predict the outcome of mixing aqueous solutions of the following reactions. write the ionic equations of each.

mercury (ll) nitrate + ammonium iodide
manganese (ll) chloride + sodium sulfide
lead (ll) nitrate + sodium sulfate
barium nitrate + lithium sulfate
aluminum sulfate + sodium hydroxide

nope

To predict the outcome of mixing aqueous solutions, we need to determine if a reaction will occur based on the solubility rules. If there is a potential reaction, we can then write the balanced molecular equation and the corresponding ionic equations.

Let's go through each reaction:

1. Mercury (II) Nitrate + Ammonium Iodide:
First, determine the solubility of the two compounds:
Mercury (II) Nitrate - All nitrates are generally soluble.
Ammonium Iodide - All ammonium salts are generally soluble, and iodides are also generally soluble except for AgI, PbI2, and Hg2I2.

Since both compounds are soluble, a reaction will potentially occur. The balanced molecular equation is:
Hg(NO3)2 + 2NH4I → HgI2 + 2NH4NO3

Breaking down the equation into ionic form, we have:
Hg2+ + 2NO3- + 2NH4+ + 2I- → HgI2 + 2NH4+ + 2NO3-

Note that the ammonium ions (NH4+) are spectator ions and do not participate in the reaction.

2. Manganese (II) Chloride + Sodium Sulfide:
Manganese (II) Chloride - Most chlorides are soluble, including MnCl2.
Sodium Sulfide - All sodium salts are soluble, and sulfides are generally insoluble, except for those of alkali metals and ammonium.

Since manganese (II) chloride and sodium sulfide are both soluble, no reaction occurs.

3. Lead (II) Nitrate + Sodium Sulfate:
Lead (II) Nitrate - All nitrates are generally soluble.
Sodium Sulfate - All sodium salts are soluble, and sulfates are generally soluble except for PbSO4, BaSO4, and SrSO4.

Based on the solubility rules, a reaction will occur. The balanced molecular equation is:
Pb(NO3)2 + Na2SO4 → PbSO4 + 2NaNO3

Breaking down the equation into ionic form, we have:
Pb2+ + 2NO3- + 2Na+ + SO42- → PbSO4 + 2Na+ + 2NO3-

4. Barium Nitrate + Lithium Sulfate:
Barium Nitrate - All nitrates are generally soluble.
Lithium Sulfate - All lithium salts are soluble, and sulfates are generally soluble except for PbSO4, BaSO4, and SrSO4.

Based on the solubility rules, a reaction will occur. The balanced molecular equation is:
Ba(NO3)2 + Li2SO4 → BaSO4 + 2LiNO3

Breaking down the equation into ionic form, we have:
Ba2+ + 2NO3- + 2Li+ + SO42- → BaSO4 + 2Li+ + 2NO3-

5. Aluminum Sulfate + Sodium Hydroxide:
Aluminum Sulfate - All sulfates are generally soluble, including Al2(SO4)3.
Sodium Hydroxide - All alkali metal hydroxides are soluble, including NaOH.

A reaction will occur. The balanced molecular equation is:
Al2(SO4)3 + 6NaOH → 2Al(OH)3 + 3Na2SO4

Breaking down the equation into ionic form, we have:
2Al3+ + 3SO42- + 6Na+ + 6OH- → 2Al(OH)3 + 3Na2SO4

Note: It's important to consider the charges and valences of the elements when writing ionic equations.

Remember to always consult solubility rules and consider the charges of ions to determine if a reaction will occur and to write the correct balanced molecular and ionic equations.

The secret here is to know the solubility rules. Here is a simplified set for you to memorize.

http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html

Here is an example.
#3.
Pb(NO3)3(aq) + Na2SO4(aq) ==> PbSO4(s) + 2NaNO3(aq)

The net ionic equation is
Pb^2+(aq) + SO4^2-(aq) ==> PbSO4(s). This reaction takes place BECAUSE PbSO4 is insoluble in water. All of the others have a ppt to form as a product, also.