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- 1. When both solids, AgCl and Ag2CrO4, are precipitated, the mass action expressions in equations 2 and 4 above must be obeyed simultaneously. a. From equations 2 and 4, derive an expression for the concentration of Cl ions in terms of the concentration of CrO42 ions. That is, derive an equation in the form [CI] = ? such that the right side of the equation contains [CrO42] but not [Ag+]. b. Assuming that [CrO42] = 0.003 M, compute [CI] still present in solution at equilibrium. C. What volume of a 0.035 M AgNO3 solution would be required to completely react with the amount of CI determined in part b above? Assume that 25 mL of the unknown Cl solution is titrated. d. From the results of the calculations in parts b and c, was it reasonable to assume that essentially all of the CI ions are removed from the solution before the Ag2CrO4 begins to form? Explain your answer. Hint: compare your answer for part c above with the readability of the buret.Ca(OH)2 (aq) + PO43- (aq) → Ca5OH(PO4)3 (s) + OH- (aq) A) What is the mass of calcium (in grams) that can be recovered?Which species is oxidized based on the following reaction? 2 Al³* (aq) + 2 Fe(s) → 2 Al(s) + 3 Fe²*(aq) O A13+ O Fe O Fe2+
- Balanced Chemical Equation Reaction 1: 2 Al(s) + 2 K+(aq) + 2 OH(aq) + 10H₂O(l) → 2 K+(aq) + 2[Al(H₂O),(OH)₂] (aq) + 3 H₂(g) Reaction 2: 2 K+(aq) + 2[Al(H₂O)₂(OH)4](aq) + 2 H+ (aq) + SO4²(aq) → 2 K+(aq) + SO₂²(aq) + 2Al(H₂O)(OH)3(s) Reaction 3: 2AI(H₂O)(OH)3(s) + 6 H*(aq) + 3 SO²-(aq) → 2 A¡³+(aq) + 3 SO² (aq) + 12 H₂O(l) Reaction 4: K+(aq) + Al³+(aq) + 2 SO²(aq) → KAl(SO4)₂∙12H₂O(s) To get the balanced overall equation for the conversion of aluminum metal to the formation of the final product, you'll need to add these four equations together and cancel the like terms. You may need to balance with additional water (H₂O) to balance fully.Mg(OH)2(s)+2HNO3(aq)→ the balanced chemical formula?Ni (s) + Cu,SO, (aq) >
- How to write a chemical equation for transition metal ions found in a solution? The ions found were Cobalt and Copper. Co2+ (aq) + Cu2+ (aq) was mixed with NaOH (aq). It formed Co(OH)2 (s) + Cu(OH)2 (s) + Na^+ (aq). The sample was decanted and Na+ was removed. NH3(aq) was added to Co(OH)2 (s) + Cu(OH)2 (s) and became Co(OH)2 + Cu(NH3)4 ^2+ and NH3. The sample was centrifuged and decanted the ions were now in their own tubes. One tube had Co(OH)2 and the other had Cu(NH3)4 ^2+ and NH3. The tube with Co(OH)2 was then mixed with HNO3 and became Co^2+. The tube with Cu(NH3)4 ^2+ and NH3 was mixed with HNO3 and became Cu^ 2+ and NH4^+.Identify which species was oxidized and which was reduced. 2Na(s) + CuSO4 (aq)→ Cu(s) + Na2SO4 (aq)2 Al (s) + 3 Pb2+ (aq) → 3 Pb (s) + 2 Al3+(aq) which species acts as the oxidizing agent? Explain.