1. Calculate the concentration of the AgNO3 solution.

2. Use your AgNO3 concentration to determine the concentration of the KSCN titrant from your standardization titrations. (See Equation 6-1)

3. Determine the amount of excess Ag+ remaining in the filtrate of your unknown solutions:

a. Equation 6-1 shows the stoichiometry for this reaction.

Ag+ + SCN- --> AgSCN

b. Use the volume of KSCN used, along with the true concentration of KSCN you determined, to find the moles of Ag+ remaining in solution after the reaction with chloride.

c. Use the concentration of AgNO3 to determine the total moles of silver you added to the reaction.

d. The difference between the values you determined in b and c equals the total number of moles of silver that reacted with the chloride in your aliquot of unknown solution.

e. Determine and report the mass% of chloride in your unknown sample.

Okay so I have my concentration of AgNO3 buthow do I use it to find the concentration of the KSCN titrant? Also How to determine the excess amount of Ag+ remaining in the filtrate of my unknown silutions?

please write it by your own.

Analysis Based [Short Answers; ANY 2 less than 100 words]
1. The foam produced by the used of detergents, is harmful to aquatic life. Explain Why?

2. What might life be like without the ozone layer?

3. What causes Air pollution? How can we reduce air pollution

4. What are the common purification techniques for Brackish or sea Water? In this region, which is the common technique employed and why

The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into carbon dioxide and water. The overall reactions of a number of such steps for methane gas is
CH4(g)+5O2(g)+5NO(g)→CO2(g)+H2O(g)+5NO2(g)+2OH(g)
Suppose that an atmospheric chemist combines 145 mL of methane at STP, 885 mL of oxygen at STP, and 59.5 mL of NO at STP in a 1.8 −L flask. The reaction is allowed to stand for several weeks at 275 K .

If the reaction reaches 92.0% of completion (92.0% of the limiting reactant is consumed), what are the partial pressures of each of the reactants in the flask at 275 K ?

If the reaction reaches 92.0% of completion (92.0% of the limiting reactant is consumed), what are the partial pressures of each of the products in the flask at 275 K ?

What is the total pressure in the flask?

Using the set of smallest whole number coefficients to balance the redox equation

MnO₄^- + NO₂^- ---> MnO₂ + NO₃^-

in basic solution, you get

a) 2 OH^- on the right.

b) 3 OH^- on the left.

c) 1 H₂O on the right

d) 3 H₂O on the left

TLC analysis of an unknown sample using pure ethyl acetate as a developing solvent gives a single spot with an Rf value of 0.08.

A. Explain why this result doesn't guarantee that the sample is a pure compound.

B. Suggest two changes that could be made to the experiment to improve the analysis of the unkonwn sample.

(1)   What do you assume the entropy S for a perfect crystal when T = 0?

(2)   Is the S(0) still zero if the crystal is not perfect? Why?

(3)   How to calculate dS when under the constant pressure and c_p is given?

(4)   How to calculate the entropy of H₂O at 500 K?

(5)   How to calculate the entropy change for a chemical reaction if you can find the S for each chemical?

(6)   For an isolated thermodynamic system, dS ³ 0. That is, dS = 0 for a reversible process and dS > 0 for an irreversible process (spontaneous process).

A flask contains 30.5 g of oxygen gas, 45.7 g of sulfur dioxide gas and 23.9 g of fluorine gas. If the total pressure of the flask is 1.45 atm, what is the partial pressure of sulfur dioxide gas in the flask?

Integrated Rate Laws: Working with Zero Order Reactions Experiments have shown the following reaction to be zero order with a rate constant = 2.50 10-1 M/sec. A → B + 2 C If you started with [A] = 2.600 M, how many minutes until the concentration of A = 2.300 M? .02 Correct: Your answer is correct. minutes How many minutes until the concentration of C reaches equals 0.899999999999999 M? 1.73 Incorrect: Your answer is incorrect. minutes

A solution is prepared by mixing 25.0g pentane with 75.0g hexane. The density of the solution is 0.65g/mL. Determine the molarity and the molality of the solution.

*Please be as thorough as possible without skipping any steps. Thank you!

A voltaic cell has one half-cell with a Cu bar in a 1.00 M Cu2+ salt and the other half-cell with a Cd bar in the same volume of a 1.00 M Cd2+ salt.

(a) Find E o cell , ΔG o , and K. Report your answers to the correct number of significant figures.

E o cell = V

ΔG o = × 10 J

K = × 10

(b) As the cell operates, [Cd2+] increases; find E cell when [Cd2+] is 1.95 M.

E cell = V

(c) Find E cell , ΔG, and [Cu2+] at equilibrium.

E cell = V

ΔG = J

[Cu2+] = × 10 M

Using the sample in question 3, how many counts per second would be observed when the detector is 10 meters away from the sample? 5. If a 10 gram sample of a radioactive substance has a half-life of 6000 years, how much would be present after 8000 years? 6. If Nitrogen-14 absorbs an alpha particle and then emits a Hydrogen-1, what is the resulting nucleus? 7. If Au-185 emits an alpha particle, what is the nucleus formed? 8. What nucleus emits an alpha particle and forms Th-234? 9. If Th-234 emits a beta particle, what nucleus is formed? 10. If Nitrogen-14 absorbs a neutron and then emits a Hydrogen-1, what nucleus is formed

Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn, and T.

ΔH∘rxn=− 132 kJ ; ΔS∘rxn= 260 J/K ; T= 310 K

ΔH∘rxn= 132 kJ ; ΔS∘rxn=− 260 J/K ; T= 310 K

ΔH∘rxn=− 132 kJ ; ΔS∘rxn=− 260 J/K ; T= 310 K

ΔH∘rxn=− 132 kJ ; ΔS∘rxn=− 260 J/K ; T= 563 K

A. Calculate KP at 298 K for the reaction NO(g)+12O2(g)→NO2(g) assuming that ΔH∘R is constant over the interval 298-600 K.

B. Calculate KP at 486 K for this reaction assuming that ΔH∘R is constant over the interval 298-600 K.

Thank you

1. How many grams of ethylene glycol, C2H4(OH)2, are needed per kilogram of water to protect radiator fluid against freezing down to -10°C?

2. For benzene, C6H6, the freezing point constant, Kf, is 5.12 K oC/m and its normal freezing point is 5.5°C. What is the freezing point of a solution containing 100.0 g of benzene and 20.0 g of naphthalene (C10H8)?

3. When 5.0 g of an unknown substance is dissolved in 100.0 g of water, the freezing point of the solution decreases by 1.5°C. What is the molar mass of the unknown substance if the compound does not dissociate to form ions in solution?

4. If 2.00 moles of a substance is dissolved in 1.00 kg of water, the freezing point of the solution decreases by 7.44°C. Does this substance dissociate to form ions in solution? Explain why.

5. Calculate the freezing point of a 0.2 m CaCl2 aqueous solution, assuming it dissociates completely to form ions in solution.