Now use the molarity and volume of the hydrochloric acid solution to determine how many moles of acid you have Your goal now is to figure out how many moles of each reactant you're mixing together.įor starters, use silver nitrate's molar mass to determine how many moles you get in that #"1.40-g"# sample of silver nitrate Notice that the reactants take part in the reaction in a #1:1# mole ratio, which means that the reaction will consume equal numbers of moles of silver nitrate and hydrochloric acid, which produce silver cations, #"Ag"^(+)#, and chloride anions, #"Cl"^(-)#, respectively.
The net ionic equation, which you get after removing the spectator ions, looks like this The balanced chemical equation for this reaction looks like this
Silver nitrate, #"AgNO"_3#, a soluble ionic compound, will react with hydrochloric acid, #"HCl"#, a strong acid that dissociates completely in aqueous solution, to form the insoluble silver chloride, #"AgCl"#, a white precipitate. You're dealing with a double replacement reaction in which two soluble compounds react in aqueous solution to form an insoluble solid that precipitates out of solution.
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