When aqueous solutions of NaBr and AGNO3 are mixed, the reaction produces NaNO3(ag) and AgBr(s). What is the net ionic equation for this reaction? Select one: O a. Na*(aq) + Br (aq) + Ag*(aq) + NO3¯paq) → Na*(aq) + NO3¯(aqg) + AgBr(s) O b. NaBr(ag) +Ag*(aq) → Na(s) + AgBr(s) O c. Br (aq) + Ag*(aq) → AgBr(s) O d. NaBr(ag) + AGNO3(aq) → AgBr{s) + NaNO3(aq)

A sample of iron ore is dissolved in acid, and the iron ore is converted to Fe. The sample is then titrated with 57.30 ml or 0.03240 M MnO solution. The oxidation-reduction reaction that occurs during titration is as follows MnO4 (aq) 5 Fe2 (aq) + 8 H (aq) - Mn (ac) SFfe (aq) 4H0 How many grams of iron were in the sample? Select one: O a. 7.631 g O b. 0.5386 g O c. 0.7631 g O d. 5.185 x 101g O e. 2.310 x 101 g

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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.

A useful application of oxalic acid is the removal of rust, Fe2O3.   Fe2O3(s)  +   6 H2C2O4(aq)  →  2 Fe(C2O4)3(aq)  +  3 H2O  + 6 H+(aq)   Calculate the number of grams of rust that can be removed by 500 mL of a 0.100M oxalic acid.

2. If Dr. Dahm wants 450 mL of a solution that has a concentration of 0.357 M HOI (aq). Determine how many grams of ICl are needed. ICI + H₂O(1) H* (aq) + Cl(aq) + HOI(aq)

Based on the balanced chemical equation shown below, determine the concentration (M) of Fe2+(aq) if 40.00 mL of the Fe2+(aq) solution is required to completely react with 43.47 mL of a 0.125 M bromate, BrO3-(aq), solution. The chemical equation for the reaction is 6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) → 6 Fe3+(aq) + Br-(aq) + 3 H2O(l)  Do not type in units nor write in scientific notation.

A sample of iron ore is dissolved in acid, and the iron is converted to Fe2*. The sample is then titrated with 47.20 mL of 0.02240 M MnO4 solution. The oxidation-reduction reaction that occurs during titration is as follows: MnO4(aq) + 5FE2*(aq) + 8H*(aq) → Mn²*(aq) + 5FE3* (aq) + 4H2O How many moles of MnO4¯ were added to the solution? Blank 1 2+ How many moles of Fe were in the sample? Blank 2 How many grams of iron were in the sample? Blank 3 If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample? Blank 4 Blank 1 Add your answer Blank 2 Add your answer Blank 3 Add your answer Blank 4 Add your answer

What is the balanced net ionic chemical equation between Cu^2+ (aq) and I^- (aq)?

A chemist wishes to precipitate iron ions out of a solution of iron (III) nitrate.  Complete balanced equation, total ionic equation and a net ionic equation have been provided. Identify a spectator ion. Complete Balanced Chemical Equation  Fe (NO3)3 (aq) + 3 NaOH (aq)  -->   Fe (OH)3 (s) + 3 NaNO3 (aq) Total Ionic Equation  Fe3+ (aq) + 3 NO3- (aq) + 3Na+ (aq) + 3 OH- (aq) -->  Fe (OH)3 (s) + 3 Na+ (aq) + 3 NO3- (aq) Net Ionic Equation  Fe3+ (aq) + 3 OH- (aq)  -->   Fe (OH)3 (s)     Identify a spectator ion: