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- 1.For the aqueous reaction A + B à C + D, the equilibrium concentrations in moles per liter are [A] = 0.002, [B] = 0.005, [C] = 0.00004 [D] = 0.00025 i. What is the equilibrium constant Keq? ii. What is the dissociation constant pK? a. The partial pressure of gas A is 10 ppmv. It has a Henry’s constant for dissolution in water of KH = 0.02Estimate the concentrations of cadmium ion (Cd2+) at pH 1 to 14 in water using solubility product constant for cadmium hydroxide. Cadmium Hydroxide => Cd(OH)2 Kso => 7.2*10-15 Note: Please try to explain the process and write legible. Thank you!!. A solution was prepared by mixing 4.00mL of 2.00 x 10-3 M Fe(NO3)3 and 3.00mL of 5.00 x 10-3 M NaSCN and diluting the mixture with water to a total of 10.00mL. Use your average value of Kc to calculate the equilibrium concentration of FeSCN2+ in the mixture. [Hint: Use as many significant figures as you legitimately can in your calculations] my average you can find on the picture below PLS HELP ASAP!!
- The solubility product for Pb(Cl)2 is K = 1.60 * 10-5, the solubility product forPb(F)2 is K = 3.70 * 10-8 , and K for the following reaction is 1.98 * 10-4:Pb(Cl)2 (s) + 2 HF ⇌ PbF2 (s) + 2 H+ + 2Cl-Calculate the dissociation constant for H1) Write the pertinent reactions associated with the question2) Write the equilibrium constantexpression for each chemicalreaction.3) Write the mass balance equations4) Write the charge balance equation5) Count the equations andunknowns.6) SolveThe sulfur dioxide concentration in San Diego was measured at 81ppb. What is the pH of an aqueous aerosol in equilibrium with SO2 at 25°C?•KH= 1.4*10^-5 M/Pa for sulfur dioxide •Ka1= 1.6*10^-2 for H2SO3•assume HSO3- formation approximates H+ and is negligible compared to concentration of H2SO3 formedDo not use quadratic equation to solve and show all mathematical stepsA 50.00 mL volume of 0.0600M K2CrO4 is mixed with 50.00 mL 0.0800 M AgNO3. Calculate the concentration of Ag+, CrO42-, K+, and NO3- at equilibrium. The solubility product of Ag2CrO4(s) is 1.20 x 10-12. Please show work
- You are on a new planet and discover a substance, Z2O that undergoes autoionization just like water on Earth. Z2O + Z2O ⇌ Z3O+ + OZ– Through a series of experiments, you determine the equilibrium constant (Kx) for this autoionization reaction at various temperatures. The value of Keq at 26.8ºC is 6.9 x 10-14. What is the pZ of the pure substance at this temperature? (pZ = -log(Z3O+) Report your answer to the hundreths placeSolid potassium hydroxide is slowly added to 175 mL of a 0.318 M nickel(II) acetate solution until the concentration of hydroxide ion is 0.0568 M. The percent of nickel ion remaining in solution is __ % Solubility Product Constants (Ksp at 25 oC) Type Formula Ksp Bromides PbBr2 6.3 × 10-6 AgBr 3.3 × 10-13 Carbonates BaCO3 8.1 × 10-9 CaCO3 3.8 × 10-9 CoCO3 8.0 × 10-13 CuCO3 2.5 × 10-10 FeCO3 3.5 × 10-11 PbCO3 1.5 × 10-13 MgCO3 4.0 × 10-5 MnCO3 1.8 × 10-11 NiCO3 6.6 × 10-9 Ag2CO3 8.1 × 10-12 ZnCO3 1.5 × 10-11 Chlorides PbCl2 1.7 × 10-5 AgCl 1.8 × 10-10 Chromates BaCrO4 2.0 × 10-10 CaCrO4 7.1 × 10-4 PbCrO4 1.8 × 10-14 Ag2CrO4 9.0 × 10-12 Cyanides Ni(CN)2 3.0 × 10-23 AgCN 1.2 × 10-16 Zn(CN)2 8.0 × 10-12 Fluorides BaF2 1.7 × 10-6 CaF2 3.9 × 10-11 PbF2 3.7 × 10-8 MgF2 6.4 × 10-9 Hydroxides AgOH 2.0 × 10-8 Al(OH)3 1.9 × 10-33 Ca(OH)2 7.9 × 10-6 Cr(OH)3 6.7 × 10-31 Co(OH)2 2.5 ×…Magnesium fluoride (MgF2, MW = 62.30 g/mol) is slightly soluble in water, with Ksp = 7.4 x 10^-11 at T= 25. C.a) Give the correctly balanced solubility reaction and expression for Ksp for MgF2.b) What mass of magnesium fluoride will dissolve in 1.000 L of pure water?
- Solid copper(Il) acetate is slowly added to 50.0 mL of a 0.0631 M ammonium sulfide solution. The concentration of copper(Il) ion required to just initiate precipitation is ______ M. (Assume that Ksp (CuS) = 7.9 × 10^-37 .) The Solubility Product Constant for iron(Il) hydroxide is 7.9 × 10^-15 Solid potassium hydroxide is slowly added to 125 mL of a 0.0509 M iron(Il) nitrate solution. The concentration of hydroxide ion required to just initiate precipitation is _____ M.At 25oC the Ksp for PbCl2 is 1.6 × 10–5 - Calculate Q for the following: 125.0 mL of 0.0700 M Pb(NO3)2 is mixed with 75.0 mL of 0.0200 M NaCl at 25oC - Will a precipitate form from the above reaction? (Yes, No, Not enough info)It is found that 8.70e-09 g of Ga(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ga(OH)3.The Ksp of Y2(CO3)3 at 25 oC is 1.03e-31. What is the molar solubility of Y2(CO3)3?