The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting concentrations of reactants and/or products are known. A. Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used make the refrigerant carbon tetraflu CF4CF4 via the reaction 2COF2(g)=CO2(g) +CF4(g), Kc-7_ If only COF2 is present initially at a concentration of 2.00 M, what

The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting concentrations of reactants and/or products are known. A. Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used make the refrigerant carbon tetraflu CF4CF4 via the reaction 2COF2(g)=CO2(g) +CF4(g), Kc-7_ If only COF2 is present initially at a concentration of 2.00 M, what

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 37P

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.
What are the main equilibria involved in the CO2–Carbonate system and what kind of equilibrium constant is associated with each (K?)? What is the overall reaction for carbonate species in water that is exposed to the atmosphere and carbonate minerals?
The KspKsp of a salt corresponds to a reaction with the following general format: salt(s)⇌mcation(aq)+nanion(aq)where mm and nn are the coefficients that balance the equation. Equilibrium constants follow the general format of products over reactants (excluding pure liquids and solids) with each species raised to the power of its coefficient in the balanced equation. KspKsp is no exception, so Ksp=[cation]m[anion]nKsp=[cation]m[anion]n Part A If 500.0 mLmL of 0.10 mol L−1 Ca2+mol L−1 Ca2+ is mixed with 500.0 mLmL of 0.10 mol L−1 SO42−mol L−1 SO42−, what mass of calcium sulfate will precipitate? KspKsp for CaSO4CaSO4 is 2.40× 10−52.40×10−5. Express your answer to three significant figures and include the appropriate units
TypeFormulaKsp Solubility Product Constants (Ksp at 25 oC) TypeFormulaKspBromidesPbBr26.3 × 10-6AgBr3.3 × 10-13CarbonatesBaCO38.1 × 10-9CaCO33.8 × 10-9CoCO38.0 × 10-13CuCO32.5 × 10-10FeCO33.5 × 10-11PbCO31.5 × 10-13MgCO34.0 × 10-5MnCO31.8 × 10-11NiCO36.6 × 10-9Ag2CO38.1 × 10-12ZnCO31.5 × 10-11ChloridesPbCl21.7 × 10-5AgCl1.8 × 10-10ChromatesBaCrO42.0 × 10-10CaCrO47.1 × 10-4PbCrO41.8 × 10-14Ag2CrO49.0 × 10-12CyanidesNi(CN)23.0 × 10-23AgCN1.2 × 10-16Zn(CN)28.0 × 10-12FluoridesBaF21.7 × 10-6CaF23.9 × 10-11PbF23.7 × 10-8MgF26.4 × 10-9HydroxidesAgOH2.0 × 10-8Al(OH)31.9 × 10-33Ca(OH)27.9 × 10-6Cr(OH)36.7 × 10-31Co(OH)22.5 × 10-16Cu(OH)21.6 × 10-19Fe(OH)27.9 × 10-15Fe(OH)36.3 × 10-38Pb(OH)22.8 × 10-16Mg(OH)21.5 × 10-11Mn(OH)24.6 × 10-14Ni(OH)22.8 × 10-16Zn(OH)24.5 × 10-17IodidesPbI28.7 × 10-9AgI1.5 × 10-16OxalatesBaC2O41.1 × 10-7CaC2O42.3 × 10-9MgC2O48.6 × 10-5PhosphatesAlPO41.3 × 10-20Ba3(PO4)21.3 × 10-29Ca3(PO4)21.0 × 10-25CrPO42.4 × 10-23Pb3(PO4)23.0 × 10-44Ag3PO41.3 × 10-20Zn3(PO4)29.1 ×…
A gaseous mixture of 10.0 volumes of CO₂, 1.00 volume of unreacted O₂, and 50.0 volumes of unreacted N₂ leaves an engine at 4.0 atm and 800. K. Assuming that the mixture reachesequilibrium, what are (a) the partial pressure and (b) the concen-tration (in picograms per liter, pg/L) of CO in this exhaust gas?2CO₂(g)⇌2CO(g)+ O₂(g).Kp=1.4x10-28 at 800. K(The actual concentration of CO in exhaust gas is much higherbecause the gases do not reach equilibrium in the short transittime through the engine and exhaust system.)
(a) If the molar solubility of Tl2S at 25 oC is 5.31e-08 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = (c) The Ksp of BaCO3 at 25 oC is 2.58e-09. What is the molar solubility of BaCO3? solubility = ____ mol/L
Solid silver chromate is added to pure water at 25 °C, and some of the solid remains undissolved. The mixture is stirred forseveral days to ensure that equilibrium is achieved between the undissolved Ag2CrO4(s) and the solution. Analysis of theequilibrated solution shows that its silver ion concentration is 1.3 x 10-4 M. Assuming that the Ag2CrO4 solution is saturatedand that there are no other important equilibria involving Ag+ or CrO42 - ions in the solution, calculate Ksp for this compound.
For the reactionH2(g) + CO2(g) ↔ H2O(g) + CO(g)At 700oC, Kc = 0.534. Calculate the concentration of H2 that are present at equilibrium if amixture of 0.300 mol of CO and 0.300 mole of H2O is heated to 700oC in a 10.0L container.
What concentration of SO2−3 is in equilibrium with Ag2SO3(s) and 9.10×10^−3 M Ag+? The ?spKsp of Ag2SO3Ag2SO3 can be found in this table. [SO2−3]= M
Some sulfuric acid is spilled on a lab bench. You can neutralizethe acid by sprinkling sodium bicarbonate on it and thenmopping up the resulting solution. The sodium bicarbonatereacts with sulfuric acid according to:2 NaHCO3(s) + H2SO4(aq)----->Na2SO4(aq) + 2 H2O(l)+ 2 CO2(g)Sodium bicarbonate is added until the fizzing due to the formationof CO2(g) stops. If 27 mL of 6.0 M H2SO4 was spilled,what is the minimum mass of NaHCO3 that must be addedto the spill to neutralize the acid?
For the equilibriumPH3BCl3(s) ⇌ PH3(g) + BCl3(g)Kp = 0.052 at 60 °C. (a) Calculate Kc. (b) After 3.00 g ofsolid PH3BCl3 is added to a closed 1.500-L vessel at 60 °C,the vessel is charged with 0.0500 g of BCl3(g). What is theequilibrium concentration of PH3?
The constant equilibrium (Kp) of a certain reaction between gases was found to be 34.67 at 29 oK . what could be the its equilbrium based on its Kc? A2 + 3B ⇔ A2B3