When 15.0 mL of a 8.89×10-4 M nickel(II) iodide solution is combined with 15.0 mL of a 4.50×10-5 M ammonium carbonate solution does a precipitate form? (yes or no)For these conditions the Reaction Quotient, Q, is equal to?

A 3.20-L solution of 1.25 103 M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 101 M NaCl. Calculate Q for the dissolution of PbCl2. No precipitate has formed. Is the solution supersaturated, saturated, or unsaturated?

A small quantity of a soluble salt is placed in water. Equilibrium between dissolved and undissolved salt may or may not be attained. Explain.

. K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of copper(II) hydroxide in mol/L and g/L at 25 °C.

A solution contains 0.0150 M lead(II) ion. A concentrated sodium iodide solution is added dropwise to precipitate lead iodide (assume no volume change). a At what concentration of I does precipitate start to form? b When [I] = 2.0 103 M, what is the lead-ion concentration? What percentage of the lead(II) originally present remains in solution?

Hydrogen iodide gas decomposes to hydrogen gas and iodine gas: 2HI(g)H2(g)+I2(g)To determine the equilibrium constant of the system, identical one-liter glass bulbs are filled with 3.20 g of HI and maintained at a certain temperature. Each bulb is periodically opened and analyzed for iodine formation by titration with sodium thiosulfate, Na2S2O3. I2(aq)+2S2O32(aq)S4O62(aq)+2 I(aq)It is determined that when equilibrium is reached, 37.0 mL of 0.200 M Na2S2O3 is required to titrate the iodine. What is K at the temperature of the experiment?

Silver(I) sulfate (Ksp=1.2105) is used in the electroplating of silver. A 1.0-L solution is prepared by mixing 15 g of silver nitrate with 20 g (2 significant figures) of potassium sulfate. Will a precipitate form? At what [Ag+] concentration will precipitation (if any) start?

In the chapter discussion of precipitate formation, we ran the precipitation reaction to completion and then let some of the precipitate redissolve to get back to equilibrium. To see why, redo Example 15-6, where Initial Cocentration (mol/L) Equilibrium Concentration (mol)/L [Mg2+]0 = 3.75 103 [F]0 = 6.25 102 reactstoformMgF2ymol/Mg2+ [Mg2+] = 3.75 103 y [F] = 6.25 102 2y

How would the solubility of calcium fluoride be affected by the presence of fluoride ion from another source? What is the solubility of calcium fluoride in a saturated solution of barium fluoride? How does this compare with the value of the solubility of calcium fluoride found in Example 17.4? Is this what you expect?