What is the net ionic equation for the following reaction? Rb2CrO4(aq) + 2AgClO(aq) --> 2RbClO(aq) + Ag2CrO4(s)

Group of answer choices

Rb+(aq) + ClO-(aq) --> RbClO (s)

2Rb+(aq) + CrO42+(aq) --> Rb2CrO4 (s)

Ag+(aq) + ClO-(aq) --> AgClO (s)

2Ag+(aq) + CrO42+(aq) --> Ag2CrO4 (s)

The net ionic equation  is

Ag⁺(aq)  +Cl⁻(aq) →  AgCl(s)

Explanation:

AgNO₃ (aq)  + KCl (aq)→ AgCl(s) +KNO₃(aq)

from above  molecular equation break  all  soluble electrolyte  into ions

Ag⁺(aq) +NO₃⁻ (aq) + K⁺(aq) +Cl⁻(aq) →   AgCl (s) + K⁺(aq) + No₃⁻(aq)

cancel the spectator  ions  in both side  of  equation =K⁺  and NO₃⁻  ions

The net  ionic equation is therefore

= Ag⁺(aq)  + Cl⁻(aq) →    AgCl(s)

in chemistry, a solution’s concentration is how much of a dissolvable substance, known as a solute, is mixed with another substance, called the solvent. the standard formula is c = m/v, where c is the concentration, m is the mass of the solute dissolved, and v is the total volume