2. A precipitate of Pbl, is formed when 5 mL of 0.012 M Pb(NO,), is added to 5 mL of 0.030 M KI.It was found experimentally that the final concentration of I in the 10 mL solution after equilibriumwas 8 x 10³Ma) How many moles of Pb?* are originally in the solution?b) How many moles of I' are originally present?c) How many moles of I´ remained in solution after equilibrium?

2. A precipitate of Pbl, is formed when 5 mL of 0.012 M Pb(NO,), is added to 5 mL of0.030 M KI. It was found experimentally that the final concentration of I in the 10 mL solution after equilibrium was 8 x 10 M a) How many moles of Pb?* are originally in the solution? b) How many moles of I' are originally present? c) How many moles of I' remained in solution after equilibrium?

2. A precipitate of Pbl, is formed when 5 mL of 0.012 M Pb(NO,), is added to 5 mL of0.030 M KI. It was found experimentally that the final concentration of I in the 10 mL solution after equilibrium was 8 x 10 M a) How many moles of Pb?* are originally in the solution? b) How many moles of I' are originally present? c) How many moles of I' remained in solution after equilibrium?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 24P

See similar textbooks

Similar questions

. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
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?
Ksp for CaSO4 at 100C is estimated to be1.6105. At 25C, 0.915 g of CaSO4 is added to one liter of water. (a) Will all the CaSO4 dissolve? (b) If the solution is heated to 100C, will all the CaSO4 dissolve?
How is the strength of an acid related to the position of its ionization equilibrium? Write the equations for the dissociation (ionization) of HCI, HNO3, and HClO4in water. Since all these acids are strong acids, what does this indicate about the basicity of the Cl-, NO3, and ClO4ions? Are aqueous solutions of NaCl, NaNO3, or NaClO4basic?
In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial concentration of N2 equal to the initial concentration of NO. Each had a concentration of 0.100 mol L-1. WTat were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L'1 ofO2, what were the equilibrium concentrations of all species?
Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
Ksp for silver chloride at 25.0C is 1.782 1010. At 35.0C, Ksp is 4.159 1010. What are H and S for the reaction?
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?