What would be the net ionic equation?

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)

In an electrolysis of a solution with sodium chloride NaCl(aq), sodium hydroxide is formed NaOH(aq), chlorine gas Cl2(g), and hydrogen gas H2(g), after the reaction equation: 2NaCl(aq) + 2H2O(l) → 2NaOH(aq) + Cl2 (g) + H2(g)   a) An electrolysis is a redox reaction. What substance is oxidized, and what substance is reduced in the electrolysis of the solution with sodium chloride NaCl(aq)? Base your answer by showing to change in oxidation figures.   b) Use the table at the back of the task set and set up two half-reactions describing what is happening on the anode and cathode of this electrolysis.

A sample of a chloride salt weighing 484.6 mg is titrated with AgNO3 using K2CrO4 as indicator. To reach the end point a 52.3 mL of 0.1475 M of AgNO3 solution is required.    The net ionic equation for the reaction of titration is: Ag+ (aq) + Cℓ- (aq) → AgCℓ (s)    How many moles of Ag+ (aq) ions are used to reach the end point?    How many moles of Cℓ- (aq) have reacted in the titration?    How many grams of chloride are present in the sample?   What is the mass percent of chloride in the sample?

The following chemical reaction takes place in aqueous solution: FeBr2(aq)+Na2S(aq)→FeS(s)+2NaBr(aq) Write the net ionic equation for this reaction.

Which reaction(s) can be identified as a redox reaction? CuO(s) + H₂SO4(aq) → CuSO4(aq) + H₂O(1) Cu(NO3)2(aq) + 2NaOH(aq) -> A →→ Cu(OH)₂(s) + 2NaNO3(aq) Cu(OH)2(s) CuO(s) + H₂O(g) CuSO4(aq) +Zn(s) → ZnSO4(aq) + Cu(s) Cu(s)+ 4HNO3(aq) - Cu(NO3)2(aq) + 2NO₂(aq) + 2H₂O(1)

Molarity of vinegar solution is .8 M

Sodium oxalate, Na2C2O4Na2C2O4, in solution is oxidized to CO2(g)CO2(g) by MnO−4MnO4− which is reduced to Mn2+Mn2+. A 50.3 −mL−mL volume of a solution of MnO−4MnO4− is required to titrate a 0.342 −g−g sample of sodium oxalate. This solution of MnO−4MnO4− is then used to analyze uranium-containing samples. A 4.60 −g−g sample of a uranium-containing material requires 33.0 mLmL of the solution for titration. The oxidation of the uranium can be represented by the change UO2+→UO2+2UO2+→UO22+.     Part A Calculate the percentage of uranium in the sample.