1. Write a balanced molecular equation for the reaction of solid AgNO3 with aque

Question

1. Write a balanced molecular equation for the reaction of solid AgNO3 with aqueous NaCl. Be sure to include the correct number of coefficients and the state of the species (aq, s, l or g).

2. Write the total ionic equation for this reaction, including all physical states.

3. Write the net ionic equation for this reaction, including all physical states.

4. Identify the spectator ions.

5. If the chloride ion is usually soluble, how can solid AgCl form? Identify the rules from Table 4.1 and explain the physical state of the products. (Be sure to discuss the exception to the chloride rule.)

Explanation / Answer

)AgNO3(aq) + NaCl(aq) ---> AgCl(s) + NaNO3(aq)

AgCl precipitated out of solution because it's insoluble in water. We first write the complete ionic equation before we write the net ionic equation. To write the ionic equation, we separate all the aqueous compounds into ions and leave the solid compound unseparated.

Ag+ + NO3- + Na+ + Cl- ---> AgCl(s) + Na+ + NO3-

Then, we omit the spectator ions- the ions that appear on both sides of the equation. We're left now with the net ionic equation

Ag+ + Cl- ---> AgCl(s)

AgNO3 (aq) + NaCl (aq) ---> AgCl (s) + NaNO3 (aq)

net ionic: Cl-1 (aq) + Ag+1 (aq) ---> AgCl (s)

* Net ionic is basically the formula for the solid. If you know what the solid is, then you add the elements that make up the solid (they will both be aqueous) and they go on the left. On the right is the solid (precipitate that forms).

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