Reddish precipitate of Mercuric iodide and clear solution of Potassium chloride is produced
no
Potassium chloride and Iodine
In aqueous solution they would not react. They would form a solution of ferric ions, chloride ions, potassium ions, and iodide ions.
Since potassium iodide is ionically bonded, it does not technically have a molecular formula. The corresponding characteristic for ionically bonded compounds is a "formula unit", and for potassium iodide, this is KI
Chlorine, a more reactive halogen would displace iodide in its hallide solution. Potassium chloride would be formed.
no
Worded Equation; Potassium Iodide + Calcium Chloride ------> Potassium Chloride + Calcium Iodide Chemical Equation; KI (l) + CaCl (l) -----> KCl (aq) + Ca(I)2 (aq) Note Answer is only correct if proper states are applied and used.
Potassium chloride and Iodine
Sodium chloride (NaCl) is table salt. Additives may include potassium chloride and potassium iodide.
In aqueous solution they would not react. They would form a solution of ferric ions, chloride ions, potassium ions, and iodide ions.
Since potassium iodide is ionically bonded, it does not technically have a molecular formula. The corresponding characteristic for ionically bonded compounds is a "formula unit", and for potassium iodide, this is KI
Chlorine, a more reactive halogen would displace iodide in its hallide solution. Potassium chloride would be formed.
ammonobasic mercuric iodide
Mercuric or mercury II chloride is HgCl2
I would guess that this is so because of potassium's mass, being much more than, sodium's molar mass per ion. So can sodium iodide be used instead of potassium iodide? Perhaps, but maybe not to the same level effectiveness. Potassium molecules have been known to dissolve better than sodium molecules. One example is Potassium Chloride and Sodium Chloride thanks
sugar, table salt, sodium sulphate, fructose, potassium chloride, potassium iodide, sodium iodide, uranyl nitrate, etc.
Formula: HgI2