Given these two reactions below: PbCl2(s) 2 Pb2*(aq) + 2Cl(aq) Ksp = 1.17x10-5 Pb2*(aq) + 3 OH (aq) Pb(OH)3 (aq) Kform 8x1013 > %D determine the equilibrium constant for this reaction shown: PbCl2(s) + 3 OH (aq) Pb(OH)3 (aq) + 2Cl (aq) K = ? > O 4x10-11 O 2x10-17 O 7x10° O 9x108
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- Given the following equilibria, Ni2+(aq) + 2 OH–(aq) Ni(OH)2(s) K1 = 1.8 × 1015 Ni2+(aq) + 4 CN–(aq) Ni(CN)42–(aq) K2 = 2.0 × 1031 determine the equilibrium constant, Kc, for the following reaction. Ni(OH)2(s) + 4 CN–(aq) Ni(CN)42–(aq) + 2 OH–(aq) Group of answer choicesWrite the equilibrium-constant expression Kc for Cd2+(aq) + 4 Br-(aq) => [CdBr4]2-(aq).The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial concentration of the acid if the pKa of the acid 5.74? A. 0.657 M B. 0.315 M C. 0.274 M D. 0.387 M E. 0.0576 M
- You are conducting a biochemical experiment with an enzyme that has optimal activity at pH = 6.50. You decide to use carbonate (pKa1 = 6.38, pKa2 = 10.30) as the buffer to keep the pH stable throughout the enzymatic reaction. (Recall that the formula for carbonic acid is H2CO3.) You prepare a 0.4 M solution of carbonate buffer at pH = 10.50. Calculate the concentrations of the major carbonate species in your solution. Show your calculations.What is the concentration of free Ag+(aq) in a solution that is initially 0.01254 M in AgNO3 and 1.04842 M NH3? These two compounds react together to form [Ag(NH3)2]+. Kf([Ag(NH3)2]+) =1.600e7 1.023 7.484e-10 0.01254 6.250e-8In following these steps . Complete the table and provide th given chemical reactions in the qualitative analaysis of Group 3 Cations. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in thecentrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in eachcentrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid…
- An enzyme is needed to be stored in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component Ka Conjugate Base Salt PAH Benzoic acid, C6H5COOH 6.25 x 10-5 NaC6H5COO SAD Boric acid, H3BO3 5.81 x 10-7 NaH2BO3 DOH Hydrogen cyanide, HCN 6.20 X 10-10 NaCN In what buffer system (PAH, SAD, or DOH) will Phoebe store the enzyme? (show calculations and briefly explain) Write the equilibrium reaction involved in the buffer system. Calculate the amount (in mL) of the 2.00 M stock solution (pH 10.00) of the same buffer system needed to prepare 250 mL of a 0.650 M buffer pH 10.00.Your research advisor asks you to prepare a buffer solution at pH = 12.5 with capacity of about 0.100 M. Given the following solutions available (of any concentration), determine possible concentrations of the best conjugate species for this solution. Acetic acid: The pKa = 4.74; hypochlorous acid: pKa = 2.06; methylamine: pKb = 3.36.17. The Ksp for Zn3(AsO4)2 is 1.1 ×10−27. When 100 mL of 5.5 ×10−4 M Zn2+ is mixed with 50 mL of 1.2 × 10−4M AsO43−, which of the following statements is true? What is the new concentration of Zn2+? a 2.53 x 10-5M b 4.91 x 10-5M c 5.32 x 10-4M d 3.67 x 10-4M
- Four tablet samples (1.6308 g) which contain acetylsalicylic acid were dissolved in a 100 mL water/ethanol mixture. A 25-mL aliquot was obtained and titrated with standard 0.1273 N NaOH solution using a pH meter. The potentiometric data are given below. Calculate the % acetylsalicylic acid (EW=180.157 g/mol) per tablet. Prove that the active ingredient is indeed acetylsalicylic acid (pKa=3.48).What is the equilibrium constant of the following reaction at 25˚C?2AgBrO₃(s) + Li₂SO₄(aq) ⇄ Ag₂SO₄(aq) + 2LiBrO₃(aq)A general expression for Alpha values Consider a 1.64 M solution of Phtalic acid C6H4 (CO2H)2 abbreviated as H2A. Given: for C6H4 (CO2H)2 (Ka1 = 1.12 x 10-3 , Ka2 = 3.91 x 10-6 ) a) What are the species expected to be in the solution? b) Calculate the alpha values corresponding to each species at pH 6. c) Which species is predominant at pH 6, based on the alpha values? Was that predictable? d) Calculate the concentration of each species at pH=6.
