Write the total ionic and net ionic equations for each of the following reactions:
A) hydrobromic acid with potassium hydroxide
B) Nitric acid with barium hydroxide
molecular equation:
HBr(aq) + KOH(aq) ==> KBr(aq) + H2O(l)
total ionic:
H^+(aq) + Br^-(aq) + K^+(aq) + OH^-(aq) ==> K^+(aq) + Br^-(aq) + H2O(l)
net ionic equation: just cancel the ions common to both sides. What's left is the NET ionic equation.
H+(aq) + OH^-(aq) ==> H2O(l)
The other equation is just another acid/base reaction.
Ba(OH)2(aq) + 2HNO3(aq) ==> Ba(NO3)2(aq) + 2H2O(l)
To write the total ionic and net ionic equations for each reaction, we need to first balance the chemical equation and then separate all the reactants and products into their respective ions.
A) Hydrobromic acid (HBr) reacts with potassium hydroxide (KOH):
The balanced chemical equation is:
HBr + KOH → KBr + H2O
Now let's separate the compounds into their respective ions:
HBr (aq) → H+ (aq) + Br- (aq)
KOH (aq) → K+ (aq) + OH- (aq)
KBr (aq) → K+ (aq) + Br- (aq)
H2O (l)
Total Ionic Equation:
H+ (aq) + Br- (aq) + K+ (aq) + OH- (aq) → K+ (aq) + Br- (aq) + H2O (l)
Net Ionic Equation:
H+ (aq) + OH- (aq) → H2O (l)
B) Nitric acid (HNO3) reacts with barium hydroxide (Ba(OH)2):
The balanced chemical equation is:
2HNO3 + Ba(OH)2 → Ba(NO3)2 + 2H2O
Now let's separate the compounds into their respective ions:
2HNO3 (aq) → 2H+ (aq) + 2NO3- (aq)
Ba(OH)2 (aq) → Ba2+ (aq) + 2OH- (aq)
Ba(NO3)2 (aq) → Ba2+ (aq) + 2NO3- (aq)
2H2O (l)
Total Ionic Equation:
2H+ (aq) + 2NO3- (aq) + Ba2+ (aq) + 2OH- (aq) → Ba2+ (aq) + 2NO3- (aq) + 2H2O (l)
Net Ionic Equation:
2H+ (aq) + 2OH- (aq) → 2H2O (l)
In both cases, the net ionic equations involve the combination of H+ and OH- ions to form water (H2O) as a neutral product.