#color(red)2# in front of NaOH (on the left) and #color(red)2# in front of NaCl (on the right). Here, sodium carbonate (Na2CO3) is added to silver nitrate (AgNO3). Silver nitrate solution is then added to. ![]() AgN O3+HCl AgCl+HN O3 The white precipitate is insoluble in nitric acid but soluble in ammonium hydroxide solution and forms a complex salt called diamine silver (I) chloride. Now, we'll count the number of each groups on both sides: The nitric acid reacts with, and removes, other ions that might also give a confusing precipitate with silver nitrate. Silver nitrate solution reacts with hydrochloric acid and it gives a thick curdy white precipitate of silver chloride. ![]() To illustrate, here's an example of a double displacement reaction: If you are interested in a "simplified" way of balancing double replacement reaction, you can balance "A", "B", "C" and "D", meaning, handling the cations and anions as a group, rather than as individual elements. When the chemical formula for each ionic compounds is written correctly, you can balance the equation like any other chemical equations by making sure the number of atoms for each element is the same on the left and the right. Silver chloride is a white precipitate and nitric acid exists as a aqueous solution. The figure below clearly illustrates how this swap takes place. When aqueous silver nitrate (AgNO3) and aqueous hydrochloric acid (HCl) are reacted, silver chloride (AgCl) precipitate and nitric acid (HNO3) are given as products. ![]() Double replacement reaction occurs when the cations and anions of two ionic compounds are exchanged.
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