Write the balanced total ionic equation and the net ionic equation (including ph

Question

Write the balanced total ionic equation and the net ionic equation (including phase labels) for the reaction between HCl(aq) and NaOH(aq). Toatal Ionic: Net Ionic: Assume that you took 39.0 mL of 0.050 M HCl(aq) and 39.0 mL of 0.050 M NaOH(aq) and mixed them together to perform the reaction. List the ions that remain after the reaction finished. (Choose all that apply) H^+(aq) OH^-(aq) Cl^-(aq) Na^+(aq) H_3O^+(aq) H_2)(l) Calculate the molar concentration of each ion. Remember that a dilution occurred when the HCl(aq) and the NaOH(aq) solutions were combined. Notice: In this case, it doesn't matter which ions remain, they would all have the same concentration, so you need only enter in one answer regardless of what you chose in the multiple choice question.

Explanation / Answer

HCl (aq) + NaOH (aq)-----> NaCl (aq) + H2O (l)

to get the net ionic equation ..you need to break all the aqueous species into ions

hence we have

H+ + Cl- + Na+ + OH- -----> Na+ + Cl- + H2O

cross out ions that appear on both side of the equation ..these are called as spectator ions

so when we cancel out the common ions we have

H+ + OH- ----> H2O

that is nothing but a neutralization reaction ...

2)

as you can see the spectator ion will remain which got cancelled out in the net ionic equation ....as they have no role to play

so the species left =

Cl- (aq), Na+ (aq)

H2O (l) will remain but it says all the ions ..and H2O is not an ion....

ii)

the conc of Na+ and Cl- has to be found out ...

since the total number of species remains same ...as they are spectator ions ..the onlt thing that happend was their dilution ...and that too they are diluted to equal volume .... hence all we have to do is to divide the conc of Na+ from NaOH or Cl- from HCl by 2 to get the conc

hence conc =

0.05/2

= 0.025 M fo Na+(aq) and Cl- (aq)each

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