Construct the expression for Ksp for solid ZnCO 2 in aqueous solution. 3 ZnCO₂(s) Zn2+(aq) + CO2 (aq) Based on your knowledge of how the solid will dissociate in aqueous solution, construct the expression for the solubility constant, Ksp. Each reaction participant must be represented by one 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

Construct the expression for Ksp for solid ZnCO 2 in aqueous solution. 3 ZnCO₂(s) Zn2+(aq) + CO2 (aq) Based on your knowledge of how the solid will dissociate in aqueous solution, construct the expression for the solubility constant, Ksp. Each reaction participant must be represented by one 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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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One mixes aqueous NaCl with aqueous AgNO3. NaCl. AgNO3and NaNO3all have appreciable solubility in water. AgCl has a solubility product constant Ksp of 1.6 x 10-10. If one mixes the NaCl solution with the AgNO3solution, one would suspect: a) no precipitate will form b) AgCl precipitate will form c) NaNO3 precipitate will form d) both AgCl and NaNO3 precipitates will form
A student ran the following reaction in the laboratory at 651 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.43×102 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.115 M. Calculate the equilibrium constant, K, she obtained for this reaction. Ke =
To determine the solubility product constant of Al(OH)3 at a specific temperature, a saturated solution of Al(OH)3 at the required temperature was titrated with 0.2M HCl via the reaction: 3HCl + Al(OH)3 → AlCl3 + 3H2O. Based on the following data, determine the Ksp of Al(OH)3 at the specified temperature: Volume of Al(OH)3 titrated: Volume of 0.2M HCl required: 9.5 mL 3.44 mL Your answer should follow the format: a) mols of HCl added b) mols of Al(OH)3 c) Molarity of Al(OH)3 d) Ksp of Al(OH)3
Using the balanced equation: PCI3(s) + 3H2O(1) --> H3PO3(aq) + 3HCI(aq) How many moles of HCI would be produced from 20 grams of phosphorous trichloride?
Determine the molar solubility for Cd₂(PO) by constructing an ICE table, writing the solubility constant expression, and solving for molar solubility. The value of Ksp for Cd₂(PO) is 2.5 × 10:³³. Complete Parts 1-3 before submitting your answer. Initial (M) Change (M) Equilibrium (M) +x 1.000 + 3x Assume the solution already contains 0.500 M NPO. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 0 1 +2x 1.500 + x Cd (PO),(s) 0.500 +3x 1.500 + 2x -0.500 0.500 + x 2 1.500 + 3x 1.000 0.500 + 2x 3 Cd²+ (aq) -1.000 3 0.500 + 3x + 1.500 1.000 + x 2 PO³(aq) RESET NEXT -1.500 1.000 + 2x
The solubility product of magnesium carbonate, MgCO3 , has the value Ksp = 6 . 82 × 1 0−6 at 25 °C. How many grams of MgCO3 will dissolve in 1.00 L of water?
At 25 °C, an aqueous solution has an equilibrium concentration of 0.00217 M for a generic cation, A+(aq), and 0.00109 M for a generic anion, B2−(aq). What is the equilibrium constant, ?sp, of the generic salt A2B(s)?
A student ran the following reaction in the laboratory at 672 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 6.42×10-2 moles of NH3(g) into a 1.00 Liter container, she found the equilibrium concentration of H2(g) to be 9.09×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 281 K: 2 CH2CI2 (g) CH4 (g) + CCI4 (g) When she introduced 7.87x102 moles of CH2CI2 (g) into a 1.00 liter container, she found the equilibrium concentration of CCI4 (g) to be 3.68×102 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. K. =
a Write the equilibrium constant expression, Keq, or solubility product constant, Ksp. for each of the following reactions. a. Fe(H2O),+ (aq) + 2 OH' (aq) <→ Fe(H2O)4(OH)2 (aq) + 2 H,O (I) on of he b. Fe(H2O),* (aq) + CO32 (aq) → FECO3(s) + 6 H2O (I) Complete the reaction table below for the reaction H2 (g) +l2(g) <→ 2 HI(g) , where all the concentrations given are equilibrium concentrations in molar. Note that Keq will be a different value at each temperature. Temperature [H2] [12] [HI] Кeq 25°C 0.388 0.355 0.0922 a. 340°C b. 0.0540 0.650 9.6 445°C 0.0321 HA 0.0392 c. 50.2 s on bsbbs ai aog animosd soM mullad to 01921 i enob ai noitouen ant 91 on mont bevomsal.HO 16 i snob al noltasen sil? noiasan at chis an endothermic or exothermic reaction? Explain.
A solution contains 0.021 M Cl- and 0.017 M I. A solution containing copper (I) ions is added to selectively precipitate one of the ions. At what concentration of copper (I) ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuCl) = 1.0 × 10-6, Ksp(Cul) = 5.1 × 10-12