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- You may want to reference (Page 834) Section 18.3 while completing this problem. Part A If 130.0 mL of 0.0020 M Na2SO4 (aq) is saturated with CaSO4, how many grams of CaSO4 would be present in the solution? [Hint. Does the usual simplifying assumption hold?] Express your answer using two significant figures. VE ΑΣΦ ? m = 0.43 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining gIminodiacetic acid (IDA) is often used in ion exchange resins as a way to remove heavy metals from industrial waste waters. It forms a 2:1 complex with many heavy metals, with a high selectivity for divalent over monovalent ions. A 14.50 mL sample of 0.0315 M Ni2+ was added to 14.50 mL of 0.187 M iminodiacetic acid (the completely protonated form is abbreviated as H3A+) buffered at pH 7.00. Given that ?A2− is 4.6×10−3 at pH 7.00, what is the final concentration of Ni2+ remaining in solution? Ni2+(aq)+2A2−(aq)↽−−⇀NiA2−2(aq)?f=2.00×1014 [Ni2+]= __________ MWhat is the solubility of NH3 if its partial pressure is reduced to 30,000 Pa?
- Iminodiacetic acid (IDA) is often used in ion exchange resins as a way to remove heavy metals from industrial waste waters. It forms a 2:1 complex with many heavy metals, with a high selectivity for divalent over monovalent ions. A 22.50 mL sample of 0.0454 M Ni²+ was added to 22.50 mL of 0.190 M iminodiacetic acid (the completely protonated form is abbreviated as H, A*) buffered at pH 7.00. Given that ais 4.6 x 10-3 at pH 7.00, what is the final concentration of Ni²+ remaining in solution? Ni²+ (aq) + 2 A² (aq) = N₁A3(aq) [Ni²+] = K₁ = 2.00 × 10¹4 Ma. A 1.00 liter solution contains 0.45 moles nitrous acid and 0.35 moles potassium nitrite .If 0.17 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of HNO2 will decrease. B. The number of moles of NO2- will decrease. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase. b. A 1.00 liter solution contains 0.38 M ammonia and 0.49 M ammonium bromide. If 0.120 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) A. The number of moles of NH3 will decrease. B. The number of moles of NH4+ will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will increase. E. The ratio of [NH3] /…The concentration of V²⁺ in a saturated solution of V₃W₂ is 1.37 x 10⁻² mg/L. What is the Ksp ofV₃W₂ if the MM of V is 40.08 g/mol?
- The Ksp for BaCO3 is 5.1×10−9.5.1×10−9. How many grams of BaCO3 will dissolve in 1000. mL of water?How many grams of lead azide will dissolve in 500 mL of 100 M Pb(NO3)2 solution? Ksp=3.4×10^-1412. The following quantities of salts were added to a volume of water to make 1 liter of solution: 1 x 10-2 moles NaCl 2 x 10-2 moles CaCl, 2 x 10-2 moles BaCl, (a) What is the ionic strength of the solution? (b) A small amount of phosphate salt is added to the same solution with negligible change in ionic strength. Given K = 10-7.2 for the reaction H,PO, = H+ + HPO,?- Calculate (H*][HPO,2-1/[H,PO,"), called °K, using the Güntelberg ap- proximation of the DeBye-Hückel law. (c) Calculate the "salting-out" coefficient, k,, for a nonelectrolyte in the same solution if its activity is 10-3 M and its concentration is 9.5 x 10 4 M.
- The solubility-product constant for Ce(IO3)3 is 3.2 X 10-10. What is the Ce3+ concentration in a solution prepared by mixing 50.0 mL of 0.0250 M Ce3+ with 50.00 mL of water?a. 0.040 M IO3- ?Iminodiacetic acid (IDA) is often used in ion exchange resins as a way to remove heavy metals from industrial waste waters. It forms a 2:1 complex with many heavy metals, with a high selectivity for divalent over monovalent ions. 3 A 27.50 mL sample of 0.0652 M Ni²+ was added to 27.50 mL of 0.195 M iminodiacetic acid (the completely protonated form is abbreviated as H3A+) buffered at pH 7.00. Given that a A²- is 4.6 × 10-³ at pH 7.00, what is the final concentration of Ni²+ remaining in solution? Ni²+(aq) + 2 A²¯(aq) = NIA2¯(aq) Kf = 2.00 × 1014A 1.00 liter solution contains 0.33 moles nitrous acid and 0.25 moles potassium nitrite . If 0.13 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) JA. The number of moles of HNO2 will remain the same. B. The number of moles of NO2 will decrease. |C. The equilibrium concentration of H30* will decrease. D. The pH will increase. E. The ratio of [HNO2] / [NO2] will remain the same.