Write the balanced molecular, complete ionic, and net ionic equations for each of the following acid-base reactions. (Type your answer using the format [NH4]+ for NH4+ and [Ni(CN)4]2- for Ni(CN)42-. Use the lowest possible coefficients.)
(a) HClO4(aq) + Mg(OH)2(s)
molecular equation, complete ionic, net ionic
(b) HCN(aq) + NaOH(aq)
molecular equation, complete ionic, net ionic
(c) HCl(aq) + NaOH(aq)
molecular,complete ionic, net ionic
These look easy enough to balance. What is your problem? What is it you don't understand? Follow the rule of
acid + base ==> salt + HOH
aqueous strontium hydroxide and hydroiodic acid net equation
(a)
Molecular equation: HClO4(aq) + Mg(OH)2(s) -> Mg(ClO4)2(aq) + H2O(l)
Complete ionic equation: 2H+(aq) + ClO4-(aq) + Mg2+(aq) + 2OH-(aq) -> Mg(ClO4)2(aq) + 2H2O(l)
Net ionic equation: 2H+(aq) + 2OH-(aq) -> 2H2O(l)
(b)
Molecular equation: HCN(aq) + NaOH(aq) -> NaCN(aq) + H2O(l)
Complete ionic equation: H+(aq) + CN-(aq) + Na+(aq) + OH-(aq) -> Na+(aq) + CN-(aq) + H2O(l)
Net ionic equation: H+(aq) + OH-(aq) -> H2O(l)
(c)
Molecular equation: HCl(aq) + NaOH(aq) -> NaCl(aq) + H2O(l)
Complete ionic equation: H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) -> Na+(aq) + Cl-(aq) + H2O(l)
Net ionic equation: H+(aq) + OH-(aq) -> H2O(l)
(a) Let's start by writing the balanced molecular equation for the reaction between HClO4(aq) and Mg(OH)2(s):
HClO4(aq) + Mg(OH)2(s) → Mg(ClO4)2(aq) + H2O(l)
To write the complete ionic equation, we need to break down the aqueous compounds into their respective ions:
H+(aq) + ClO4-(aq) + Mg2+(aq) + 2OH-(aq) → Mg2+(aq) + 2ClO4-(aq) + 2H2O(l)
Next, we can cancel out the spectator ions that appear on both sides of the equation. In this case, the spectator ions are Mg2+ and ClO4-.
H+(aq) + OH-(aq) → H2O(l)
The resulting equation is the net ionic equation for the reaction.
(b) Now let's write the balanced molecular equation for the reaction between HCN(aq) and NaOH(aq):
HCN(aq) + NaOH(aq) → NaCN(aq) + H2O(l)
Breaking down the aqueous compounds into their respective ions, the complete ionic equation is:
H+(aq) + CN-(aq) + Na+(aq) + OH-(aq) → Na+(aq) + CN-(aq) + H2O(l)
Again, we can cancel out the spectator ions, which are Na+ and CN-:
H+(aq) + OH-(aq) → H2O(l)
Therefore, the net ionic equation for this reaction is the same as the complete ionic equation.
(c) Lastly, let's write the balanced molecular equation for the reaction between HCl(aq) and NaOH(aq):
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
Breaking down the aqueous compounds into their respective ions, the complete ionic equation is:
H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) → Na+(aq) + Cl-(aq) + H2O(l)
Once again, we can cancel out the spectator ions, which are Na+ and Cl-:
H+(aq) + OH-(aq) → H2O(l)
Thus, the net ionic equation for this reaction is the same as the complete ionic equation.