Question

3. Write the complete and the net ionic equations for each acid-base reaction. a. HI (aq) + RbOH (aq) → b. HCHO2 (aq) + NaOH (aq) → C. HC2H302 (aq) + LiOH (aq) → 4. A 30.00-ml solution of H3PO4 of an unknown concentration is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.38 mL of NaOH is added. What is the concentration of the unknown solution of H3PO4? The neutralization reaction is: H3PO4 (aq) + 3NaOH (aq) > 3H20 + Na3PO4 (ag) 5. Complete and balance each equation. Write the complete and the net ionic equations. If no reaction occurs, write "NO REACTION".

I really need some help with number 3 and number 4 if you could also explain the steps I would greatly appreciate it!

Answer 1

Solution:

3) A) Balanced equation will be:

HI(aq) + RbOH(aq) = RbI(s) + H2O(aq)

Total ionic equation will be:

H+(aq)+ I-(aq) + Rb+(aq) + OH-(aq) = RbI(s) + H+(aq) +OH-(aq)

Net ionic equation:

Rb+(aq) + I-(aq) = RbI(s)

B) Balanced molecular equation will be:

HCHO2(aq) + NaOH (aq) = NaCHO2 (aq) + H2O(l)

Total ionic equation:

HCHO2 (aq) + Na+(aq) + OH-(aq) = CHO2-(aq) + Na+(aq) + H2O(l)

Net ionic equation:

HCHO2(aq) + OH-(aq) = CHO2-(aq) + H2O(l)

C) Balanced equation will be:

HC2H3O2(aq) + NaOH(aq) = NaC2H3O2(aq) + H2O(l)

Total ionic equation:

HC3H3O2(aq) + Na+(aq) + OH-(aq) = Na+(aq) + C2H3O2-(aq) + H2O(l)

Net ionic equation:

HC3H3O2(aq) + OH-(aq) = C2H3O2-(aq) + H2O(l)