Determine the concentrations of the ionic species present in a 0.285 M solution of the HO2CCH2CO2H . (pKa1 = 2.83 , pKa2 = 5.69 ).

a) [ HO2CCH2CO2H ]

b) [ HO2CCH2CO2- ]

c)[ -O2CCH2CO2- ]

d) [H3O+]

e) [OH-]

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?

a) 2CH4(g)→C2H6(g)+H2(g)

b) 2NH3(g)→N2H4(g)+H2(g)

c) N2(g)+O2(g)→2NO(g)

d) 2KClO3(s)→2KCl(s)+3O2(g)

Can you please show equations. I am having so much trouble with these.

Having trouble calculating the error of a diluted solution in a 100mL volumetric flask. Concentration is 0.005 +/- 0.005M Amount of Concentrated solution: 5.0mL +/- 0.1mL Volumetric flask: 100mL +/- 0.08mL

My calculation so far is ((0.1/5)+(0.005/0.005)+(0.08/100))*.00025 I keep getting 0.0002552 as my error but the answer key is 0.00003. Whats wrong in my formula?

You make two dilutions. You take 82.19 mL of the stock solution (8.1×10^-5M) and dilute to 500.0 mL to make Solution #1. You then add 66.26 mL of Solution #1 to 30.11 mL of water to make Solution #2.

What is the concentration of the Solution #1 in terms of molarity?

What is the concentration of the Solution #2 in terms of molarity?

Explain why surface tension and viscosity decrease with increasing temperature.

Why do substances with high surface tensions also tend to have high viscosities?

Calculate the concentration of all species in a 0.160M solution of H2CO3.

Enter your answers numerically separated by commas. Express your answer using two significant figures.

Using an ice bath, cool 10mL of saturated sodium bisulfite solution; then add, drop by drop, 5mL of 2-pentanone. Stir the solution until there is precipitation of a solid. Add 25 mL of ethanol to encourage precipitation; then filter the crystals and wash them with 5 ml of ethanol. The product is a bisulfite addition adduct. What makes the Bisulfite product soluble in 10% NaOH but insoluble in 10% HCl. What does ethanol do to the product in this reaction? Provide a mechanism.

The mole fraction of glucose in an aqueous solution is 0.015. The density of the solution is 1.05 g/mL. Calculate the molarity and molality of the solution.

6. when choosing a solvent for recrystallization of an organic solid, what rule of thumb is generally used? What characrsitics should an ideal recrystallizing solvent have?

7. During recrystallization, why is it important to let the solution cool slowly to room temperature before cooling in ice? what would happen if the hot solution was immediatly cooled in ice?

a gas has a volume of 3.80 L. at 0 C. what final temperature, in degrees Celsius, is needed to change the vine of the gas to each of the following, if n and P do not change?

1. 1.40 L (express in 3 Sig fig) 
T1=
2. 1800 L (2 Sig fig)
T2=
3. 12.0 L (3 Sig fig)
T3=
4. 42.0 L (3 Sig fig) 
T4=

1. Calculate the pH of:

A) 0.10 M ammonia (kb = 1.7 x 10 ^-5) .

B) 0.15 M ammonium iodide (ka = 1.8 x 10 ^-5) .

C) pure water

D) 0.15 M hydrogen fluoride (ka = 4.2 x 10 ^-5) .

E) 0.25 M hydrochloric acid.

F) 0.15 M calcium hydroxide.

O2 (g) is sealed in a container at t=200k and p=43.0 bar. Using various techniques the compression factor, Z, for O2(g) in this container was determined to be 0.802

a. assuming that O2 (g) behaves as a perfect gas, calculate V_m for O₂ in this container

b. assuming that o2 (g) behaves as a van der waal's gas, calculate V_m for O₂ (g) in this container

c. use the definition of z to determine V_m for O₂ in this container.

d. compare these three calculated values of V_m and explain briefly why they are different. Which one of the 3 models is closest to the true value of V_m for O_2(g) in this container? why is your chosen model most accurate

Why do mountaineers need weeks or even months to become
acclimated before climbing summits like Mount Everest?
Write the reaction of hemoglobin (Hb) with oxygen to help you answer this question.
How does that relate to the equilibrium constant?

- A 35.0 g sample of ethylene glycol, HOCH2CH2OH is dissolved in 500 g of water. The vapor pressure of water at 32 C is 35.7 mmHg, What is the vapor pressure of the water/ethylene glycol solution at 32 C?

- What is the Boiling Point of the solution resulted from the dissolving of 32.5 g of sugar (C6H12O6) in 250.0 g of water?

- . A 1.07 mg sample of a compound was dissolved in 78.1 mg of camphor. The resulting solution melted at 176.0 C. What is the molecular mass of the compound? The melting point of pure camphor is 179.5 C. The freezing-point-depression constant for camphor Kf is 40.0 C/m.