Resarch project( le chatelier's principle ) Be sure to explain the Chemistry involved in this reaction or process and how this reaction relates to Technology, Society and/or the Environment. Some examples include: Haber-Bosch Process Blood Buffering add lots of pictures and details

Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?

The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction] in which each system will proceed to leach equilibrium. (a) 2NH3(g)N2(g)+3H2(g) Kc=17;[NH3]=0.20M,[N2]=1.00M,[H2]=1.00M (b) 2NH3(g)N2(g)+3H2(g) Kp=6.8104 initial pressures NH3=3.0atm,N2=2.0atm,H2=1.0atm (c) 2SO3(g)2SO2(g)+O2(g) Kc=0.230;[SO3]=0.00M,[SO2]=1.00M,[O2]=1.00M (d) 2SO3(g)2SO2(g)+O2(g) Kp=16.5 initial pressures SO3=1.00atm,SO2=1.00atm,O2=1.00atm (e) 2NO(g)+CI2(g)2NOCI(g) Kc=4.6104;[NO]=1.00M,[CI2]=1.00M,[NOCI]=0M (f) N2(g)+O2(g)2NO(g) Kp=0.050 initial pressures NO=1.00atm,N2=O2=5atm

. Under what circumstances can we compare the solubilities of two salts by directly comparing the values of their solubility products?

Aluminum ions react with the hydroxide ion to form the precipitate Al(OH)3(s), but can also react to form the soluble complex ion Al(OH)4. In terms of solubility, Al(OH)3(s) will be more soluble in very acidic solutions as well as more soluble in very basic solutions. a. Write equations for the reactions that occur to increase the solubility of Al(OH)3(s) in very acidic solutions and in very basic solutions. b. Lets study the pH dependence of the solubility of Al(OH)3(s) in more detail. Show that the solubility of Al(OH)3, as a function of [H+], obeys the equation S=[H+]3Ksp/Kw3+KKw/[H+] where S = solubility = [Al3+] + [Al(OH)4] and K is the equilibrium constant for Al(OH)3(s)+OH(aq)Al(OH)4(aq) c. The value of K is 40.0 and Ksp for Al(OH)3 is 2 1032. Plot the solubility of Al(OH)3 in the pH range 412.

What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.

Most barium compounds are very poisonous; however, barium sulfate is often administered internally as an aid in the X-ray examination of the lower intestinal tract (Figure 15.4). This use of BaSO4 is possible because of its low solubility. Calculate the molar solubility of BaSO4 and the mass of barium present in 1.00 L of water saturated with BaSO4.

Write the expression of the reaction quotient for the ionization of HOCN in water.