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Refer to the precipitation reaction below. CoCl2(aq)+2NaOH(ag) Co(OH)2(s)+2NaCI(aq) How much 0.5 M NaOH solution in liters...
Solve stoichiometry problems with reactants in solution Question Refer to the precipitation reaction below. CoCl2 (aq) + 2NaOH(aq) + C(OH)2(s) + 2NaCl(aq) How much 0.5 M NaOH solution in liters will completely precipitate the Co2+ in 1.6 L of 0.12 M CoCl2 solution? Round to two significant figures, and do not include units in your answer. Provide your answer below:
2NaOH (aq) + MgCl; (aq) + 2NaCl (aq) + Mg(OH)2 (s),- how much 0.1 M NaOH solution will completely precipitate the Mg²+ in 0.8 L of 0.10 M MgCl, solution? Round to 2 significant figures. Provide your answer below: LNaOH FEEDBAC
Solve stoichiometry problems with reactants in solution Question Refer to the precipitation reaction below. KCl(aq) + AgNO3 (aq) → KNO3(aq) + AgCl(s) How much 0.9 M KCl solution in liters will completely precipitate the Ag+ ion in 0.9 L of 0.19 M AgNO, solution? Round to two significant figures, and do not include units in your answer.
Let us assume that Cd(OH)2(s) is completely insoluble, which signifies that the precipitation reaction with NaOH(aq) (presented in the transition) would go to completion. Cd2+(aq)+2NaOH(aq) → Cd(OH)2(s)+2Na+(aq) If you had a 0.450 L solution containing 0.0190 M of Cd2+(aq), and you wished to add enough 1.31 M NaOH(aq) to precipitate all of the metal, what is the minimum amount of the NaOH(aq) solution you would need to add? Assume that the NaOH(aq) solution is the only source of OH−(aq) for the...
Let us assume that Fe(OH)3(s) is completely insoluble, which signifies that the precipitation reaction with NaOH(aq) (presented in the transition) would go to completion. Fe3+(aq)+3NaOH(aq) ? Fe(OH)3(s)+3Na+(aq) If you had a 0.450 L solution containing 0.0200 M of Fe3+(aq), and you wished to add enough 1.33 M NaOH(aq) to precipitate all of the metal, what is the minimum amount of the NaOH(aq)solution you would need to add? Assume that the NaOH(aq) solution is the only source of OH?(aq) for the precipitation....
Solve stoichiometry problems with reactants in sol ution Question Refer to the precipitation reaction below. CaCl2 (aq)2AgNO3 (aq) - Ca(NO3)2 (aq) +2AgCI (s) How much 1.5 M CaCl2, in liters, will completely precipitate the Agt in 1.0 L of 0.20 mol A^NO2 solution? Round to two significant figures. Do not include units in your answer. Provide your answer below:
KCl (aq) + AgNO3(aq) → KNO3(aq) + Agus) How much 0.9 M KCl solution in liters will completely precipitate the Agion in 0.9 L of 0.19 M AgNO, solution? Round to two significant figures, and do not include units in your answer.
Answer the following for the reaction: NiCl2(aq)+2NaOH(aq)→Ni(OH)2(s)+2NaCl(aq) A.) How many milliliters of 0.200M NaOH solution are needed to react with 48.0 mL of a 0.240 M NiCl2 solution? Express your answer with the appropriate units. B.) How many grams of Ni(OH)2 are produced from the reaction of 34.0 mL of a 1.70 M NaOH solution and excess NiCl2? Express your answer with the appropriate units. C.) What is the molarity of 30.0 mL of a NiCl2 solution that reacts completely...
Let us assume that Fe(OH)3 (s) is completely insoluble, which signifies that the precipitation reaction with NaOH(aq) (presented in the transition) would go to completion. Fe3+ (aq) + 3NaOH(aq) + Fe(OH)3(s) + 3Na+ (aq) If you had a 0.350 L solution containing 0.0150 M of Fe3+ (aq), and you wished to add enough 1.26 M NaOH(aq) to precipitate all of the metal, what is the minimum amount of the NaOH(aq) solution you would need to add? Assume that the NaOH(aq)...
2KI (aq) + Pb(NO3)2 (aq) + PbI, (s) + 2KNO3 (aq). How much 0.7 M KI solution in liters will completely precipitate the Pb2+ in 2.1 L of 0.18 M Pb(NO3), solution? Do not include units in your answer and round to two significant figures. Druiden bela