OH- + H+ H2O
The ionic equation is:
H+ + [Cl- + Na+]tribune ions+ OH- --> H2O + [Cl- + Na+]tribune ions
When tribune ions are left out you'll get the net ionic equation:
H+ + OH- --> H2O
The products are NaCl and H2O.
This is a neutralization, so the products are: a salt, NaCl, and water.
HCl + NaHCO3 -----> NaCl + H2O + CO2
H+ + Cl- + Na+ + HCO3- ----> Cl- + Na+ + H2O+CO2 (Ionic equation)
H+ + HCO3- ----> H2O+CO2 (Net Ionic Equation)
This is the balanced equation... HCl + NaHCO3 => NaCl + H2O + CO2 All species are a 1:1 molar ratio.
Na2CO3 (aq) + 2HCl (aq) -> 2NaCl (aq) + H2O (l) + CO2 (g)
2 h+ + co3- -> co2 + h2o
CaCl2 + Na2CO3 -----> 2NaCl + CaCO3
NH4+ + Cl- + K+ + OH- --> NH3 + H2O + Cl- + K+ Since the question is not asking for the net ionic equation, spectator ions should be included in the ionic equation as well.
Balanced 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)Cancel out the "spectator" ions, or ions that do not change in structure or charge (on both sides of the equation; "cancel out")Net Ionic Equation:H+ (aq) + OH- (aq) --> H2O(l)User forgot to place the yield arrows (separating products from reactants)
Cl(aq)+Ag(aq)-->AgCl(s) *do not forget to writte the charges on the elements, Cl 1 minus
Na+ and C2H3O2- (acetate) don't react. Only Ag+ and Cl- do so by precipitation: Ag+ + Cl- --> (AgCl)s
So NH4Cl(s) -----> NH4+(aq) + Cl-(aq). As NH4Cl is ionic you can assume it is a solid. Since H2O is polar it reacts with the NH4Cl ion in a way which allows it to dissociate the ion. The oxygen is slightly negative while the hydrogens have a partial positive charge. The negativity of the oxygen in H2O causes the positive charge of the NH4+ molecule to cancel making it no longer attracted to the Cl. The hydrogen in H2O will do the same to the Cl. Once this happens you will have the products stated above in the reaction equation. NH4+ will further react with the water. NH4+ + H2O ---> NH3 + H3O+ . H3O+ is produced rather than OH- because NH4+ is acidic and therefore will donate a hydrogen. Note that because NH4Cl fully dissociates, you do not add in the + H2O in the first equation.
The products are sodium chloride, which remains dissolved, and water. The complete ionic equation is Na+ + OH- + H+ + Cl- --> Na+ + Cl- + H2O The net ionic equation is: H+ + OH- --> H2O
NH4+ + Cl- + K+ + OH- --> NH3 + H2O + Cl- + K+ Since the question is not asking for the net ionic equation, spectator ions should be included in the ionic equation as well.
Na+ + OH- + H+ + Cl- H2O + Na+ + Cl-
i think its 2NaOH + Cl2 ------------> NaClO + NaCl + H2O i think
Balanced Molecular Equation: CaO(aq)+2HCl(aq) --> CaCl2 (aq) + H2O(l) Balanced Total Ionic Equation: Ca(aq)+2 + O(aq)-2 +2H(aq)+ + 2Cl(aq)-2 --> Ca(aq)+2 + 2Cl(aq)-2 + H2O(l) Total Ionic Equation: O(aq)-2 +2H(aq)+ --> H2O(l)
The chemical equation is:Na + OH- + H+ + Cl- = Na+ + Cl- + H2O(l)
Overall ionic equation: K+(aq) +OH-(aq)+ H30+(aq) + Cl-(aq)------>2H20 (l) + K+(aq) + Cl-(aq) Net ionic Equation OH-(aq)+ H30+(aq) ------>2H20 (l)
The chemical equation is:Na + OH- + H+ + Cl- = Na+ + Cl- + H2O(l)
Balanced 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)Cancel out the "spectator" ions, or ions that do not change in structure or charge (on both sides of the equation; "cancel out")Net Ionic Equation:H+ (aq) + OH- (aq) --> H2O(l)User forgot to place the yield arrows (separating products from reactants)
The chemical equation is:Na + OH- + H+ + Cl- = Na+ + Cl- + H2O(l)
Ionic compounds will dissociate completely as ions in water: LiCl (s) ---> Li+(aq) + Cl-(aq)
NaOH(aq) + HCl(aq) ---> H2O(l) + NaCl(aq) Na+ + OH- + H+ + Cl- ---> H2O + Na+ + Cl-