Calculate the molar solubility of CuS in a medium containing H;S at pH=1 and pH=4. KspCus = 6.5x10-30 [H*][HS¯] [H2S] H2S - H* + HS- Ka1 5.7x10-8 [H*][s²-] HS- - H* + S2- Ка2 1.2x10-15 [-SH] [H*]°[s²-] H;S - 2H+ + Sz KaixKa2 - = 6.8x10-23 = [H2S]
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![Calculate the molar solubility of CuS in a medium containing
H2S at pH=1 and pH=4. Kspcus = 6.5x10-30
[H*][HS¯]
[H2S]
H2S - H* + HS-
Ka1
5.7x10-8
Ka2 = 1.2x10-15 =
Каг
[H*][s?-]
[HS-]
HS - H* + S2-
H;S - 2H+ + Sz KaixKa2
[H*]?[s²-]
[H2S]
6.8x10-23](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F675a343e-d4bc-47a5-93b7-a75a37057497%2F0ab970a5-95bd-469b-9b36-e491be970a95%2F65f3kq_processed.png&w=3840&q=75)
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- Neutralization Titration In the standardization of HCI solution using 10.00 ml of 0.02 Na,co, according to the equation M of Na,CO, 2 HCI 2NaCl + H₂O+CO, 15.0 ml of HCI is required to reach the end point using Bromocresol green indicator the molarity of HCI (mol/L) would be al 0.032 b) 0.027 20.013 d) 0.008 e) 0.064A solution is 0.025 M in Pb2 + . What minimum concentration of Cl- is required to begin to precipitate PbCl2? For PbCl2, Ksp = 1.17 * 10 - 5.a) 1.17 * 10 - 5 Mb) 0.0108 Mc) 0.0216 Md) 5.41 * 10 - 4 M1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…
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- Calculate the solubility of AgCl(s) in 2.0 M NH3(aq).Ksp = 1.6 × 10-10 for AgClKf = 1.7 × 107 for Ag(NH3)2+(aq) 1.9 × 10-5 M 9.5 × 10-2 M 1.3 × 10-5 M 5.2 × 10-2 M 5.4 × 10-3 MIn order to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. Ksp= 1.57x10^-9What is the concentration of the excess reagent?What is the molar solubility of Ba(IO3)2 in this solution? 2.04x10^-5 M 4.07x10^-5 M 6.15x10^-5 M 8.30x10^-5 MIf 0.3074 g of a mixture of pure KCl and KBr requires 30.98 mL of 0.1007 M AgNO3 solution for its titration, calculate the% KCl and KBr in the sample. (Pat Data: Cl, 35.453; Br, 79.904; K, 39.098)