It actually reacts with AgCl to produce NaCl (which is soluble), and some Na3[Ag(S2O3)2]complexes which are also soluble in water.
Cl(aq)+Ag(aq)-->AgCl(s) *do not forget to writte the charges on the elements, Cl 1 minus
Bromide: Ag+ + Br- = AgBr which is a cream precipitate Chloride: Ag+ + Cl- = Ag Cl which is a white precipitate Iodide: Ag+ + I- = AgI which is a yellow precipitate
The balanced equation is: Ag+ (aq) + Cl- (aq) → AgCl(s)
Salt (NaCl) is white, solid, salty, soluble in water, usually found in small granules, etc. Sodium (Na) is a silver/white, highly reactive alkali metal. Chlorine (Cl) is a greenish gas, and a halogen.
p-chlorophenol forms salt with a base which is soluble in water. Cl-C6H4-OH + NaOH = Cl-C6H4-O-Na+ + H2O
slightly
slightly
It would come out to Ag^+ + Cl^- = AgCl Remember solubility rules nitrate and Ca both are soluble therefore they are not in the final equation.
For sodium and potassium bromide is more soluble than chloride.
Ag +1, Cl -7
How many moles is in 0.0688 Ag Cl
Sodium chloride is dissolved and dissociated in water: NaCl--------------Na+ + Cl-
You think probable to sodium chloride and bromide.
Ag+ + NO-3 + Na+ + Cl----------NaNO3 (aq) + AgCl (white precipitate)
Sodium chloride disassociates in water to produce Na+ and Cl - ions. NaCl + H2O = Na+ aq and Cl- aq.
Table salt, or NaCl (Sodium Chloride) will dissolve in water.
Cl(aq)+Ag(aq)-->AgCl(s) *do not forget to writte the charges on the elements, Cl 1 minus