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A solution consists of 0.020 mol.kg-1 KCl(aq) and 0.035 mol.kg-1 Ca(NO3)2(aq). For Cd(NO3)2(aq), calculate (i) the average activity coefficient, and (ii) the activities of Cd2+ and NO3
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- Determine the activity coefficients and effective concentrations (activities) of Na+ and Ca2+ ions in an aqueous solution having the following composition: [Ca2+] = 3.25x 10-3 M; [Na+] = 0.96x 10-3 M; [HCO3-] = 5.75x 10-3 M; [SO42-] = 0.89x 10-3 M. (Note: Solvated ionic radii are: a(HCO3-) = a(SO42-) = 4 Å; a(Ca+) = 6 Å)At a certain temperature, the solubility of zinc(I) chromate is (7.6x10^-5) M. What is the Ksp? Report your answer to 2 sig figs. Note: Your answer is assumed to be reduced to the highest power possibleA solution consists of 0.020 mol.kg-1 KCl(aq) and 0.035 mol.kg-1 Ca(NO3)2(aq). For Cd(NO3)2(aq), calculate (i) the average activity coefficient, and (ii) the activities of Cd2+ and NO3
- A chemist has a 50.0 mL sample of 0.010 M Na₂C₂O4 at 25 °C (solution A, oxalate ion = C₂04²-). An aqueous solution of Ca(NO3)2 with a volume of 50.0 mL (solution B) is added to solution A, at the same temperature. Above what minimum concentration must Ca(NO3)2 in solution B be, prior to mixing, to cause CaC₂O4 to precipitate given that for CaC₂O4, Ksp = 2.7 x 10-⁹ at 25 °C? Enter your answer with two significant figures, without units, and in millimolarity (mM) where: millimolarity = (molarity)(1000)Calculate the solubility of Ba(IO3)2 in pure water, Ksp=1.5x10^-9. Then calculate the solubility of the same Ba(IO3)2 in a 0.0025M Al(NO3)3 solution. Assume there is no other interatcion between any of the ionic componets of the 2 molecules. (do an activity coeffiecient problem using the neatest u value to determine f from the table)Determine the Ksp of PbBr2 if its molar solubility in water at 25 °C is 1.05 x 10−2 M. You can use either Method 1 or 2. Note: This equation, (S = n+m√Ksp/nn . Mm), can be rearranged to the following to solve for Ksp; Ksp = S(n+m) . nn.mm
- 4. Calculate the percent relative error in the solubility of Fe(OH)3 in 0.0250 M NH&NO3 by using molar concentrations instead of activities.19" 0.00014 m Na2 Coz are combined? Determine the solubility of Cul (s) (Ksp.= 1.1x1013 In 0.15m Cu₂ (03 (aq) Solution,Use the Debye-Hückel equation to calculate the activity coefficient of each ion at the given ionic strength in an aqueous solution at 25 °C. Pb2+ in a solution where μ = 0.0611 M YPb²+ = PO3 in a solution where μ = 0.0483 M YPO x10 TOOLS Ion Pb²+ Mg2+ Zn²+ Cro Cr³+ PO Zr¹+ Ce4+ Ion size (a, nm) 0.450 0.800 0.600 0.400 0.900 0.400 1.100 1.100
- ST5G.2 - Estimate the solubility of CaF2(aq) [in units of PICOmolar] in the presence of 0.701 molar AIF3(aq). [This is a bit fictitious - I don't think aluminum fluoride is soluble, but I want you to think carefully about the fluoride concentration.] Type your answer..a) What is the solubility of copper(II) iodate, Cu(IO;)2? Ksp. = 1.4 x 107 at 25 °C %3D b) Will the solubility of Cu(IO3)2 (s) increase, decrease or remain the same if some solid Cu(NO:)2 is added? (copper(II) nitrate is very soluble and completely dissolves) c) Aqueous copper(II) ions, Cu²* to the reaction: (a0), react with aqueous ammonia to form a complex according Cu2+, (a0+ 4NH3 (a) [Cu(NH3)4]* (aq) with a formation constant, Ke= 1.2 x 1013 How will the addition of aqueous NH3 effect the solubility of Cu(IO3)2 (s)? (increase, decrease or no effect)Calculate the % relative error in solubility by using concentrations instead of activitiesfor Fe(OH)2 in 0.0500 M KNO3 (give the source for thermodynamic solubility).