Nothing - barium chloride is soluble. You can however precipitate either the barium (e.g. with sodium sulphate, giving barium sulpate, or the chloride, e.g. with silver nitrate giving silver chloride precipitate.
A solution of barium chloride is added to a solution of potassium chromate, a yellow precipitate forms.
The valency of a barium ion is +2. Barium chloride (BaCl2) consists of a barium ion (Ba^2+) and two chloride ions (Cl^-), which gives the overall compound a neutral charge.
One such salt would be aluminum chloride since it is soluble but when reacted with ammonium hydroxide, the insoluble aluminum hydroxide forms a precipitate. Not sure what is meant by "is insoluble in excess", however.
Barium salts, such as barium chloride or barium nitrate, are commonly used to produce a green flame when burned. The green color is a result of the specific wavelength of light emitted by the barium ions during the combustion process.
To prepare a 2 m solution of barium chloride (BaCl₂), you need to know the molarity (moles per liter) and the molecular weight of BaCl₂, which is approximately 208.23 g/mol. For a 2 m solution, you need 2 moles per kilogram of solvent. Since 20 mL is 0.02 kg, you would need 0.04 moles of BaCl₂ (2 moles/kg × 0.02 kg). Multiplying 0.04 moles by the molar mass (208.23 g/mol) gives approximately 8.33 grams of barium chloride.
A solution of barium chloride is added to a solution of potassium chromate, a yellow precipitate forms.
Silver chloride (AgCl) gives a white precipitate. Silver Bromide (AgBr) also gives a white precipitate, though it's a slightly more creamy white than the precipitate formed by AgCl. Silver iodide (AgI) gives a pale yellow precipitate.
Barium gives its two electrons to two chlorine atoms (to form chloride ions) and they form an ionic compound barium chloride.
The test for barium ions involves adding a solution of a sulfate compound (e.g. sodium sulfate) to a solution containing the barium ions. A white precipitate of barium sulfate forms if barium ions are present.
The balanced chemical equation for Barium chloride plus Aluminium sulphate gives Barium sulphate Aluminium chloride is represented as .3BaCl2(aq) + Al2(SO4)3(aq) --> 3BaSO4(ppt) + 2AlCl3(aq).The ppt formed are white in color.
The valency of a barium ion is +2. Barium chloride (BaCl2) consists of a barium ion (Ba^2+) and two chloride ions (Cl^-), which gives the overall compound a neutral charge.
When silver nitrate (AgNO3) is mixed with sodium chloride (NaCl), a white precipitate of silver chloride (AgCl) is formed. This reaction is a double displacement reaction where the silver cation from AgNO3 and the chloride anion from NaCl switch partners to form the insoluble AgCl precipitate.
Chloride anions form a white precipitate of silver chloride when mixed in solution with silver nitrate.
When sodium acetate is added to hydrochloric acid, the resulting precipitate will be sodium chloride. This is due to the reaction between the sodium ions from sodium acetate and the chloride ions from hydrochloric acid.
The reactant ion is likely to be Chloride (Cl-) ions. With AgNO3, Cl- ions form a white precipitate of silver chloride (AgCl). When treated with HCl followed by KSCN, the white precipitate of AgCl dissolves in HCl to form a colorless solution, then reacts with KSCN to form a light red color due to the formation of silver thiocyanate (AgSCN).
The III is there because as a transition metal, iron can have multiple oxidation states. This means iron is 3+. The charge on each Cl is -1, so you need 3. This gives you FeCl3 Next, Barium has 2+ charge, so you need two OH-'s i.e. Ba(OH)2
Ferrous chloride in presence of hydrochloric acid gives brown precipitates of Ferric chloride with potassium permanganate.