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Please answer the question attached below with complete solution showing how the mean salt method was used:
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- Calculate the mean ionic molality for 0.25m LaCls. [Ans. 1.1914 m] 570 nsmer For aqueous HCl solutions, it can be determined: Y- =0.72515 + 0.029188m + 0.055959m Determine the molality at which auCi= 1. (Note: This is the molality for the standard state of HCL in Water; pHCI) [Ans. 1.1914 m] %3DCalculate the molar solubility of tin(II) hydroxide (Ksp = 5.45x10-27). Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-2).The equilibrium for the various proportions of the dissociation of the liquid solutions of amyl ester of dichloroacetic acid (CHCI,COOC,H,) into the acid (CHCI,COOH) and amylene (CH) was investigated. The initial amount for the CHCI,COOC.H, used is 1 mole. Completethe table below: Let b the initial moies of amylene. V the total volume of mixtures in Ilters, x be the number of moles of b V Kc 7.30 0.959 0.650 8.16 1.062 3.49 ester at equilbrlum and Kc equilbrium constant in moles per liter. 11.33 0.688 3.35 1.734 0.700 3.24
- The equilibrium for the vorious proportions of the dissociation of the liquid solutions of amyl ester of dichloroacetic ccid (CHCI,.COOC,H,} into the acid (CHCLCOOH) and amylene (C,H was investigated. The inltial amount tor the CHCI,COOC.H used Is 1 mole. Completethe table below Let b the inltial moles of omylene, V the totdl volume cof mixtures in iters, x. be the number of moles of V. 1.05 0.215 0.455 3.12 .af equibrium ond Kc ester outionum constont n.moles per iter. 2.61 0.401 4.45 0.628 3.54 0.794 0.658 3.441 A 0.05 m CaCI, solution has a mean activity coefficient of 0.58. The mean ionic activity of the solution is: O 0.058 m 0.0794 m O 0.037 m 0.063 m 0.046 mA solution of HCl was titrated against sodium carbonate. What is the average normality of acid in the given data? (MW Na₂CO3 = 106) T2 0.3479 0.3562 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (mL) Vol HCl used (mL) 35.10 39.40 N of HCl (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)
- The mean activity coefficient of a 0.010 m H2SO4 solution is 0.544. What is its mean activity?Analysis of dissolved sulfate concentration is based on the precipitation reaction of barium sulfate, creating Baso4 5) (named barite) and its settling. The following water quality is given: TDS = 650 mg/I, (SO) = 40 mg/l as S. Solubility constant of BaSO:: Kip (Baso.) = 1.1 1010 Determine how many mg of BaCl, should be added to 200 ml of a solution at the given quality for completely precipitating the sulfate. That is, calculate the dose required for 99.9% removal, while assuming saturation with respect to barite is immediately reached.(c) (a) Pure Pure Composition reactants products For the three curves, what is the common feature of them? Choose one only. A. Same amount of starting materials. B. At the equilibrium points the slopes of dG/dn = 0. C. same chemical potential at the equilibrium point. D. same composition at the equilibrium point. Gibbs energy, G
- 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 possibleWhich of the following sentence is correct: O Reprecipitation usually increases coprecipitated impurities O Digestion is a process in which a precipitate is heated in the presence of solution to improve the purity and filterability OIn peptization, the size of coagulated colloid increased and become stable O Coprecipitation doesn't cause either positive or negative errors O To increase the particle size of the precipitate the relative supersaturation should be maximized.ST5H.2 - Estimate the mean ionic activity coefficient for the ions in an aqueous solution at 25°C that is 5.36*10-4 molar M2X1 (with ions M1+ and X2). Type your answer..