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Answered 2011-05-06 14:15:41

Sodium chloride and Ammonia

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When sodium carbonate is added to hydrochloric acid, sodium chloride is formed, water is formed and carbon dioxide gas is liberated as well.


NaCl salt is formed and H2 gas is given off


Sodium Nitride, whenever you have a salt the Cation is called its normal name 'Sodium' while a 'Ide' is added to the end of the Anion 'Nitrogen' -> 'Nitride'



If Sodium hydroxide is added to Hydrochloric acid the reaction will produce Sodium chloride (common salt) and water.NaOH + HCl = NaCl + H2O


When sodium comes in contact with hydrochloric or any acid, hydrogen gas is released.


There shouldn't be any precipitate. Metathesis between those reactants gives sodium chloride (soluble) and acetic acid (also soluble).



that's because soap contains sodium salt and a mixture of carboxylic acid. when HCL added, percipate formed due to acids are less soluble in water



what would magnesium chloride look like after the reaction MAGNESIUM + HYDROCHLORIC ACID --------> MAGNESIUM CHLORIDE + HYDROGEN




When Hydrochloric Acid is added to Zinc, a product called zinc chloride is formed. Additionally, hydrogen gas (H2) is formed, by an immediate reaction.


When you add sodium hydroxide to hydrochloric acid it reacts to form a neutral salt (NaCl) in solution, once enough acid is added to neutralize all of the base.


The general rule is that when a metal and an acid react, they produce a salt and hydrogen gas. For example:Magnesium + Hydrochloric Acid --> Magnesium Chloride + HydrogenSodium + Hydrochloric Acid --> Sodium Chloride + Hydrogen



2Na (s) + 2HCl (aq) --> 2NaCl (aq) + H2 (g) When sodium is added to hydrochloric acid, the sodium quickly dissolves and you can see some colorless gas bubbles.


yes it will. i did this exact experiment at school, and the temperature drops



The chemical reaction is:NaHCO3 + HCl = NaCl + CO2 + H2O



Fe + 2HCl → FeCl2 + H2↑Iron + Hydrochloric acid → Iron II chloride + Hydrogen gas


A solution of sodium chloride will be formed. It will act as an electrolyte.




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