mesured mass-mass by subtraction/mass by subtraction * 100%
NH4Cl
3Cu^2+(aq) + 2PO4^3-(aq)====>Cu3(PO4)2(s)
you have to write... 2KI + Cl2 = 2KCl + I2
4 LiH + AlCl3 =======> LiAlH4 + 3 LiCl
Ammonium carbonate, (NH4)2CO3 dissolves in water releasing the ammonium ion, NH4+, and carbonate ion, CO32- into solution. Both of these ions hydrolyze (react with water). The chemical equations describing the hydrolysis reactions are given. By adding these reactions one can write the overall balanced net ionic equation for the reaction that occurs when ammonium carbonate dissolves in water. Write the overall balanced net ionic equation, calculate the equilibrium constant, write the overall equilibrium expression, and calculate the carbonate ion concentration, [CO32-], of a 1.0 mol/L solution of ammonium carbonate. (Hint: this requires solving a quadratic equation)... --Equations (1) (NH4)2CO2 (aq) --> 2NH2+ + CO32- (2) NH2+ + H2O(l) <--> NH2(aq) + H2O+ Ka=5.6x10-10 (3) CO32- + H2O(l) <--> HCO3- + OH- Kb=2.1x10-4
NH4Cl
3Cu^2+(aq) + 2PO4^3-(aq)====>Cu3(PO4)2(s)
NH4+ and Cl- don't react, Only SO42- and Ba2+ do so by forming precipitate: SO42- + Ba2+ --> (BaSO4)s
NH3(g) + HCl(g) ==> NH4Cl(s). This type of reaction is called "synthesis". The two gases react to form a solid ammonium chloride salt.
NH3Cl, (careful how you write it) is nothing. Although for most purposes the existence NH3Cl+ can be ignored, it does exist. It can be prepared as a salt with an appropriate cation. However it is may not be very stable. NH4Cl+ is ammonium chloride.
you have to write... 2KI + Cl2 = 2KCl + I2
The chemical equation is:K2CO3 + CaCl2 = CaCO3(s) + 2 KCl
2KClO3 ----> 2KCl + 3O2
4 LiH + AlCl3 =======> LiAlH4 + 3 LiCl
2Al + 3CuCl2 --> 3Cu + 2AlCl3
The equation is:2 Zn + Cl2 = 2 ZnClZinc chloride has many applications: soldering flux, fingerprint detection with ninhydrin, paper industry, disinfectant in medicine etc.
Ammonium carbonate, (NH4)2CO3 dissolves in water releasing the ammonium ion, NH4+, and carbonate ion, CO32- into solution. Both of these ions hydrolyze (react with water). The chemical equations describing the hydrolysis reactions are given. By adding these reactions one can write the overall balanced net ionic equation for the reaction that occurs when ammonium carbonate dissolves in water. Write the overall balanced net ionic equation, calculate the equilibrium constant, write the overall equilibrium expression, and calculate the carbonate ion concentration, [CO32-], of a 1.0 mol/L solution of ammonium carbonate. (Hint: this requires solving a quadratic equation)... --Equations (1) (NH4)2CO2 (aq) --> 2NH2+ + CO32- (2) NH2+ + H2O(l) <--> NH2(aq) + H2O+ Ka=5.6x10-10 (3) CO32- + H2O(l) <--> HCO3- + OH- Kb=2.1x10-4