Buffer capacity is a measure of a buffer solution\'s resistance to changes in pH as strong acid or base is added. Suppose that you have 125 mL of a buffer that is 0.400 M in both propanoic acid (C2H5COOH) and its conjugate base (C2H5COO–). Calculate the maximum volume of 0.290 M HCl that can be added to the buffer before its buffering capacity is lost.

1. In oxidation of borneol to camphor why do we add Sodium bicarbonate??    what role it plays?? what do we want to get rid of??   what chemical reaction takes place??

2. In oxidation of borneol to camphor why do we add Sodium bisulfite??    what role it plays?? what do we want to get rid of??     what chemical reaction takes place??

Please answer my questions. 2 questions Thanks.

Using the mechanical EOS given in your book, calculate the critical compressibility Zc = PcV c RTc for (a) the van der Waals equation, (b) the Soave equation, and (c) the Peng–Robinson equation. (d) Discuss the relative accuracy of each equation in relation to real fluids by comparing to the critical compressibilities for methane, n-butane, n-octane, methanol and water.

In this problem you will be calculating enthalpy changesforN2 . Do not assume constant values of heat capacity. Use a reference state o fT = 25 ̊C and 1 atm pressureto set H = 0 kJ/mol.

a.What is the change in enthalpy thereference state to400 ̊C?

b.What is the change in enthalpy from 800 ̊C to 400 ̊C? In addition, what is the value for enthalpyat 800 ̊C?

c.If the reference state for N2was changed to 100 ̊C, would your answer for part (b) change? If so, what would the change be?

Can you please differentiate the Antoine Equation with respect to temperature? ie dPsat/dT

1. One of the common fertilizer used to enrich soil with phosphate is

superphosphate, CaH4(PO4)2. Typically, superphosphate is produced by reacting some form of phosphate rock with sulfuric acid. In one preparation, calcium phosphate is reacted with sulfuric acid according to the reaction Ca3(PO4)2 +2H2SO4  CaH4(PO4)2 + 2CaSO4

20,000 kg/day of raw calcium phosphate containing 14wt% inert impurities is reacted with 15,000 kg/day of 92wt% H2SO4 in water. 95% of the limiting reactant is converted. The molecular weight of Ca3(PO4)2 and H2SO4 are 310 and 98, respectively
a) What is the limiting reactant? Show your work
b) What are the flow rates (in kmol/day) of the exiting species

Prepare a recipe for an inorganic medium to be used in a laboratory CSTR to grow 500 mg VSS/d of bacteria biomass, assuming that the composition of the biomass is as listed below. Determine the concentration of essential inorganic compounds required for a feed rate of 1 L/d. Assume that phosphorus is added as KH2PO4, sulfur as Na2SO4, nitrogen as NH4Cl, and other cations associated with chloride.   Note: assume that 90% of the biomass (sludge) is organic, i.e., VSS = 0.90·TSS

1.) Saturated liquid water flowing at 3kg/s is initialy at 30 bar.

a.) this steam is throttled through a valve to 9 bar. What is the vapor fraction of the steam after the valve?

b.) afterwards, 6.0 MW is added to the steam. What is the final temperature of the steam?

What is the entropy change for this heating, in kW/K?

C4H10 ↔ C2H4 + C2H6 at 700K

For the products of the reaction, compute the change in enthalpy from 298K to 700K

In Athens, GA, which is ≈ 600 ft above sea level, the average barometric pressure is 29.8 inches of mercury. Choose all of the places from this list that would have a barometric pressure lower than the average barometric pressure in Athens, GA.

The choices are: A. A hot¸sunny day on the beach in Daytona¸Florida,B.In Death Valley on a clear¸sunny day,C.In the eye of a hurricane,D.n the center of a tornado, E. Inside the face mask of a scuba diver 100 feet below the Atlantic Ocean's surface

definition and purpose of the term 'soluble reaction phosphorus "?what is its purpose? How to get it?

Comprehensive thermochemical problem: Consider an electrochemical cell with the following half- cells: Pb2+(aq)(0.01 M)/Pb(s) and Sn2+(aq)(2M)/Sn(s) at 25 °C.

a. Find the potential of the cell.

b.Determine the oxidizing agent and reducing agent.

c. Calculate the standard free energy change for the reaction.
d. Find the free energy change for the cell under the current conditions.
e. Determine the equilibrium concentrations of the solutions.
f. Use ΔH°f data to determine ΔH°rxn. ΔH°f (Sn2+ (aq)) = -8.8 kJ/mol ΔH°f (Pb2+ (aq)) = 1.6 kJ/mol

g. Calculate K at 50 °C.

h. Determine the equilibrium concentrations at 50 °C.
i. Calculate the standard change in molar entropy for the reaction from values you determined in the previous problems.

A haze droplet is activated to form a cloud droplet when the ambient saturation ratio exceeds the critical value S* and the droplet radius exceeds r*. At this point the original condensation nucelous may be assumed to be completely dissolved in the droplet. Prove that, for a given hygroscopic material and a fixed temperature, the concentration of the solution when r=r* is stronger for small condensation nuclei than for large ones. Evaluate the concentration, in units of mass of salt per unit mass of water, for sodium chloride nuclei ranging from 10^-19 to 10^-14g.

Consider a mixture of 30% n-butane, 35% n-hexane, 35% n-heptane. If the pressure is 202 kPa, calculate the bubble point temperature in ?C and the unknown mole fractions. Specify whether the unknown mole fractions are vapor or liquid. .