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 HCI(aq) and NaOH(aq). Total Ionic: NaOH(aq) + HCI(aq) H_20(l)+ NaCl(aq) Net Ionic: H_30^+ (aq) + OH^- (aq) H_20(l) Assume that you took 44.0 ml of 0.050 M HCI(aq) and 44.0 mL of 0.050 M NaOH(aq) and mixed them together to perform the reaction. List the ions that remain after the reaction is finished. (Choose all that apply). Calculate the molar concentration of each ion. Remember that a dilution occurred when the HCI(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

balanced equation : NaOH (aq) + HCl(aq) ----------------> NaCl(aq) + H2O(l)

total ionic :

Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) -----------------> Na+(aq) + Cl-(aq) + H2O(l)

net ionic :

H+(aq) + OH-(aq) ------------------> H2O(l)

2)

Molar concentration of NaOH = 44 x 0.05 / 44 + 44

= 0.025 M

Molar concentration of each ion = 0.025 M

3) ions remain after the reaction :

OH-

Na+

Cl-

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