1. Calculate the solubility of ZnC204 in a solution held at pH 4.00. Consider the equilibria ZnC204(s) Zn2+ + C₂042- 2- Ksp = 7.5 x 10-9 C2O4 + H2O HC204 + OH Kb1 = 1.8 × 10-10 HC2O4 + H2O H2C2O4 + OH¯ Kb2 = 1.8 x 10-13
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- Consider the following two acids: pKa1 = 2.98; pKa2 = 13.40 HO2CCH2CH2CH2CH2CO2H Adipic acid pKa1 = 4.41; pKa2 = 5.28 In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results.Calculate the molar solubility of SrC2O4 in a solution that has a fixed H3O+ concentration of (Ksp (SrC204) = 5.0 × 108, K₁ (H2C2O4) = 5.60 x 102, K2(H2C2O4) = 5.42 × 10-5) a. 8.0 × 10-6 M. Molar solubility= M b. 8.0 × 107 M. Molar solubility = c. 8.0 x 109 M. Molar solubility = d. 8.0 x 10-11 M. Molar solubility = M M Mys 111111
- What is the pH of a buffer that is 0.12 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in sodium lactate [CH3CH1OH2COONa or NaC3H5O3]?For lactic acid, Ka = 1.4 * 10-4.Calculate the molar solubility of AgSCN (Ksp = 1.1 x 10^-12) in a solution maintained at pH 9.00 and where the concentration of ammonia is 0.1 M. HSCN: pKa = 4.0 [Ag(NH3)2]^+ : Kf1 = 2.04 x 10^3; Kf2 = 8.13 x 10^3A buffer was made with HC2H3O2 and its conjugate base. What is the pH of the buffer if at equilibrium there was [HC2H3O2] = 0.5000 M and [C2H302ª] = 0.7000 M and the Ka = 1.60 x 10-5 ? everything is based upon the acid dissolving in water: HC2H3O2 + H20 C2H3O21 + H30*1 [ Ka = [ solve for [H30*'] then put in the numbers Ka [ ( [H3O+1] : [ ] [H3O+'] = pH = - log d. HC6H6O61 f. SO3? a. H30+1 b. Он1 c. H2C6H606 е. HSO31 -2 g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. s2 m. HX п. X-1 О. 1 р. 2 q. 3 r. 0.5000 s. 5.5 X 10-5 t. 3.5 X 10-4 u. 8.00 x 10-5 v. 1.75 x 10-6 w. 1.11 x 10-8 х. 5.5 х 102 y. 0.7000 z. 1.60 x 10-5 аа. 1.143 х 10-5 bb. 0.4900 сс. 1.104 х 10-5 dd. 0.7100 ее. 1.26 х 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957
- What is the solubility of CaF2CaF2 in a buffer solution containing 0.45 M formic acid and 0.20 M sodium formate? Given: Ka for formic acid = 1.7×10−41.7×10−4 Ka for hydrofluoric acid = 6.8×10−46.8×10−4 Ksp for CaF2=3.4×10−11Given the values of K and Kb below, which of the systems given would be most suitable to use to construct a buffer of pH 97 HCOOH, K, = 1.8 x 104 CH3COOH, K3=18x105 H3ASO4. Ka1 = 6.0 x 10, Ka2 = 1.1 x 10, Ka3 = 3 x 1012 C5H5N, Kp = 1,7x10-9 NH3 КЬ - 1.3 х. 10-5 OA H3ASO4/NaH2As04 eB. HCOOH/NAHCOO OC. C5H5N/ C5H5NHCI OD.CH3COOH/KCH3CO0 FOE NH4C/NH3A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 ml ot a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONA). [Ka= 1.8 x 10-1 What is the new concentration of the conjugate base, CH3COO after buffering? 0.3385 0.2434 0.1172 0.2269 0.4287
- A pH 7.0 buffer solution is made using NaOH and phosphoric acid. The sum of the concentrations of all phosphoric acid species is 0.1 M. The equilibrium constant Kw for the ionization of water is 10-14 and Ks for the following equilibria are given: H3PO4 H* + H2PO4 K1 = 7.1×10-3 2- H2PO4 H* + HPO4 K2 = 6.2x10-8 3- НРОД H* + PO4 K3 = 4.5×10-13 Calculate the concentrations of all species in solution. Formulas: pH=-log1o[H"], pK=-log1„KFor each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. IF the solubilitv does change, pick the pH at which you'd expect the highest solubility. You'll find K data in t do Data sp Does solubillty change with pH? highest solubillity BaCro4 1.17x10-10 compound pH = 4 pH = 6 pH = 7 BaSO4 1.08x10-10 O yes CaCO3 3.36x10-9 CaCl, O no CaF2 3.45x10-11 Co(OH)2 5.92x10-15 O yes Ca (OH), CuBr 6.27x10-9 О по CuCo3 1.4x10-10 O yes Mg Cl, Fe(OH)2 4.87x10-17 О по PBCO3 7.40x10-14 PbCro4 2.8x10-13 PBF2 3.3x10-8 Mg(OH)2 5.61x10-12 Ni(OH)2 5.48x10-16 AgBrO3 5.38x10-5 Ag2CO3 8.46x10-12 AgCI 1.77x10-10 Ag2Cro4 1.12x10-12 SrCO3 5.60x10-10 ZnCO3 1.46x10-10 Zn(OH)2 3.0x10-17 AgBr 5.35x10-13 AuCI 1.77x10-10 Explanation Check O2021 McGraw-Hill Education. All Rights Reserved. Tems of Use Privacy Accessibility MacBook Air FI F2 F6 F10consider the reaction Ag2O(s) + H2O -> 2Ag+ + 2OH- Ksp = 3.8 x 10-16 If Ag2O forms to an appreciable extent what effect will this equilibrium have on the solubility of AgCN? Explain your reasoning. Judging by the equilibrium reaction shown, would you expect the effect of this equilibrium on the solubility of AgCN to be pH dependent?