Calculate the molar solubility of BaSO4 in a solution in which H30 is (Ksp (BaSO4) = 1.1 x 10-10, K2(H2SO4) = = 1.02 x 10-2) %3D %3D а. 2.3 М. Molar solubility= M %3D b. 0.40 M. Molar solubility = M c. 0.057 M. Molar solubility = M %3D d. 0.16 M. Solubility = M %3D
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- Copper(I) ions in aqueous solution react with NH, (aq) according to Cut (aq) + 2 NH, (аq) — Си(NH, ); (aq) 3 6.3 х 1010 - Calculate the solubility (in g-L-!) of CuBr(s) (Ksp = 6.3 × 10-9) in 0.72 M NH, (aq). solubility of CuBr(s): g/LO e) % KBr = % 66.2 , % KCI = % 33.8 %3D The solubility product (Ksp) for 4 points Pb(OH)2 (s) is 2.5 x 10-16. What would be the quantity of solubility by g/L of Pb(OH)2 which has Mwt =241.2 g/mole)? O 9.947 x 10-4 O 5.975 x 10-4 O 7.596 x 10-5 O 9.575 x 10-4 O 9.723 x 10-4 Calculate [H+], PH and POH 4 pointsCalculate 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).
- 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.TUOv to lls worla taum uo 1o9TIOoni bolam od lliw elimu iboo lut o 19 4. Given the Borax reaction below, what would be the solubility product (Ksp) of borax at 40 °C, if the solubility of borax is 0.8 mol L¯1 at 40 °C? Na,B4O5 (OH)4 · 8H,O(s) = 2Na+ (aq) + B405(OH) (aq) +8H,O(1) sr vol (A) gnsb vgotino brrbae ar bo CHO)gab xglerino bisbasie orb il SA solution of Na,SO, in water is saturated at 50°C. When a saturated solution of Na,SO, is cooled, crystals of Na,SO4-10H2O separate from the solution Temperature, °C Solubility of Na,SO, g/100g water 49 50 46.7 10 9 If 1000 kg of this solution is cooled to 10°C, the percentage yield obtained is nearly а. 91 b. 90 с. 100 d. 80
- 4. Write the eauilibrium constant expressions (Ka, Kb, Kw and Kc), for the following reactions. (REVISION) a. C(s) + O2(8) = CO:(8) b. C3Ha(g) + 502 (g) = 3CO2(g) + 4H;0(g) c. HCl(aq) + H20(1) = cr(aq) + H30*(aq)Calculate the solubility of PbCO , in water at 25 °C. You'll find K, data in the ALEKS Data tab. sp Round your answer to 2 significant digits. dlo Ar alo Data BaSO4 1.08×10-10 СаСОз 3.36×10-9 CaF2 3.45x10-11 Co(OH)2 5.92×10-15 CuBr 6.27×10' o-9 CuCo3 1.4x10-10 Fe(OH)2 4.87×10¬17 PЬСОЗ 7.40×10-14 PbCro4 2.8×10-13 PBF2 3.3x10-8 Mg(OH)2 5.61×10¬12 Ni(OH)2 5.48×10-16 AgBrO3 5.38x10-5Calculate the solubility at 25 °C of PbCrO4 in pure water and in a 0.0180 M Na2CrO4 solution. You'll find K Round both of your answers to 2 significant digits. sp data in the ALEKS Data tab. solubility in pure water: solubility in 0.0180 M Na2CrO4 solution: ㅁ은 g x10 ☐ L ☑ 믐 D
- will W S > 3. What is the final molar concentration if 285.0 mL of water is added to 450.0 mL of a 0.925 mol/L aluminum sulfate (Al2(SO4)3] ? JUN 10 TO 0 #3 Q E D 4 C I R F % 5 V T MacBook Pro & ^ 6 G Y 7 U H BN * 00 8 4 1 ( 9 JK M 0 V LWrite the ionic equation for dissolution and the solubility product (Ksp) expression for the following slightly soluble ionic compounds: Ag2S O a. Ag2S(s) 2Ag* (s) +S2 (s) , Ksp= [Ag*j?js?J/Ag2S (s) , Ksp= [Ag*]2Ag" +s2- (aq) , Ksp= [Ag*?is21 (aq) O C. Ag2S(s) Ag" +s2- (aq) , Ksp= [Ag*][S27 (aq) O d. Ag2S(s) Ag* (ag) +S (aq) , Ksp= [Ag*][S]For a 0.0448 M aqueous solution of aniline, C6H5NH2 (Kb = 7.4E-10), determine the following. Kw = 1.0E-14. a. What is the concentration of the minor species present in the solution? b. What is the concentration of the major species present in the solution? c. What is the concentration of H3O+?