Both AgCl and AgI are very sparingly soluble salts, but the solubility of AgI is much less than that of AgCl, as can be seen by their Ksp values. Suppose that a solution contains both Cl− and I− with [Cl−] = 0.046 M and [I−] = 0.047 M. If solid AgNO3 is added to 2.22 L of this mixture (so that no appreciable change in volume occurs), what is the value of [I−] when AgCl first begins to precipitate?

7. Choose the bond that is least polar (how would you do this without looking at an electronegativity chart)

a. P-F

b. C-F

c. C-Cl

d. C-Br

e. C-I

8. Using periodic trends, place the following in order of increasing ionic character.( Please explain)

Si-P, Si-Cl,Si-S

9. How do you calculate the bond order of resonance structures (Please explain.)

Using the following reduction potentials:

I₂(s) + 2e^- <---> 2I^-(aq) E⁰ = 0.535 V

I₂ (aq) +2e^- <---> 2I^-(aq) E⁰ = 0.620 V

I₃^-(aq) + 2e^- <---> 3I^-(aq) E⁰ = 0.535 V

a) Calculate the equilibrium constant for I₂(aq) + I^-(aq) <---> I₃^-(aq)

b) Calculate the equilibrium constant for I₂(s) + I^-(aq) <---> I₃^-(aq)

c) Calculate the solubility (g/L) of I₂(s) in water.

A 0.025 M solution of hydroxylamine has a pH of 9.11. What is the value of Kb for this weak base?

H2?NOH(aq)+H2O(?)?H3?NOH+(aq)+OH-(aq)

In the second row of the transition metals there are five elements that do not follow the normal orbital filling. Five - Nb, Mo, Ru, Rh, and Ag-result in a [Kr] 5s14dx configuration and Pd results in a [Kr] 4d10 configuration. Write the ground state electron configuration for the following species.

Ag

Ag+

Ru

Ru3+

Rh

Rh2+

Pd

Pd+

Pd2+

At 1 atm, how much energy is required to heat 89.0 g H 2 O ( s ) at − 24.0 ∘ C to H 2 O ( g ) at 115.0 ∘ C? Use the heat transfer constants found in this table.

q = kJ

Potassium dichromate is used in breathalyzers to measure alcohol content. The balanced chemical equation for the reaction between ethanol and potassium dichromate is given below.

3CH3CH2OH (aq) + 2K2Cr2O7 (aq) + 8H2SO4 (aq) --> 3CH3COOH (aq) + 2Cr2(SO4)3 (aq) + 2K2SO4 (aq) + 11H2O (l)

a. what is the oxidation state of Cr is Kr2Cr2O7?

b. what is the oxidation state of Cr in Cr2(SO4)3

c. Is Cr oxidized or reduced in the reaction? Explain.

Question 1.) Given the following data:

C2H2(g) + 5/2 O2(g) à2CO2(g) + H2O(l)      ΔH= -1300.kJ

C(s) + O2(g) àCO2(g)                                   ΔH= -394kJ

H2(g) + O2(g) à H2O(l)                                 ΔH= -286kJ

Use Hess’s Law to calculate ΔH for the reaction

2C(s) + H2(g) àC2H2(g)

Question 2.) Calculate ΔH° for each of the following reactions using the data for the enthalpy of

formation in the appendix.

2Na(s) + 2H2O(l)à2NaOH(aq) + H2(g

Thermophilic bacterium can convert glucose (C6H12O6) to ethanol and acetic acid .

1) Calculate the reaction enthalpy ΔrH when 1 mol of glucose is oxidized to ethanol at 80∘C.
C6H12O6(s)→2C2H5OH(l)+2CO2(g)

2) Calculate the reaction enthalpy ΔrH when 1 mol of glucose is oxidized to acetic acid at 80∘C.
2O2(g)+C6H12O6(s)→2CH3COOH(l)+2CO2(g)+2H2O(l)

For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.222 M , [Co2+]= 0.275 M , and [Cl−]= 0.309 M and the pressure of Cl2 is PCl2= 3.80 atm ?

delete

What would the limiting reagent be for the reacton between 1.33g of sodium bromide, 0.8g of i-butanol, and 2g of concentrated H2SO4?

Liquid helium at 4.2 K has a density of 0.147 g/mL. Suppose that a 3.00-L metal bottle that contains air at 99K and 3.0 atm pressure is sealed off. If we inject 130.0 mL of liquid helium and allow the entire system to warm to room temperature (25°C), what is the pressure inside the bottle?

A. What do antacids do? B. What are two bases that may be found listed on the labels of antacids? C. Write a balanced chemical reaction to show how one of the bases in part B does what you answered in part A.