Assume all of the ionized aspirin remains in the buffer solution and all of the un-ionized aspirin goes into the ethyl acetate, what is the molarity of the aspirin in the ethyl acetate at pH 2.0 and pH 8.0?

Did the spots observed for aspirin depend on the pH for the aqueous phase? Why or why not?

Did the spots observed for 3-aminophenol depend on the pH of the aqueous phase? Why or why not?

Did the spots observed for acetaminophen depend on the pH of the aqueous phase? Why or why not?

Entropy & heat capacity: The definitions for the entropy and heat capacity are pretty similar. So, what is actually the difference between dS=dq/T and cp = dq/dT? Apply a simple and plausible example to illustrate the different nature of S and cp.

Part B) For 490.0 mL of a buffer solution that is 0.175 M in HC2H3O2 and 0.155 M in NaC2H3O2, calculate the initial pH and the final pH after adding 0.020 mol of HCl. Part C) For 490.0 mL of a buffer solution that is 0.185 M in CH3CH2NH2 and 0.165 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.020 mol of HCl.

Lithium trimers are the star-destroying material of science fiction. Consider the series of tri-atomic species Li₃, Li₃⁺, and Li₃^-. For each species, draw a Lewis dot electron diagram, predict the geometry, identify the Li-Li bond order, and identify the hybridization of the central lithium atom.

If the pH of a 1.00-in. rainfall over 1300 miles2 is 3.30, how many kilograms of sulfuric acid, H2SO4, are present, assuming that it is the only acid contributing to the pH? For sulfuric acid, Ka1 is very large and Ka2 is 0.012. Express your answer to two significant figures and include the appropriate units.

Refridgerant-134a with a flow rate of 0.12 kg/s is cooled to 40 degrees C at constant pressure in a condenser by using cooling water. Initially the refrigerant is at 1,200 kpa and 50 degrees C. Estimate the heat removed by the cooling water.

Estimate the pH of a 50 mM solution of acetic acid made up in 0.1 M K₂SO_4?

A tanker truck carrying 2.01×10³ kg of concentrated sulfuric acid solution tips over and spills its load. The sulfuric acid solution is 95.0% H₂SO₄ by mass and has a density of 1.84 g/mL. Sodium carbonate (Na₂CO₃) is used to neutralize the sulfuric acid spill. How many kilograms of sodium carbonate must be added to neutralize 2.01×10³ kg of sulfuric acid solution? Express your answer with the appropriate units.

A 35.00 mL sample of an unknown H₃PO₄solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.28 mLof NaOH solution is added. What is the concentration of the unknown H₃PO₄ solution? The neutralization reaction is H₃PO₄(aq)+3NaOH(aq)→3H₂O(l)+Na₃PO₄(aq)

How much 5.5 M NaOH must be added to 590 mL of a buffer that is 0.0195M acetic acid and 0.0250M sodium acetate to raise the pH to 5.75?

Calculate the pH of a .003 M solution of NaF, given that the Ka of HF = 6.8 x 10^-4 at 25 degrees celcius.

For the equilibrium: O2(g) + 2 F2(g)
2 OF2(g) ; Kp = 2.3 x 10–15
Which ONE of the following statements is true?
A) If the reaction mixture initially contains only OF2(g), then at equilibrium, the reaction mixture will consist of essentially only O2(g) and F2(g).
B) For this equilibrium, Kc = Kp.
C) If the reaction mixture initially contains only OF2(g), then the total pressure at equilibrium will be less than the total initial pressure.
D) If the reaction mixture initially contains only O2(g) and F2(g), then at equilibrium, the reaction mixture will consist of essentially only OF2(g).
E) If the reaction mixture initially contains only O2(g) and F2(g), then the total pressure at equilibrium will be greater than the total initial pressure.

Find the value of the equilibrium constant Kc at 460°C for the reaction-
½ H2(g) + ½ I2(g)
HI(g)
given the following data: A 4.50-mol sample of HI is placed in a 1.00-L vessel at 460°C, and the reaction system is allowed to come to equilibrium. The HI partially decomposes, forming 0.343 mol H2 at equilibrium.
A) 0.0123 B) 0.0081 C) 0.0309 D) 11.1 E) 5.69

What technique can be used to monitor the compounds that are collected from the column?

copper (II) oxide reacts with hydrogen gas to produce copper and water, what volume of H2 at 1.01 at and 225C is needed to reduce 0.446 mol of copper (II) oxide ?

A student dilutes 50 mL of a phosphoric acid-dihydrogen phosphate buffer solution to a final volume of 100 ml.

Will the pH of the buffer change noticeably? (Use Henderson -Hasselbeck conceptually )

For the same dilution above will the buffer capacity change ?

Calculations: A 50.0 mL sample of a 0.100 M phosphoric acid, H3PO4 is titrated with 0.100 M NaOH.

Identify the major chemical species present and calculate the pH at these four points (first consider the titration curve)

Given : K_a (H₃PO₄)=7.5 x10^-3, K_a(H₂PO₄^-)=6.2x10^-8, K_a(HPO₄^2-)=4.2x10^-13

^{Point 1: after 20.0 mL of NaOH is added}

^{Point 2: after 50.0 mL total of NaOH is added}

^{Point 3: after 75.0 mL total of NaOH is added}

^{Point 4: after 100.0 mL total of NaOH is added}