Construct the expression for Ksp for solid ZnCO 2 in aqueous solution.3ZnCO₂(s) Zn2+(aq) + CO2 (aq)Based on your knowledge of how the solid will dissociate in aqueous solution, construct theexpression for the solubility constant, Ksp. Each reaction participant must be represented byone tile.Ksp =RESET[ZnCO₂]2[ZnCO₂][ZnCO₂]²[Zn+]2[Zn+][Zn+]²[Zn2+]2[Zn2+][Zn²+]²[CO]2[CO₂][CO]²[CO2]2[CO2][CO₂2-12

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Answered: Construct the expression for Ksp for…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.ACP

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Create the Ksp expression for the dissolution of AgCl by dragging the elements and their charges, plus any exponents, to their appropriate positions.
The compound you will be investigating in this experiment is the ionic salt barium nitrate, Ba(NO3)2. (a) Write the balanced equilibrium reaction for the dissolution of barium nitrate in a satu- rated solution and the expression for the solubility product, Ksp. (b) Write the mathematical relationship between the molar solubility of barium nitrate and the concentrations of the barium ions in the saturated solution [Ba2+]eq and nitrate ions in the saturated solution [NO3–]eq. (c) Write an equation that relates the molar solubility of barium nitrate and the solubility product Ksp, similar to how Equation 3 in the Background was written for sodium chloride. (d) Consider dissolving the barium nitrate in nitric acid HNO3, a strong acid (it reacts completely with water to form hydronium and nitrate ions), instead of water. Does the nitric acid influence the barium nitrate’s solubility equilibrium? If so, how, and will this cause more or less barium nitrate to dissolve in the…
Determine the solubility product constant (Ksp) for PbCl 2 . The solubility of PbCl 2 is 0.016 mol/D at 25 degrees Celsius. What does the solubility (0.016 mol/L) represent?
Consider the following mixtures of chemicals. Complete the table by writing balanced equations and calculating the value of Q. Hence indicate whethe precipitation will occur. Mixture Balanced equation Ksp Q Precipitation occurs (yes or no) 100mL 0.5 molL-1 Ca(NO3)2 mixed with 100 mL 0.2 molL-1 Na2SO4 6.1x10-5 20 mL 0.01 molL-1 AgNO3 mixed with 80 mL 0.05 molL-1 K2CrO4 1.7x10-12
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
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.87 × 10⁻³ at a certain temperature. If 5.00 g of solid PH₃BCl₃ and 0.0700 g of BCl₃ are added to a 4.500 L reaction vessel, what will the equilibrium concentration of PH₃ be? PH₃BCl₃(s) ⇌ PH₃(g) + BCl₃(g) 1.) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms 2.) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown. 3.) Based on your ICE table, set up the expression foe Kc in order to determine the unknown. 4.) Based on your ICE table and expression for Kc, solve for the partial pressure of PH3, at equilibrium.
Write the reaction and Ksp expression for dissolving silver sulfate in water.
Choose the equilibrium constant expression for lead(II) chloride dissolving in water.a) Ksp = [Pb2+][Cl-]2/[PbCl2]b) Ksp = [Pb2+]2[Cl-]c) Ksp = [Pb2+][Cl-]d) Ksp = [Pb2+][Cl-]2
The Ksp of calcium phosphate (Ca3(PO4)2) is about 10−29. With the balanced solubility equilibrium equation of: Ca3(PO4)2(s)↽−−⇀3Ca2+(aq)+2PO3−4(aq) Write the solubility product expression for calcium phosphate. Do not include phase abbreviations for the ions in the expression.
A reaction mixture that consisted of 0.20 mol N2(g) and 0.20 mol H2(g) was introduced into a reactor of volume 25.0 L and heated. At equilibrium, 5.0% of the nitrogen gas had reacted. What is the value of the equilibrium constant KC for the reaction N2(g) + 3H2(g) ⇋ 2 NH3(g) at this temperature?
Given that CuBr would precipitate later than CuI in a solution containing equimolar concentrations of Br- and I-, it can be concluded that: A. Ksp,CuI < Ksp,CuBr B. Ksp,CuI > Ksp,CuBr C. Ksp,CuI = Ksp,CuBr D. Cannot be determined
For the vapor phase reaction 2AZ ⇄ A2 + Z2 KC = 16 at 523 K. If 0.030 mol of AZ is introduced into an evacuated 1.00 L vessel at 523 K, what is the equilibrium concentration of Z2?

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