Select the correct total ionic equation for the reaction of iron(III) nitrate with sodium hydroxide. Read each answer choice carefully. Fe(NO3)з (aq) + 3NaOH (аq) — Fe(ОН)з (s) + 3NaNO3 (аq) Fest (aq) + 3NO3° (aq) + 3Na* (aq) + 30H¯ (aq) → Fe(OH)3 (s) + 3Na* (aq) + 3NO3 (aq) + NO3 (aq) + Na* (aq) → NaNO3 (s) Fe(NO3)3 (aq) + 3NAOH (aq) → Fe(OH)3 (aq) + 3NaNO3 (s) Fe3+ (aд) + 3ОН (аq) — Fe(ОH)з (s) Fe3+ (aд) + 3NO3 (аq) + 3Na* (аq) + 3он (ад) — Fe$* (aq) + 3ОН (аq)+ 3NaNO3 (s)

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 73.mg .   Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 111. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 0-2 X 5

Balance the molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and states of the products in each of the cases. CaCl2 (aq) + Pb(OH)2 (aq) → H2SO4 (aq) + Ba(OH)2 (aq) - AGNO3 (aq) + KCI (aq) – HCIO4 (aq) + Ca(OH)2 (aq) -

Which of the below represents the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of iron(II) nitrate and potassium sulfide are mixed? Group of answer choices Fe2+(aq) + S2-(aq) → FeS(s) K+(aq) + NO3-(aq) → KNO3(s) 2 K+(aq) + S2-(aq) + Fe2+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s) No reaction occurs. 2 K+(aq) + S2-(aq) + Fe2+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq)

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s)  +   CuSO4 (aq)  →   Cu (s)  +   FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a  300.mL  copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of  67.mg .   Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.

Give the net ionic reaction equation for the following reaction: CuCl 2 (aq) + 2 NaOH (aq) → Cu(OH) 2 (s) + 2 NaCl (aq)

5. Identify each of the following reactions as either synthesis, decomposition, single displacement, double displacement, combustion, or neutralization 2Li(s) + H₂O(1)→ Li₂O(s) + H2(g) SO2(g) + H₂O → H₂SO3(aq) 02|| AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) + 2NaOH(aq) → Na₂CO3(aq) + H₂CO3(aq) 2H₂O C3H8(g) + 502(g) → 3CO2(g) + 4H₂O(1) Mg(OH)2(aq) → MgO(s) + H₂O(1)