2)

a) Describe in your own words and terms where the origin of the activation barrier comes from and what it represents in a chemical reaction. b) Given the same thermodynamic factors, consider the reaction of two small molecules or two large molecules with one another. Which pair should have the higher activation energy? Why?

Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.00

Two students are preparing 850 mL of a buffer using trimethyl-acetic acid (CH3)3COOH, and its potassium salt, potassium trimethyl-acetate (CH3)3COOK. When they make their buffer, they used .36 moles of the acid, but forgot to rwrite down how much (CH3)3COOK they added. They know the Ka of the weak acid is 9.3x10^-6.

a.) Rather than start over, they know that if they measure the pH, they can figure out how much (CH3)COOK they used. THey find that the pH=5.25. How many moles of (CH3)3COOK did they add when they made their buffer?

b.) They know that a buffer resists pH changes because it cintains a weak acid and a weak base. One of these can neutralize added strong acif (H3O^+). The other can neutralize strong base (OH^-) if it is added. Complete the statements below...each answer should be a chemical formula.

The weak acid in the buffer is________________ and it would neutralize added _______________.

The weak base in the buffer is _______________ and it would neutralize added________________.

c.) They add 160 mL of 1.6M NaOH to their buffer. Write the reaction describing what happens. Do not include any spectator ions. Also, state (Yes or No) whether all of the strong base can be neutralized.

d.) Compute the concentrations of the (CH3)3COOK and (CH3)3COOH remaining after the strong base in part c is added and the pH of the buffer.

*Please show all work. Thank you!

Calculate the molar solubility of magnesium fluoride in each of the following solutions: (MgF2 Ksp = 7.4*10^-9)
a) pure water
b) 0.010 M potassium fluoride solution
c) 0.050 M solution of magnesium nitrate
d) Why are the results of parts (a) thru (c) different?

The pKa of hypochlorous acid is 7.530. A 60.0 mL solution of 0.116 M sodium hypochlorite (NaOCl) is titrated with 0.291 M HCl. Calculate the pH of the solution:

a) after the addition of 7.18 mL of 0.291 M HCl.

I figured this one out by using henderson hasselbalch and got pH=7.90

b) after the addition of 25.2 mL of 0.291 M HCl

c) at the equivalence point with 0.291 M HCl.

I would appreciate it worked out! Thanks!

organic chemistry isolation of chlorophyll and carotenoid pigments post-lab questions:

A student made a mistake of running a TLC plate using MeOH as the eluant. Describe what the TLC plate could possibly look like. Be specific.

A scientist performed a hydrolysis reaction on trimyristin to obtain myristic acid. The student wants to confirm if the reaction worked. During the melting point measurement, a 50:50 (by weight) mixture of the starting trimyristin and the product myristic acid was found to be similar to that of trimyristin alone. According to the mixed melting point concept, this result may indicate that:

a) trimyristin was hydrolyzed to myristic acid

b) trimyristin was not hydrolyzed to myristic acid

c) trimyristin is the same as myristic acid

d) trimyristin was decomposed during the hydrolysis reaction

e) none of the above

Learning Goal:

To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid.

Sulfuric acid, H2SO4, is a strong acid. Its complete dissociation in aqueous solution is represented as

H2SO4→H++HSO4−

A HSO4− anion can dissociate further by

HSO4−⇌H++SO42−

but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as

Ka2=[H+][SO42−][HSO4−]=0.012

Part A

Calculate the concentration of H+ ions in a 0.010 mol L−1 aqueous solution of sulfuric acid.

Express your answer to three decimal places and include the appropriate units.

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Part B

Calculate the concentration of SO42− ions in a 0.010 mol L−1 aqueous solution of sulfuric acid.

Express your answer to four decimal places and include the appropriate units.

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Part C

Calculate the concentration of HSO4− ions in a 0.010 mol L−1 aqueous solution of sulfuric acid.

Express your answer to two significant figures and include the appropriate units.

if you allow your titration to go beyond a faint pink endpoint and it ends up dark pink, what affect will that have on your molarity NaOH? What affect, in any, would this have on the molarity of acid Hcl

Phosgene (carbonyl chloride), COCl2 C O C l 2 , is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g)+Cl2(g)⇌COCl2(g) C O ( g ) + C l 2 ( g ) ⇌ C O C l 2 ( g ) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 457 ∘C ∘ C . At equilibrium, the concentrations were measured and the following results obtained: Gas Partial Pressure (atm a t m ) CO C O 0.900 Cl2 C l 2 1.23 COCl2 C O C l 2 0.170 What is the equilibrium constant, Kp K p , of this reaction?

The following reaction was performed in a sealed vessel at 767 ∘C∘C :

H2(g)+I2(g)⇌2HI(g)H2(g)+I2(g)⇌2HI(g)

Initially, only H2H2 and I2I2 were present at concentrations of [H2]=3.35M[H2]=3.35M and [I2]=2.95M[I2]=2.95M . The equilibrium concentration of I2I2 is 0.0200 MM . What is the equilibrium constant, KcKc

If 3 spots on a TLC plate have the following RF’S, A=0.43, B=0.89 and C=0.53 what would be the order that the spots came off a column? What would happen if you increased the polarity of the solvent?

What are the real-world applications of Le Chatelier

The following data were collected for the reaction between hydrogen and nitric oxide at 700 C:

2H₂(g)+2NO(g) -> 2H₂O(g)+N₂(g)

a) What is the rate law for the reaction?

b) Calculate the rate constant for the reaction

c) More careful studies if the reaction show that the rate law over a wide range of concentrations of reactants should be:

rate= (k₁[NO]²[H₂])/(1+k₂[H₂])

What happens to the rate law at very high and very low hydrogen concentrations?

What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.4 bar ?

I got 0.042 and it says its wrong.