Ammonium chloride is soluble in water. Silver chloride is not soluble in water and will form a white precipitate in an aqueous solution.
their colours, a white precipitate for silver chloride, and a yellow precipitate for silver iodine
The products are Silver chloride (a white precipitate) and potassium ethanoate (acetate). NB THis is a classic test for halides.
The correct name for AgCl is silver chloride. Its IUPAC name is chlorosilver. Other names for silver chloride are cerargyrite, chlorargyrite, and horn silver.
Silver (I) Chloride and Potassium Acetate. All one has to do to solve this problem is to switch the anions and the cations.
The silver in the Silver Nitrate precipitates the chloride ions out of the ammonium chloride solution, leaving Ammonium Nitrate in solution and a Silver Chloride solid.
One way to differentiate between iron chloride and sodium chloride solutions is to perform a chemical test using silver nitrate. Iron chloride solution will form a white precipitate of silver chloride, while sodium chloride solution will not react with silver nitrate. Another method is to use a flame test: iron chloride imparts a yellow color to the flame, while sodium chloride does not.
their colours, a white precipitate for silver chloride, and a yellow precipitate for silver iodine
Silver chloride: AgCl
For example the product of the reaction between sodium chloride and silver nitrate is the insoluble silver chloride.
Silver chloride is not a nonmetal but a chemical compound formed between silver and chlorine. Silver is a metal and chlorine is a nonmetal, so silver chloride can be considered an inorganic compound.
When silver nitrate is titrated against potassium chloride, a white precipitate of silver chloride is formed due to the reaction between silver ions from silver nitrate and chloride ions from potassium chloride. This reaction can be used to determine the concentration of chloride ions in a solution.
Silver Chloride AgCl
There would be no reaction because they are both chlorides.
First, calculate the moles of silver nitrate in the solution using Molarity = moles/volume. Then, use the balanced chemical equation between silver nitrate and silver chloride to determine the moles of silver chloride that can be produced. Finally, convert the moles of silver chloride to grams using the molar mass of silver chloride.
The products are Silver chloride (a white precipitate) and potassium ethanoate (acetate). NB THis is a classic test for halides.
When sodium chloride is added to a solution of silver nitrate (both are very soluble in water), silver chloride, which is only very slightly soluble, will precipitate.
Silver chloride has ionic bonds. The electrostatic attraction between the positively charged silver cation and the negatively charged chloride anion holds the compound together.