(3 points) Using the dissociation constant(ka), calculate the equilibrium concentrations of Cd2+ and CN in a 0.250 M solution of Cd(CN)4². Cd2++4CNCd(CN)2 kd = 3.4 x 10-15
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- 1. If the equilibrium constant for the reaction A + 2B ↔ C + 5/2 D has a value of 4.0, what is the value of the equilibrium constant for the reaction2C + 5D ↔ 2A + 4Bat the same temperature? 2.What is the molarity of a solution that is made by dissolving 0.40 mole of NaOH in enough water to give a final volume of 250.0 mL?1) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, i.e., -log[Cu2+], in an aqueous NaOH solution that has a pH of 12.86 and is saturated with Cu(OH)2. 2) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, i.e. -log[Cu2+], if 2.46 g of CuCl2 is dissolved in 1.000 L of a 0.938 M NaCN solution. The addition of CuCl2 does not affect the volume (the final volume is always 1.000 L).Calculate the [Ag+] in a solution prepared by dissolving 1.00 g of AgNO3 and 10.0g KCN in enough water to make 1.00 L of solution. Kf[Ag(CN)2]1- = 1.0 x 1021
- For the aqueous [Ag (CN)₂] complex K=1.26 × 10²¹ at 25 °C. + Suppose equal volumes of 0.0022M AgNO3 solution and 0.48M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Agion. Round your answer to 2 significant digits. M x10 X Ś ?In aqueous solution the Ag ion forms a complex with two cyanide anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the last step in the formation of the complex. K₂ = ☐ Write the Last Step: Last Step: ☑ ロ→ロAn experiment was carried out to determine the value of the equilibrium constant, Kc for the reaction.• Total moles of Ag+ present= 3.6 x 10 -3 moles• Total moles of NH3 present = 6.9 x 10-3 moles• Measured concentration of Ag(NH3)2 + at equilibrium = 3.4 x 10-2 M• Total solution volume = 100 mLCalculate the equilibrium concentration of Ag+ and NH3(uncomplexed)
- Given that Ksp for AgCl is 1.6E-10 and Kf for Ag(CN)2- is 5.6E8, calculate the concentration of Ag+ when 0.15 M AgNO3 is reacted with 0.25 M KCN.For the aqueous [Ag (CN)₂] complex K₁=1.26 × 10²¹ at 25 °C. + Suppose equal volumes of 0.0026M AgNO3 solution and 0.38M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Agion. Round your answer to 2 significant digits. M ? ☐x10 × Ś1) The following reaction was allowed to reach equilibrium at 25oC. Enclosed with the phase of each species is the equilibrium concentration. Calculate the equilibrium constant (Kc and Kp) for this reaction. 2 NOCl(g, 2.6 M) = 2 NO(g, 1.4 M) + Cl2(g, 0.34 M) 2) Calculate the pH of a 0.10 M hypochlorous acid solution. Ka = 3.5 x 10-8.
- Calculate the equilibrium isothiocyanatoiron(III) ion concentration, [FENCS2*leg• you will report when making your standard curve. Give your answer to three decimal places. Also give your answer in millimolar (mM) (because you won't be able to enter an answer in scientific notation here). Fe(NO3)3 0.10 M HNO3 NaSCN 0.194 M 1.97 x 10-3 M initial buret reading (mL) final buret reading (mL) 0.02 0.03 0.01 1.87 0.39 7.571. It is possible to dissolve significant amounts of Mg(OH)2 in solutions in which the concentration of either Mg2+ or OH− is very, very small. Explain, using Ksp, why this is the case. 2. Explain why Mg(OH)2 might have very appreciable solubility in 1 M HCl. (Consider the effect of the equilibrium of H2O on the Mg(OH)2 solution reaction.)Calculate the concentration of ions in the following saturated solutions: (a) [I- ] in AgI solution with [Ag+ ] = 9.1 x 10-9 M ; Ksp= 8.3 x 10-17 (b) [Al3+] in Al(OH)3 solution with [OH- ] =2.9 x 10-9 M ; Ksp = 1.8 x 10-33