1. Calculate the molar amount of KHP used to neutralize the NaOH solution.

2. Calculate the molar concentration of the NaOH solution that you prepared.

3. Compare the actual molarity of your NaOH solution with your goal of 0.10 M.

Equivalance point-25.3,

Measurements found in lab.

Consider three hydrocarbon compounds: ethane, CH₃CH₃; ethene, CH₂CH₂; and

            ethyne, CHCH, in all of which the two carbon atoms are bonded to each other. Of the three, ethyne has the _____________ carbon-carbon bond.

A. longest and strongest                   B. shortest and weakest

C. shortest and strongest                   D. longest and weakest

Molarity of standard NaOH solution: x/1 H 2/3 Unknown + 2/3 NaOH -> 2/3 H2O +Na 2/3 Acetate

Unknown Acid code and number of reactive hydrogens: H+3

10. Find the moles of base (NaOH) for each of your unknown acid titrations.

11. Find the balanced equation using the number of reactive hydrogens (call an acid with one reactive hydrogen HA, one with two reactive hydrogens H₂A, and so on).

12. Find the moles of unknown acid for each of your three unknown acid solutions.

13. Use the mass of unknown acid and the moles of unknown acid to find the formula mass of your unknown acid for each of your three unknown acid titrations.

Rank the relative acid strengths of the following compounds: H2O, H2S, and H2Se

___ > ___ > ___

Leachate is produced when precipitation infiltrates a sanitary landfill,

contacts the waste material, and appears at the bottom of the stored waste. Assume 6.9 kg of

benzene

(C 6 H 6 ) were placed in the landfill and it is all dissolved in the 90,000 gallons of leachate produced

during 1 year. What is the benzene concentration in the leachate during this 1 year in (a) mg/L, (b)

ppb m and (c) moles/L?

a)Calculate the equilibrium constant at 10 K for a reaction with ΔH^o = 10 kJ and ΔS^o = 100 J/K.

b) Calculate the equilibrium constant at 105 K for the thermodynamic data in the previous question.

1000 m3 of moist air at 101 kPa and 25 °C with a dew point of 11 °C enters a process. The air leaves the process at 98 kPa with a dew point of 58 °C. Assume ideal gases.

(a) Draw and label a flowsheet for the process.

b) What is the mole fraction of water in the air entering the process? Leaving the process?

(c) How many moles of water are added to or removed from the 1000 m3 of moist air?

I have had such a hard time figuring out this problem please show with detailed response! thank you

Consider the titration of a 23.0?mL sample of 0.175M CH3NH2 with 0.155M HBr. Determine each of the following.

1.the initial pH

2.the volume of added acid required to reach the equivalence point

3.the pH at 6.0mL of added acid

4.the pH at one-half of the equivalence point

5.the pH at the equivalence point

6.the pH after adding 6.0mL of acid beyond the equivalence point

A. Write the K_sp expression for the sparingly soluble compound silver phosphate, Ag₃PO₄. Ksp=?

B. Write the K_sp expression for the sparingly soluble compound barium phosphate, Ba₃(PO₄)₂. Ksp=?

C. The solubility of PbF₂ is measured and found to be 0.527 g/L. Use this information to calculate a K_sp value for lead fluoride. Ksp=?

D.The solubility of Ag₂CO₃ is measured and found to be 3.55E-2 g/L. Use this information to calculate a K_sp value for silver carbonate. ksp=?

Write the balanced chemical equation for ethanol C2H6O burning in air as a LEAN mixture if the reactant side of the reaction is C₂H₆O + ?(O₂ + 3.76N₂) ===> ? CO₂ + H2O + ? ?????

NOTE: A LEAN mixture means you have more air than you need to burn all the fuel. You will have excess oxygen left over after the reaction process.

Volumes and molarities for titration of CdC2O4 solutions.

