A redox titration of 150.0 mL of 0.110 M CrSO4 with 0.110 M KMnO₄ was performed at 25 °C with its pH being maintained at 2.50 using a suitable buffer. One half of an electrochemical cell is made up of the solution in contact with a platinum electrode. The other half-cell is a standard hydrogen electrode. The two half-cells are joined by a wire and a salt bridge, and the cell potential is measured with a voltmeter to track the titration's progress. If the expected products are Cr³⁺ and Mn²⁺, what is the net ionic equation for the titration reaction?

Select the correct statement:

For the reaction HCHO_2(aq) + Na₂CO_3(aq) → NaCHO_2(aq) + CO_2(g) + H₂O_(l), provide the balanced complete and net ionic equations.

Which statement below best describes net ionic equations?

a) obtained when the ions forming the solids are removed from complete ionic equation

b) lists all the ions present in the solution

c) all substances are shown except for spectator ions; substances as compounds, no ions

d) all substances are shown except for spectator ions; substances as ions if soluble and compounds if insoluble

When the contents of two beakers are mixed together, identify the spectator ions in the reaction that occurs. Make sure to write balanced molecular and net ionic equations.

Beaker 1: silver ion and nitrate ion

Beaker 2: potassium ion and iodide ion

A solution contains one or more of the following ions: Ag⁺, Ca²⁺, and Cu²⁺. When you add sodium chloride to the solution, no precipitate forms. When you add sodium sulfate to the solution, a white precipitate forms. You filter off the precipitate and add sodium carbonate to the remaining solution, producing another precipitate. Write net ionic equations for the formation of each of the precipitates observed.