b)Draw on the axes below how the concentrations of H₂O, [Cu(H₂O)]²+, and [CuC14]²- changeupon (1) addition of the copper nitrate and (II) when equilibrium is re-established. Assume initialconcentrations of the different species are as follow: [H₂O] >> [Cu(H₂O)]²+>[CuC14]²- Label yourcurves appropriatelyConcentration (M)H₂OEnthalpy:c)Upon cooling the solution, the solution turns royal blue. What can be said about the value ofthe enthalpy Hº, and the equilibrium constant, Kc, of the reaction when cooling the solution?Select one for each:Equilibrium Constant, Kc:TimeAH° < 0IncreasesAHO=0[Cu (H₂O) 6 ] ²+(Cull 4] ²-DecreasesΔΗ° > 0Remains the same

The following equilibrium exist when [CuCl4]2- dissolved in water [CuCl4]2-+ 6H2O → Cu(H2O)6]2++…

Upon cooling the solution, the solution turns royal blue. What can be said about the value of the enthalpy Hº, and the equilibrium constant, Kc, of the reaction when cooling the solution? Select one for each: Enthalpy: Equilibrium Constant, Ke: AH° <0 Increases AH⁰ = 0 Decreases AH°> 0 Remains the same

Upon cooling the solution, the solution turns royal blue. What can be said about the value of the enthalpy Hº, and the equilibrium constant, Kc, of the reaction when cooling the solution? Select one for each: Enthalpy: Equilibrium Constant, Ke: AH° <0 Increases AH⁰ = 0 Decreases AH°> 0 Remains the same

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

A test tube contains the following chemical equilibrium: N2O4(g) + 59 kJ ⇌ 2NO2(g). You notice that the colourless contents of the test tube turn brown. Provide two realistic reasons as to why this change would occur in a laboratory setting. Support claims with evidence from course concepts
Sulfuric acid (H2SO4) is a strong acid in aqueous solution, yet the pKa of sulfuric acid is 7.6 in acetonitrile (CH3CN). Explain how this can be in terms of the relevant equilibria and the properties of the two solvents.
Mixing the chelating reagent B with Ni(II) forms the highly colored NiB22+, whose solutions obey Beer’s lawat 395 nm overa wide range. Provided the analytical concentration of the chelating reagent exceeds that of Ni(II) by a factor of 5 (or more), the cation exists, within the limits of observation, entirely in the form of the complex. Use the accompanying data to evaluate the formation constant Kf for the process Ni2++2BNiB22+
The equilibrium constant for the reaction 2CrO42(aq)+2H+(aq)Cr2O72(aq)+H2O is 31014 . What must the pH be so that the concentrations of chromate and dichromate ion are both 0.10 M?
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.
If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/L
(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
What wt of magnetite should be taken for analysis in order that after converting to a precipitate of Fe2O3.xH2O, the percentage of Fe3O4 in the sample can be found by multiplying the wt in grams of the ignited precipitate (Fe2O3) by 100.
a solution containing 6.25×10–3 M of S2– and 5.63×10–3 M of Cd2+ was prepared. CdS ⇌ Cd2+ + S2- Calculate the Qsp of the mixture (in 3 sig. figures) and In the given scenario, will a precipitate (Ksp = 3×10–28) form?
Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07
A saturated AgClAgCl solution was analyzed and found to contain 1.25 x 10-5 M Ag+AgX+ ions. Use this value to calculate the Ksp of AgCl
Calculate the solubility of BaSO4 solid in 0.0167 M Ba(NO3)2 solution, taking into account its activity.(Ksp 1.1x10-10 for BaSO4; activity coefficients for Ba++ and SO42- ions are 0.46 and 0.44, respectively)