Question

unit 4 - part 2: mcq
remember to log your answers onto my ap to earn full credit on this hw assignment. you may omit pg. 6 - 13 from your pdf.

1. a student combines a solution of nacl(aq) with a solution of agno3(aq), and a precipitate forms. which of the following is the balanced net ionic equation for the formation of the precipitate?

a. ag+(aq) + cl-(aq)→agcl(s)
b. na+(aq) + no3-(aq)→nano3(s)
c. nacl(aq) + agno3(aq)→nano3(s) + agcl(aq)
d. nacl(aq) + agno3(aq)→nano3(aq) + agcl(s)

Explanation:

Step1: Write the complete ionic equation

When \(NaCl(aq)\) (which dissociates into \(Na^{+}(aq)\) and \(Cl^{-}(aq)\)) reacts with \(AgNO_{3}(aq)\) (which dissociates into \(Ag^{+}(aq)\) and \(NO_{3}^{-}(aq)\)), the complete ionic equation is \(Na^{+}(aq)+Cl^{-}(aq)+Ag^{+}(aq)+NO_{3}^{-}(aq)\to Na^{+}(aq)+NO_{3}^{-}(aq)+AgCl(s)\)

Step2: Cancel out spectator ions

Spectator ions (\(Na^{+}(aq)\) and \(NO_{3}^{-}(aq)\) as they appear on both sides of the equation) are removed. The net - ionic equation is \(Ag^{+}(aq)+Cl^{-}(aq)\to AgCl(s)\)

Answer:

A. \(Ag^{+}(aq)+Cl^{-}(aq)\to AgCl(s)\)