(g) → CO2(g) + H2O(g)
B) Copper(II) hydroxide decomposes into copper(II) oxide and water when heated;
C) Solid calcium carbide, reacts with water to form an aqueous solution of calcium hydroxide and acetylene gas, C2H2.
D) As2O3(s) + NO3-(aq) → H3AsO4(aq) + N2O3(aq)

Calculate the equilibrium constant K of the reaction Sn(s)|Sn²⁺(aq)||Ag⁺(aq)|Ag(s) at 25 °C.