Why is the mixture of .033 M of H₂SO₃ and .033 M of NaSO₃ not good buffers?

Phosphoric acid is a triprotic acid (Ka1 = 6.9× 10–3, Ka2 = 6.2× 10–8, and Ka3 = 4.8× 10–13). To find the pH of a buffer composed of H2PO4–(aq) and HPO42–(aq), which pKa value would you use in the Henderson-Hasselbalch equation?

Calculate the pH of a buffer solution obtained by dissolving 15.0 g of KH2PO4(s) and 33.0 g of Na2HPO4(s) in water and then diluting to 1.00 L.

For each of the following, what is AE, NE, Lewis structure, VSEPR sketch, VB sketch, geometry description, and bonding description? OF2 H3O+ PCL3 H2O2 CH2O N2 CO2 O3 NO3- NO2 PCl5 SiF6 2- SF4 I3- IF5 XEF4

What mass of ammonium chloride should be added to 2.45 L of a 0.165 M NH3 in order to obtain a buffer with a pH of 9.65?

Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is described by the following thermochemical equation. 4C2H5O2N(s) + 9O2(g) → 8CO2(g) + 10H2O(l) + 2N2(g) ΔH°rxn=-3857 kj/mol. What is the energy transfer in the oxidation of 17.00g of glycine?

(¶) Provide a component diagram sketch of a typical gas chromatography instrument setup and discuss the importance of each component.

(a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City to Baltimore burned 11,800 lbs. (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of C_nH_2n+2 hydrocarbons, with n = 6 to 16, so the carbon: hydrogen ratio is close to 1:2. During this flight, how much CO₂ was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO₂ and H₂O. Give both the mass of CO₂ produced (in kg and lb) and the volume it would occupy at 298 K, 1 atm.

(b) How much CO₂ would be released into the atmosphere is those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg/L and that carbon and hydrogen dominate the composition in a ration of 1:2. The road trip is 1082 miles.

Note: This is in the complete problem as written in the textbook, in a chapter about gas laws (both ideal and nonideal).

a. What ammonia levels are considered normal in an estuarine system? What types of toxic effects can it cause? At what concentration levels?

b. What effects do fluoride ions have on finfish? At what concentrations?

An open tubular column with a diameter of 193 um and a staionary phase thickness on the inner wall of 0.52 um passes unretained solute through in 61 s. A particular solute has a retention time of 453 s.

a) What is the partition coeffecient for this solute?

b) What fraction of time does this solute spend in the stationary phase?

9. Which of the following solutions has the greatest buffering capacity?

   [A] 0.243 M HF and 0.192 M NaF

   [B] 0.485 M HF and 0.383 M NaF

   [C] 0.970 M HF and 0.766 M NaF

   [D] 0.160 M HF and 0.126 M NaF  

   [E] They are all buffer solutions and would all have the same capacity.

   10. The Henderson-Hasselbalch equation is ________

   [A] pH = pK_a + log [acid]/[base]

   [B] [H⁺] = K_a + [base]/[acid]

   [C] pH = log [acid]/[base]

   [D] pH = pK_a - log [base]/[acid]

   [E] pH = pK_a + log [base]/[acid]

7. Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid and 0.300

   mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The K_a of benzoic

   acid is 6.30 x 10^-5.

[A] 2.516 [B] 4.502 [C] 3.892 [D] 4.195 [E] 10.158

8. What change will be caused by addition of a small amount of HCl to a solution containing

fluoride ions and hydrogen fluoride?

[A] The fluoride ions will precipitate out of solution as its acid salt.

[B] The concentration of fluoride ion will decrease and the concentration of hydrogen

fluoride will increase.

[C] The concentration of hydronium ions will increase significantly

[D] The concentration of hydrogen fluoride will decrease and the concentration of

   fluoride ions will increase.

[E] The concentration of fluoride ions will increase as will the concentration of hydronium

   ions.

11. The addition of hydrofluoric acid and ________ to water produces a buffer solution

[A] HF [B] KI [C] NaF [D] NaBr [E] NaNO₃

(assume all thermodynamic quantities refer to the system, except where indicated)

Carbon dioxide sublimes at -78.5 degrees C at 1 bar pressure. When 1 mole of solid carbon dioxide is converted gas at 0 degrees C and 1 bar, which of the following quantities will be POSITIVE? CHOOSE ALL THAT APPLY: w, q, delta S, delta S_surr , delta S_total , delta G, delta H.

Consider an ionic compound, MX2 , composed of generic metal M and generic, gaseous halogen X . The enthalpy of formation of MX2 is Δ?∘f=−677 kJ/mol. The enthalpy of sublimation of M is Δ?sub=161 kJ/mol. The first and second ionization energies of M are IE1=647 kJ/mol and IE2=1377 kJ/mol. The electron affinity of X is Δ?EA=−339 kJ/mol. (Refer to the hint). The bond energy of X2 is BE=221 kJ/mol. Determine the lattice energy of MX2 . Δ?lattice= kJ/mol

I am asked to create a table of reducing potentials by setting ANY of the half-cell potential to 0V. Show calculations.

My half-cells and their Eocell is :

Ag+ + e- = Ag(s) 0.80V

Cu2+ + 2e- = Cu(s) 0.34V

Pb2+ + 2e- = Pb(s) -0.13V

Sn2+ + 2e- = Sn(s) -0.14V

Fe2+ + 2e- = Fe(s) -0.44V

Zn2+ + 2e- = Zn(s) -0.76V

Mg2+ + 2e- = Mg(s) -2.37V

Methanol (CH3OH) is made industrially in two steps from CO and H2. It is so cheap to make that it is being considered for use as a precursor to hydrocarbon fuels such as methane (CH4): Step 1. CO(g)+2H2(g)→CH3OH(l) ΔS∘ = -332J/K Step 2. CH3OH(l)→CH4(g)+1/2O2(g) ΔS∘ = 162J/K

a. Calculate an overall ΔG∘ for the formation of CH4 from CO and H2.

b. Calculate an overall ΔH∘ for the formation of CH4 from CO and H2.

c. Calculate an overall ΔS∘ for the formation of CH4 from CO and H2

d. is the overall reaction spontaneous?

e. If you were designing a production facility, would you plan on carrying out the reactions in separate steps or together?

f.