PART A Data

Initial reading of buret (KMnO4) (mL) 0.50

Final Reading of buret (KMnO4) (mL) 14.00

Molarity of KMnO4 solution (M) 0.000969

PART B DATA

Initial Reading of buret (NH3) (mL) 1.00

Final reading reading of buret (NH3) mL 22.50

Molarity of NH3 solution (M) 5.00

FOR PART A Find:

Moles of MnO4- used for titration (mol)

Moles of C2O42- in 100.0mL of solution (mol)

Molarity of C2O42-(M)

Molarity of Cd2+ (M)

Ksp of CdC2O4

For PART B Find:

Total Moles of C2O42-

Molarity of C2O42- (M)

Total moles of Cd2+ (mol)

Moles of [Cd(NH3)4 2+] (mol)

Molarity of [Cd(NH3)4 2+] (M)

Moles of NH3 added by titration (mol)

Moles of NH3 that did not react with Cd2+ (mol)

Molarity of NH3 that did not react with Cd2+ (M)

Kf for [Cd(NH3)4 2+]

Gold is isolated from rocks by reaction with aqueous cyanide, CN-: 4 Au(s) + 8NaCN(aq)+O2(g)+H20(l)-> 4Na[Au(CN)2](aq)+4NaOH(aq). (a)Which atoms from which compounds are being oxidized, and which atoms from which compounds are being reduced? (b) The[Au(CN)2]- ion can be converted back to Au(0) by reaction with Zn(s) powder. Write a balanced chemical equation for this reaction. (c) How many liters of a 0.200 M sodium cyanide solution would be needed to react with 40.0kg of rocks that contain 2.00% by mass of gold?

Draw a log modulus–temperature plot for an amorphous polymer. What are the five regions of viscoelasticity, and where do they fit? To which regions do the following belong at room temperature: chewing gum, rubber bands, Plexiglas®?

1. A state has an energy  = 76.5×10−21 J and a degeneracy of 15. What is the free energyof the state at 25◦C and at 150◦C? Express your answer in kJ/mol.

2. A molecule has a bond that can rotate between the cis and trans states, both of whichhave zero entropy. It is found that the trans state is three times more common than thecis state when the temperature is 250 K. If the molecule is heated to 450 K, what is thenew ratio of trans to cis?

3. A system consists of two independent subsystems, A and B. Subsystem A has 1.3 × 106
allowed microstates and subsystem B has 4.6 × 107 allowed microstates. What is theentropy of the combined system?

4. Macrostate X consists of 5 microstates, each of which have an energy of x = 1.5×10−21
Joules. Macrostate Y consists of 150 microstates, each of which have an energy y =7.0 × 10−21 J. Calculate probability that the system is in state X if the temperature is25◦C.

5. A molecular system at room temperature (25◦C) is found with energy EA 95% of thetime and with energy EB 5% of the time. It is known that state A consists of an ensembleof 3 microstates while there are only 2 microstates in state B. Determine the differencein energies between the two states (EA − EB).

6. Chemical reactions are often described using a three state modelReactants → Transition State → ProductsIn most cases the energy of the transition state is much higher than the energy of the
reactant state. This means that the reaction cannot proceed until there is a randomthermal fluctuation large enough to ‘kick’ the reactant molecule(s) up to the transitionstate energy. Say we have a reaction in which the transition state is 9.0 × 10−20 J abovethe reactant state.
(a) Calculate the ratio of the probability the system is in the transition state to the probability that it is in the reactant state PTS/PR at 37◦C.

(b) Use your answer above to estimate the time it takes for the reaction to occurspontaneously at 37◦C. Assume that the system samples a new microstate everynanosecond (10−9 s).

(c) One way to speed up the reaction is to heat the system. If the temperature isincreased to 1000 K, how long does it take for the reaction to occur?

(d) In biological systems it is not feasible to accelerate reactions by heating them to1000 K. Instead, the reactions rely on enzymes that catalyze reactions by loweringthe energy of the transition state. If catalyzed reaction has a transition state energy2.0 × 10−20 J, what is the approximate reaction time? Use a temperature 37◦C.
1

(e) Finally, estimate the uncatalyzed reaction time if the transition state is not a uniquemicrostate, but actually an ensemble of 100 microstates. Use a temperature 37◦C.

7. A salt ion is dissolved in a large volume of pure water. The wall of the container has asingle defect that can bind the ion with an energy bound = −2.1 × 10−19 J.

(a) If the ion is only bound to the impurity site 2% of the time at room temperature(25◦C), what is the free energy of the ion in the unbound state? Assume that thefree energy of the bound state is equal to the binding energy (the state is non-degenerate).

(b) Calorimetry experiments reveal that the energy of the ion in the unbound state issolv = −5.1 × 10−20 J. Is the change in energy bigger or smaller than kBT at roomtemperature? [i.e. calculate (solv − bound)/kBT]

(c) What is the entropy of the unbound state?

(d) How many microstates are in the unbound ensemble?