Item 13 Reactions between ionic compounds often result in the precipitation of a

Question

Item 13

Reactions between ionic compounds often result in the precipitation of an insoluble compound. Spectator ions and precipitation products of a chemical reaction can be predicted by consulting an ionic substance solubility table. Here is one such table:

Entering chemical equations

Add phases to all chemical reactions unless asked otherwise. When adding phases, make sure not to place them as a subscript.

Do not stack charges and subscripts. To add a charge to an ion with a subscript, first enter the subscript. For example, to type SO42 start by typing SO4 . Then use the arrow key to arrow over before adding a superscript with the charge.

Part A

What is the net ionic equation of the reaction of FeCl2 with NaOH ?

Express you answer as a chemical equation including phases.

Part B

What is the net ionic equation of the reaction of MgSO4 with Ba(NO3)2 ?

Express you answer as a chemical equation including phases.

Item 13

In many chemical reactions of two or more compounds, ions are present in the solution that do not participate in the reaction. These ions, known as spectator ions, can be removed from the chemical equation describing the reaction. A chemical equation that has the spectator ions removed is known as a net ionic equation.

Reactions between ionic compounds often result in the precipitation of an insoluble compound. Spectator ions and precipitation products of a chemical reaction can be predicted by consulting an ionic substance solubility table. Here is one such table:

Rule General trend 1 Most salts containing alkali metal or ammonium (NH4+) cations are soluble. 2 Most salts containing NO3 are soluble. 3 Most salts containing Cl , Br , and I are soluble, except with metals such as Ag+ , Pb2+ , and Hg22+ . 4 SO42 salts with +1 cations and Mg2+ are soluble, but with most +2 cations these salts are insoluble. 5 Most compounds with OH anions and group 1 or 2 cations are soluble. Notable exceptions are Be(OH)2 and Mg(OH)2 .

Entering chemical equations

When entering chemical equations, please follow the following formatting guidelines

Add phases to all chemical reactions unless asked otherwise. When adding phases, make sure not to place them as a subscript.

Do not stack charges and subscripts. To add a charge to an ion with a subscript, first enter the subscript. For example, to type SO42 start by typing SO4 . Then use the arrow key to arrow over before adding a superscript with the charge.

If you make a formatting error, you will see an message such as "Check your placement of subscripts and superscripts." or "There is an error in your submission. Make sure you have formatted it properly." You will not lose any credit, but the answer will need to be edited and re-submitted.

Part A

What is the net ionic equation of the reaction of FeCl2 with NaOH ?

Express you answer as a chemical equation including phases.

Part B

What is the net ionic equation of the reaction of MgSO4 with Ba(NO3)2 ?

Express you answer as a chemical equation including phases.

Explanation / Answer

Part A

What is the net ionic equation of the reaction of FeCl2 with NaOH ?

FeCl2(aq) + 2NaOH(aq) = Fe(OH)2(s) + 2NaCl(aq)

bet ionic contains those ions being precipitated so

Fe+2(aq) + 2OH-(aq) = Fe(OH)2(s)

Express you answer as a chemical equation including phases.

Part B

What is the net ionic equation of the reaction of MgSO4 with Ba(NO3)2 ?

Mg+2(aq) + SO4-2(aq) + Ba+2(aq) + 2NO3-(aq) = BaSO4(s)(aq) + Mg+2(aq) + 2NO3-(aq)

Net ionic contains only reacting ions

SO4-2(aq) + Ba+2(aq) = BaSO4(s)(aq)

Express you answer as a chemical equation including phases.

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