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- 10A Complete the figure below. Br NaCN DMSO B A NH₂ C 1. Br₂, NaOH 2. H₂O/H* TT. H₂SO4BaCO3 - Ba2+ + CO3? reaction was given. It is known that the carbonate anion is hydrolyzed in [HCO ][OH] [co? ] CO3- + H20 = HCO; + OH Kb1 and [H2CO3][OH¯] [HCO3] HCO; + H2O = H;CO3 - OH- Kb2 = form. Since Ka1 = 1.44x10-7, Ką2 = 4.7x10-11 and KspBaco3 = 5.1x10-9, calculate the solubility of BaCO; salt at pH = 8 and 12 depending on the pH value.9. Homework • Unanswered HCl(ag) +_N22CO3(aq) → Identify the spectator ions. NaCl(ag) + _CO2(8) + _H2O(1) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. Nat andH+ a b Nat and CO Natand Cl- d co?-and Cl-
- 1. BH3, THF 2. H₂O₂, OH H₂/Pd Br₂ CH3OH HBr NaCl exceso Br₂ CHCl3 HBr / H₂O₂ (1) Hg(OAc)2; H₂O (2) NaBH₂OHa. HCl(aq) + NaOH(aq)→NaCl(aq) + H2O(1) b. Ba(OH)2(aq) + ZnCl2(aq)→BaCl2(aq) + Zn(OH)2(s) c. 2A9NO3(aq) + Mg(s)→Mg(NO;)2(aq) + 2Ag(s) d. HNO3(aq) + NH3(aq)→NH¼NO3(aq) + H2O(1) e. 2Cu(s) + O2(g)→2CUO(s) f. CaCl2(aq)+K2CO:(aq)→2KCI(aq)+CaCO3(s) 2. Calculate the maximum volume of 6 M HNO3 which would be required to react with 0.350 g of Cu metal as shown in the initial equation (step 2)? 3.If you used 2-3 mL of 6.0 M HNO; to dissolve the sample of Cu (0.350 g), what volume of 4.0 M NaOH would be required to neutralize the excess HNO3? 4.Solid zinc is used in the last reaction to reduce the copper in the copper (II) sulfate solution to elemental copper. Identify 2 other metals that could be used to perform the reduction. Explain your answer. Write a balanced chemical equation for each identified metal. 5.Based on your research, which of these metals you think would be the "greenest" metal to use? Justify your answer using MSDS and costs effects.1._C,H + 0, > CO H,O 2. Ca,(PO.),(OH). + H,POla + Ca(H,PO), H,O, 3. C.H,Os + CO.e + NH,NO > _N H,0 +
- 1. T(OIPr), TBHP (+)-DET но 2.Cro, HSO.3. Complete and balance the following single displacement equations. If no reaction takes place, indicate by writing N.R. a. d. Cl2 + KBr → е. Zn + SnBr2 → ||Use the acidity model pH = −log[H+], where acidity (pH) is a measure of the hydrogen ion concentration [H+] (measured in moles of hydrogen per liter) of a solution.Find the pH when [H+] = 4.7 × 10−5. (Round your answer to two decimal places.)pH =