# Write a molecular equation for the precipitation reaction silver nitrate and strontium iodide

All double displacement reactions have the general form: When a double displacement reaction occurs, the cations and anions switch partners, resulting in the formation of two new ionic compounds AD and CB, one of which is in the solid state. The following is a typical problem. Predict whether a precipitate will form when water solutions of silver nitrate, AgNO3 aqand sodium sulfide, Na2S aqare mixed. If there is a precipitation reaction, write the complete and net ionic equation that describes the reaction. Study Sheet Tip-off — When you are asked to predict whether a precipitation reaction takes place when two aqueous solutions of ionic compounds are mixed and to write complete and net ionic equations for the reaction, if it takes place.

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

Predict whether either of the possible products is water insoluble. If either possible product is insoluble, a precipitation reaction takes place, and you will continue with step 3. Follow these steps to write the complete equation. Separate the formulas for the reactants and products with a single arrow.

Write the physical state for each formula. Follow these steps to write the net ionic equation. Write the complete ionic equation by describing water-soluble ionic compounds as separate ions and insoluble ionic compounds with a complete formula.

Eliminate the formulas for the ions that are unchanged in the reaction the spectator ions. Rewrite what is left after the spectator ions are removed.

Determine the possible products using the general double displacement equation. Remember to consider charge when you determine the formulas for the possible products. Therefore, Ag2S would be insoluble. Write the complete equation. Write the net ionic equation.

Describe the solid with a complete formula. Predict whether a precipitate will form when water solutions of barium chloride, BaCl2 aqand sodium sulfate, Na2SO4 aqare mixed. According to our solubility guidelines, most sulfates are soluble, but BaSO4 is an exception.

It is insoluble and would precipitate from the mixture. Write the complete ionic equation, describing the aqueous ionic compounds as ions. Describe the solid as a complete formula.Unlike silver nitrate and sodium chloride, silver chloride isn't water-soluble.

As soon as it forms, it "precipitates," or drops out of solution. The result of mixing silver nitrate and sodium chloride is immediate formation of a white solid that settles to the bottom of the beaker or reaction vessel -- . Consider the reaction between copper metal and silver nitrate solution to form copper nitrate solution and silver metal.

This is called a chemical equation, which shows all the reactants and products in a chemical reaction. Silver nitrate is soluble in water. When writing chemical equations, they are assigned the solid states (s). The potassium ion is "K"^+ and the iodide ion is "I"^-. The two charges balance in a 1: 1 ratio, so potassium iodide is simply "KI".

In lead (II) iodide, the charges balance in a 1: 2 ratio, so the formula is "PbI"_2. Finally, in potassium nitrate, the charges balance in another 1 . Two questions where I have to write a balanced net ionic equation.

1. Write a balanced net ionic equation for the reaction that occurs when aqueous solutions of sodium chromate and silver nitrate are mixed 2. Write a balanced net ionic equaion reaction for ; Chemistry Write a blanaced molecular equation for the reaction 2Na(NO3) + Cu(OH)2.

Silver nitrate (AgNO3) reacts with strontium chloride (SrCl2) in a double displacement reaction. Write the balanced chemical equation which shows this reaction.

Determine the volume (mL) of M sulfuric acid needed to react with g of aluminum to produce aluminum sulfate%(1). I understand about the redox reaction and single displacement happened during the recovery of silver in a silver nitrate solution with copper coil.

Cu + 2 AgNO3 > 2 Ag + (CuNO3) 2 In that reaction, I know that copper II ion is what makes the solution blue.

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