In a solution that is 0.0500M in
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GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
- At 25C, 10.24 mg of Cr(OH)2 are dissolved in enough water to make 125 mL of solution. When equilibrium is established, the solution has a pH of 8.49. Estimate Ksp for Cr(OH)2.arrow_forwardCalculate the Fe3+ equilibrium concentration when 0.0888 mole of K3[Fe(CN)6] is added to a solution with 0.0.00010 M CN–.arrow_forwardGive detailed Solutionarrow_forward
- Consider the equilibrium reaction below. [Cu(H₂O)6]²+ (aq) + 4 Cl (aq) light blue 1. A test tube in 2. the to [CuC14]²+ (aq) + 6 H₂O (1) orange COWNIC is color? 14 TOT Châtelie anges to for the color? pic. Dior species diesent 3. The test tube in 2, is put into an ice bath. The solution changes to a light blue color. What is the major species present in the solution responsible for the color? b. Explain the effect of heat in terms of Le Châtelier's principle.arrow_forward[Fe(H2O)6]3+ (aq) + SCN1- ↔ Fe(H2O)5SCN]2+(aq) + heat yellow red For the above reaction, describe using Le Chatelier’s Principle what changes (color changes and shifts) would occur when each stress is applied to this equilibrium. Explain your answers. a) Add KSCN(aq) b) Decrease temperature c) Add AgNO3, which causes AgSCN to precipitate out.arrow_forwardWhat is the approximate concentration of free Cu+ ion at equilibrium when 1.91x10-2 mol copper(I) nitrate is added to 1.00 L of solution that is 1.030 M in CN. For [Cu(CN)₂], K = 1.0x1024. [Cut] = M use tine References to access important values ir needed for this question. What is the approximate concentration of free Cd2+ ion at equilibrium when 1.48x10-2 mol cadmium(II) nitrate is added to 1.00 L of solution that is 1.030 M in CN. For [Cd (CN)4]2, K₁= 6.0x10¹8. [Cd2+] = Marrow_forward
- 1.) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, or -log[Cu2+], in an aqueous solution of NaOH which has a pH of 12.45 and is saturated in Cu(OH)2. 3.) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if we were to dissolve 2.52 g of CuCl2 in 1.000 L of a solution 0.946 M in NaCN. The addition of CuCl2 does not alter the volume (the final volume is still 1.000 L).arrow_forwardAgBr has very low solubility in water. Silver ions form a complex ion with thiosulfate. Ag*(aq) + 2S2O3²"(aq}-- [Ag(S203)2]3¬(aq) If sodium thiosulfate is added to a saturated solution of AgBr in equilibrium with solid AgBr, how will the concentrations of free Ag*(aq) and Br"(aq) change? Equilibrium arrow (reaction above): Ag (aq) decreases, Br (aq) decreases Ag*(aq) decreases, Br"(aq) increases Ag"(aq) increases, Br¯(aq) decreases Ag"(aq) increases, Br (aq) increasesarrow_forwardConsider the equilibrium reaction below. [Cu(H₂O)6]²+ (aq) + 4 Cl (aq) light blue Aube cur in the solu on Jution Co [CuCl4]² (aq) + 6 H₂O (1) orange for the Color? 2. To the test tube in 1, 1 M HCl is added dropwise. The solution changes to an orange color. a. What is the major species present in the solution responsible for the color? b. Explain the effect of HC1 in terms of Le Châtelier's principle.arrow_forward
- An aqueous solution is prepared in which 0.00113 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a total volume of 1.00 L. Kf for Ni(NH3)62+ is equal to 5.5 × 108. Calculate the concentration of Ni(H2O)62+ ions at equilibrium in the solution formedarrow_forwardCalculate [Cr3+] in equilibrium with Cr(OH)4-(aq) when 0.010 mol of Cr(NO3)3 is dissolved in 1 L of solution bufered at pH 10.0.arrow_forwardChoose the best answer below. Consider the following complex ion formation equilibrium and it's equilibrium constant, Kf. Which of the following statements is FALSE? Cu2* (aq) + 4CN" (aq) Û Cu(CN)4² (aq) K = 1.0x1025 Cu2* is a Lewis acid in the reaction, and CN' is a Lewis base Removing some of the Cu2* (e.g., by precipitation) will cause some of the complex ion to dissociate O If enough CN is added, the equilibrium mixture would contain zero Cu²+ The complex ion is a Lewis acid-base adduct Adding more CN" will cause more complex ion to form ) The equilibrium lies in favor of the complex ionarrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning