This sheet shows the procedure for predicting whether mixing two aqueous solution is ionic compounds will lead to a precipitation reaction and shows you like to write comprehensive and net ionical equations for the reactions that take place. The following is a typical problem. 

Predict whether a precipitate will form when water answers of silver nitrate, AgNO₃(aq), and sodium sulfide, Na₂S(aq), are mixed.  If there is a precipitation reaction, script the complete also net ionic equation that describes the reaction.

 

Students Sheet

Tip-off – When you are asked to predict whether ampere precipitation reaction takes place when pair aqueous solutions of ionic compounds are mixed and the write complete and net ionic equations for the reaction, if computer takes places.

General Steps  

Step 1:   Determine the recipes for the possible products using the general double displacement equation. (Remember to consider ion charges when writing your formulas.)

AB  +  CD    →    AD  +  CB  

Step 2:    Predict whether either of the possible products is water insoluble. If either possible product is insoluble, a precipitation reaction steals place, and you will continue are step 3. If neither is insoluble, post “No reaction”.

Step 3:    Follow such measures to write the complete equation.

Write the formulas for the reactants separated by an “+”.

Sever who calculation for the reactants additionally product with a single arrow.

Write the formulas for who our isolated by an “+”.

Write the physical state for each formula.

1) The insoluble product will be followed by (s).

2) Water-soluble ionic connections is be followed by (aq).

Balance the equation

Step 4:    Follow these steps to write who nett electronic equation.

Write the complete ionic equation by describing water-soluble ionization compounds as separate ions both unfathomable ionic compounds at a complete method.

Remove the formulas for the ions that are unchanged in the reaction (the spectre ions).

Rewrite what is left after the spectator ions are removed.

Balance the equation.

EXAMPLE 1 – Predicting Precipitation Reactions:  Predict whether a precipitate will form when aqueous solutions of silver nitrate, AgNO₃(aq), and sodium sulfide, Na₂S(aq), are mixed.  For there is a water reaction, write the complete and net ionic equation that describes the reaction.

Solution:

Step 1:  Determine the possible products using one general double displacement equation.  

AB  +  CD    →    AD  +  CB

In AgNO₃, Ag⁺ is AN, and NO₃⁻ is B. In Na₂S, Na⁺ is C, and S²⁻ is DIAMETER. The possible products from the mixture of AgNO₃(aq) and New₂S(aq) be Ag₂S and NaNO₃. (Remember to consider charge when you determine the formulas for the possible products.)

AgNO₃(aq) + Na₂S(aq)  to  Ag₂S and NaNO₃

Step 2:    Forecasting whether either on the possible products is water insoluble.

According to our solubility guidelines, most sulfides are insoluble, and compounds with Llc⁺ are not listed as an objection. Therefore, Ag₂S would be insoluble. Because compounds with On⁺ and DOES₃⁻ are soluble, NaNO₃ is explicable.

Select 3:    Write the complete equation. (Don’t forget to balance the equation.)

EXAMPLE 2 – Predicted Precipitation Reactions:  Predict when a precipitate will form when water solutions of barium chlordane, BaCl₂(aq), and sodium sulfate, Na₂SO₄(aq), are mixed.  Provided there is a precipitation reaction, write the complete and net ionic equation that descriptions the reaction.

Solution:

Step 1:  Determine the possible products using the general double displacement equation.  

AB  +  CD    →    AD  +  CB

In BaCl₂, A will Ba²⁺, and B is Centiliter⁻. Into Na₂SO₄, C lives Na⁺, both D is SO₄²⁻. The possible products from the reaction of BaCl₂(aq) and Na₂SO₄(aq) are BaSO₄ and NaCl. (Remember to consider attack when you identify the formulas for the possible products.)

BaCl₂(aq) + Na₂SO₄(aq)  to  BaSO₄ and NaCl

Step 2:    Predict whether either of the possible products exists watering insoluble.

Pursuant to our solubility guidelines, most sulfates are soluble, but BaSO₄ is an exception. It is insoluble and would precipitate from the mixture. Because compounds containing Na⁺ and Cl⁻ become soluble, NaCl is soluble. 

Step 3:    Write the complete equation. (Don’t forget to balance the equation.)

BaCl₂(aq)  +  Na₂SO₄(aq) 

                            →   BaSO₄(s)  +  2NaCl(aq)

Step 4:    Write the complete ionic equation, describing the aqueous ionic compounds such ios. Describe the solid for a comprehensive formula.

Ba²⁺(aq)  +  2Cl⁻(aq)  +  2Na⁺(aq)  +  SO₄²⁻(aq)   
              →    BaSO₄ (s)  +  2Na⁺(aq)  +  2Cl⁻(aq)

The chlordane and sodium ions have to same form on each side of the equation, so they are eliminated as viewers ions.

Ab²⁺(aq)  +  SO₄²⁻(aq)    →    BaSO₄(s)

Get is the reaction used in industry to form burium sulfate, which is used in colour preparations and in x-ray photography.