When solid barium fluoride is in equilibrium with its ions, the ratio of fluoride ion to barium ion is which of the following? 3:2 2:3 1:1 2:1 1:2

Tell what will happen to each equilibrium concentration in the following when the indicated stress is applied and a new equilibrium position is established. a. LiOH(s)+CO2(g)LiHCO3(s)+heat; CO2 is removed. b. 2NaHCO3(s)+heatNa2O(s)+2CO2(g)+H2O(g); The system is cooled. c. CaCO3(s)+heatCaO(s)+CO2(g); The system is cooled.

For the equilibrium reaction in Question 4, write the expression for the equilibrium constant. (a) How would this equilibrium constant change if the total pressure on the system were doubled? (b) How would the equilibrium constant change if the temperature were increased?

Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.

. When the volume of a vessel containing a gaseous equilibrium system is decreased, the _________ of the gaseous substances present is initially increased.

. For the reaction N2(g)+3H2(g)2NH3(g), list the types of bonds that must be broken and the type of bonds that must form for the chemical reaction to take place.

12.19 For each of the following equations, write the equilibrium expression for the reverse reaction. 2C(s) + O,(g)^2CO(g) AgCl(s)5=BAg+(aq) + Cr

Even though barium is toxic, a suspension of barium sulphate is administered to patients who need x rays of the gastrointestinal tract. The barium milkshake is safe to drink because the solubility of barium sulfate is so low. Calculate the solubility of barium sulfate in grams per liter using the data in Table 14.4.

Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.

Solubility and Solubility Product You put 0.10-mol samples of KNO3, (NH4)2S, K2S, MnS, AgCl, and BaSO4 into separate flasks and add 1.0 L of water to each one. Then you stir the solutions for 5 minutes at room temperature. Assume that you have 1.0 L of solution in each case. a Are there any beakers where you would observe solid still present? How do you know? b Can you calculate the potassium ion concentration, K+, for the solutions of KNO3 and K2S? If so, do the calculations, and then compare these K+ concentrations. c For the solutions of (NH4)2S, K2S, and MnS, how do the concentrations of sulfide ion, S2, compare? (You dont need to calculate an answer at this point; just provide a rough comparison.) Be sure to justify your answer. d Are there any cases where you need more information to calculate the sulfide-ion concentration for the solutions of (NH4)2S, K2S, and MnS from part c? If so, what additional information do you need? e Consider all of the solutions listed at the beginning of this problem. For which ones do you need more information than is given in the question to determine the concentrations of the ions present? Where can you find this information? f How is the solubility of an ionic compound related to the concentrations of the ions of the dissolved compound in solution?