4. Balance the following reactions: a. Ag:0 + C→ CO: + Ag. b. Pb(NOs)2 + NaCl → PbCl2 + NaNO3 I Pb 2n03 IPb TNCI 2 c1 2 Na C. HCI → AICI3 + H2S. d. NaF > Na + F2
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- Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?Sodium formate reacts with permanganate in neutral solution according to the equation CHO2 + MnO4 + H2O → MnO2(s) + CO2 + OH" (a) A 0.500 g sample containing sodium formate is treated with 50.00 mL of 0.0600 M MnO4 (an excess) in neutral solution, and the reaction given above is allowed to proceed to completion. The solution is filtered to remove the MnO2, acidified with H2SO4, and titrated with 30.00 mL of 0.1000 M H2C2O4. The MnO4- is reduced to Mn2+ and the oxalate oxidized to CO2. Calculate the percentage of NaCHO2 in the sample.Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid (below). A solution is created by reacting 4.5 g of PCl5 (MW=208.2 g/mole) with excess H2O. How many moles of NaOH are needed to titrate the resulting solution to completion. PCl5 + 4 H2O ----->5 HCl + H3PO4
- The vanadium in a sample of ore is converted to VO2+ . The VO2+ ion is subsequentlytitrated with MnO4- in acidic solution to form V(OH)4+ and manganese(II) ion. Theunbalanced titration reaction is MnO4 − (aq) + VO2+ + (aq) +H2O (l) → V(OH)4+ (aq) + Mn2+ (aq) + H+ (aq) To titrate the solution, 26.45 mL of 0.02250 M MnO4- was required. If the mass percent ofvanadium in the ore was 58.1 %, what was the mass of the ore sample? Hint: Balance the titration reaction by the oxidation states method.(A). __C₅H₁₂ + __O₂ --> __H₂O + __CO₂ To balance the attached reaction, what coefficient needs to be put in front of the CO₂? (B). __C₅H₁₂ + __O₂ --> __H₂O + __CO₂ What type of reaction is this considered? (C). To make balancing problems that contain H₂O on one side of the equation and the polyatomic ion (OH) on the other side, you should write water as __________ to make it easier to balance43. In the preparation of Rochelle salt (MW = 282.83 g/mol), 7.2 grams of monohydrated Sodium carbonate (MW = 124.01 g/mol) dissolved in 80 mL water was made to react with 20g of Potassium bitartrate (MW = 188.10 g/mol). What is the amount of Rochelle salt obtained from Monohydrated Sodium carbonate? Rochelle's Salt:2 KHC4H4O6 + Na2CO3.H2O + 6 H2O -> 2 KNaC4H4O6.4H2O + CO2 ↑ a 38.77 g b 28.74 g c 36.48 g d 32.84 g
- In the preparation of Rochelle salt (MW = 282.83 g/mol), 6.6 grams of monohydrated Sodium carbonate (MW = 124.01 g/mol) dissolved in 80 mL water was made to react with 43 g of Potassium bitartrate (MW = 188.10 g/mol). What is the amount of Rochelle salt obtained from Potassium bitartrate? Rochelle's Salt:2 KHC4H4O6 + Na2CO3.H2O + 6 H2O -> 2 KNaC4H4O6.4H2O + CO2 ↑ a 37.59 g b 48.12 g c 64.66 g d 33.78 gIn the lime soda process once used in large scale municipalwater softening, calcium hydroxide prepared from limeand sodium carbonate are added to precipitate Ca2+ asCaCO3 (s) and Mg2+ as Mg(OH)2 (s): Ca2+(aq) + CO32-(aq)---->CaCO3(s)Mg2+(aq) + 2 OH-(aq)----->MgOH2 (aq)How many moles of Ca(OH)2 and Na2CO3 should be addedto soften (remove the Ca2+ and Mg2+) 1200 L of water in which[Ca2+] = 5.0 x 10-4 M and[Mg2+] = 7.0 x 10-4 M?A.) What is the balanced ionic reaction for the standardization reaction of C2O42- and MnO4-? B.) How many moles of KMnO4 would we need to neutralize C2O4-?
- The vanadium in a sample of ore is converted to VO2+. The VO2+ ion issubsequently titrated with MnO4- in acidic solution to form V(OH)4+ and manganese (II) ion. The unbalanced titration reaction isMnO4 - (aq) + VO2+ + (aq) + H2O (l) V(OH)4+ (aq) +Mn2+ (aq)+ H+ (aq)To titrate the solution, 26.45 mL of 0.02250 MMnO4- was required. If themass percent of vanadium in the orewas 58.1%,what was the mass ofthe ore sample? Hint: Balance the titration reaction by the oxidation states method.In the potentiometric standardization of a K2Cr2O7 solution, 0.4548 g of Mohr's salt [Fe(NH4)2(SO4)2 is weighed. 6H2O] (392.13 g/mol) which consume 20.0 mL of the K2Cr2O7 solution. What is the Molar concentration of K2Cr2O7? Make the ionic reaction correctly balanced.In an oxidation-reduction reaction, 0.0450 mol of aqueous FeSO4 (source of Fe2+) reacts completely with 120.0 mL of an acidified aqueous solution of KMnO4 (source of MnO4-).5Fe2+(aq) + MnO4-(aq) + 8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(ℓ)What is the molarity of the KMnO4 solution?Provide your answer in decimal notation, rounded to the appropriate number of significant figures.