a Choose the correct balanced equation that describes this precipitation reaction: Naz CO3 (ag) + CaCl2 (ag) → CaCO3(s) + NaCl(aq) Naz CO3 (ag) + CaCl2 (ag) → CaCO3(s) + 2NaCl(ag) Naz CO3 (aq) + CaCl2 (ag) → CaCO3 (aq) + 2NACI(ag) Naz CO3 (ag) + CaCl2 (ag) → CaCO3(s) + NaCl(ag) Naz CO3 (ag) + CaCl2 (aq) → CaCO3 (aq) + NaCl(ag) b Choose the correct balanced equation that describes this precipitation reaction: Fe(C,H3O2)2 (aq) + Na, S(ag) → FeS(s) + NaC, H3 O2 (aq) Fe(C2H3 O2)2(ag) + Na2 S(aq) FeS(aq) + NaC, H3 O2 (aq) Fe(C, H3 O2)2 (ag) + Naz S(ag) →FES(s) + NaC, H3 O2 (aq) Fe(C, H3O2)2 (ag)+ NazS(aq) FeS(ag) + 2NAC2 H3 O2(ag) Fe(C,H3O2)2 (ag) + Na2S(aq) → FeS(s) + 2NAC, H3 O2 (ag) c Choose the correct balanced equation that describes this precipitation reaction: KOH(ag) + FeCl2(aq) → Fe(OH)2 (s) + KCl(aq) 2КОН(ад) + FeCl3 (aq) + Fe(ОН)2 (aq) + 2KCI(аg) 2КОН(ад) + FeCl, (aq) > Fe(ОH)2 (8) + 2КCI(ад) 2КОН(аq) + FeCla (ag) > Fe(ОH)2 (8) + КСІ(ад) о коН(ад) + FеClz (aq) Fe(ОН): (8) + 2КCI(aд)

In the reaction, Cu + 2 AGNO3 → Cu(NO3), + 2 Ag, the substance that becomes oxidized is Cu Ag O Ag+ O Cu2+

Choose the correct complete ionic equation and total ionic equation for the following reaction. Lithium carbonate reacts with magnesium chloride. O Mg2+ (aq) + 3CO² (aq) → MGCO3 (s) O Mg2+ (aq) + C (aq) + 302 (aq) → MgCO, (s) O Liz* (aq) + CO32 (aq) + Mg2+ (aq) + Cl2 (aq) → MgC03 (s) + Liz* (aq) + Cl, (aq) O2LI* (aq)+ C032 (aq) + Mg²* (aq) + 2Cl (aq) MgCO3 (s) +2Li* (aq) + 2CI (aq) O Mg2* (aq) + Co, (aq) MgCO3 (s) O Li* (aq) + CO32- (aq) + Mg2* (aq) + CI (aq) → MGCO3 (s) +Li* (aq) + CI (aq)

How many grams of Ag₂CO3 will precipitate when excess Na₂CO3 solution is added to 49.0 mL of 0.590 M AgNO3 solution? 2AgNO3(aq) + Na2CO3(aq) → Ag2 CO3(s) + 2NaNO3(aq) g

Write the net ionic equation for the reaction when solutions of magnesium sulfide (MgS) and copper (1) nitrate (CUNO3) are mixed given the reaction below: Reaction: MgS (aq) + 2 CuNO3 (aq) → Mg(NO3)2(aq) + Cu₂S (s) Be sure to write out the complete ionic reaction first to find which ions are spectator ions.

1.45-g sample of oxalic acid, H2C2O4, is dissolved in distilled water to make 50.00 mL of aqueous solution. This solution is called “Solution A”. The 5.00 mL of Solution A is added to 20.00 mL of distilled water to make “Solution B”.H2C2O4(aq) reacts with MnO4–(aq) to produce CO2(g) and Mn2+(aq).When 19.41 mL of H2C2O4(aq) (Solution B) is mixed with 21.59 mL of 0.0400 M MnO4–(aq), the mass of CO2(g) obtained is 0.0990 g.(a) In this chemical reaction, which substance is the oxidizing agent? Why?(b) Calculate the percentage yield of CO2(g).(c) Determine the molarity of the excess reactant at the end of the chemical reaction.

You are carrying out an experiment to determine the MW of a solid acid with the generic formula H3A. You weigh out 0.362 g of the solid acid in a weigh boat and transfer it to a 125 mL Erlenmeyer flask. After dissolving the acid in 25 mL of distilled water, you add 22.51 mL of 0.343 M Sr(OH)2 (aq) solution with a buret until your indicator changes color at the equivalence point. What is the molar mass of the solid acid in units of g/mole? Enter your answer with at least 4 significant digits (Canvas sometimes truncates zeros so assume that all numbers in this question have at least 4 sig figs (ie if Canvas tells you there are 12.3 mL assume 12.30 mL). This question will require precision so don't round any numbers until your final answer.

Potassium iodide reacts with lead(II)(II) nitrate in the following precipitation reaction: 2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s)2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s) What minimum volume of 0.218 MM potassium iodide solution is required to completely precipitate all of the lead in 145.0 mLmL of a 0.150 MM lead(II)(II) nitrate solution?

A student combined CuCl2 (aq) and Na (s). The student observed a color change, thus a reaction occurred. Write the balanced molecular equation for this reaction showing coefficients and phase labels. Write the complete ionic equation for this reaction. Write the net ionic equation for this reaction. Assign oxidation numbers to the reactants and products in the net ionic equation. Which reactant, CuCl2 (aq) or Na (s), got oxidized? Which reactant, CuCl2 (aq) or Na (s), got reduced? Which reactant, CuCl2 (aq) or Na (s), is the oxidizing agent? Which reactant, CuCl2 (aq) or  Na (s), is the reducing agent?

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.