Remember that carbonic acid is unstable and decomposes immediately to CO 2( g)+ H 2O( l): So, let’s make a list of steps for predicting the products of ionic reactions.ġ) Identify the ions and write their charge on topĢa) Balance the equation and omit the chargesĢ) Balance the equation and omit the charges:ĢAgNO 3( aq) + CaCl 2( aq) → 2AgCl( s) + Ca(NO 3) 2( aq) Adjust the subscript based on the charges and remember, the overall charge of the compound should balance to zero. To obtain correct formulas, make sure you know the charge of the cation and the formula together with the charge of the anion. We predict the products by combining the cation from each reactant with the anion from the other. Reactions in Aqueous Solutions Practice Problems.Stoichiometry of Reactions in Aqueous Solutions.Molecular, Ionic, and Net Ionic Equations.In the next post, we will talk about the stoichiometry of reactions in aqueous solutions and examples of precipitation and acid-base reactions. Determine the precipitate (in this case AgCl) and label it as ( s) – solid.ĢAgNO 3( aq) + CaCl 2( aq) → 2AgCl( s) + Ca(NO 3) 2( aq)ĪgCl is a solid (precipitate) because the salts of halides are soluble except when combined with Ag +, Pb 2+, and Hg 2 2+.īeing able to predict the products of a reaction is very important partly because it is required for solving problems on determining the amount of the product based on the stoichiometry of the reaction. I.e., we don’t carry the subscript of Cl, but we do for the nitrate since the formulas are Cl – and NO 3 – :Ģ) Place the ionic charges on top of elements and adjust the subscripts:ģ) Balance the equation with coefficients and remove the charges:ĢAgNO 3( aq) + CaCl 2( aq) → 2AgCl + Ca(NO 3) 2Ĥ) Label the soluble compounds as ( aq). Only carry the subscripts that are part of the formula. Let’s use the table of the most common polyatomic ions, and determine the products of the reaction between AgNO 3 and CaCl 2:Ĭomplete and balance the following equation between solver nitrate and calcium chloride:ġ) Exchange the cations and anions. To be able to predict the products of a double displacement reaction, you need to know the formulas and the charges of the ions in the starting materials and use the solubility rules to identify the precipitate in the reaction. These types of reactions are called metathesis or double-displacement reactions. If we compare the formulas of the reactants and products in the previous reaction, we can see that an exchange of ions had occurred the cation of one salt combined with the anion of the other salt and vice versa. Na 2CrO 4( aq) + AgNO 3( aq) → Ag 2CrO 4( s) + NaNO 3( aq) For example, when an aqueous solution of sodium chromate (Na 2CrO 4) is added to an aqueous solution of silver nitrate (AgNO 3), a dark orange precipitate of silver chromate (Ag 2CrO 4) is formed: Precipitation reactions usually involve ionic compounds. In a precipitation reaction, an insoluble product is formed which is called a precipitate.
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