Other than a specific confirmatory test, give a simple test that would allow you to distinguish between the following pairs of anions and cations. Tell what you would do and what you should observe for each anions and cations.

Anions:
a. CO3 2- and NO3 -
b. Br- and NO3-
c. Cl- and SO4 2-
d. S2 - and I -
Cations:
a. Ag+ and Cu 2+
b. Ca 2+ and Zn 2+
c. Fe 3+ and Al 3+
d. Al 3 + and Zn 2+

This is really a question you need to know how to answer. It is a good test of the chemistry you know. For example,

a. Most carbonates are insoluble. Most nitrates are soluble. So try dissolving in water.
c. Cl and SO4. Add BaCl2. The sulfate gives a white ppt of BaSO4.

cations:
c. Most Fe^+3 solutions have a reddish brown color. Most Al^+3 solutions are colorless.

To distinguish between different pairs of anions and cations, you can utilize some simple tests that can provide observable differences. Here's how you can differentiate between the specified pairs:

1. Anions:
a. CO3 2- and NO3 -
- Test: Add a small amount of dilute hydrochloric acid (HCl) to each anion separately.
- Observation: CO3 2- will produce effervescence (bubbling) due to the release of carbon dioxide gas (CO2). NO3 - will not produce any observable reaction.

b. Br- and NO3 -
- Test: Add a small amount of silver nitrate (AgNO3) solution to each anion separately.
- Observation: Br- will form a yellowish precipitate of silver bromide (AgBr), whereas NO3 - will not show any precipitate.

c. Cl- and SO4 2-
- Test: Add a small amount of barium chloride (BaCl2) solution to each anion separately.
- Observation: Cl- will form a white precipitate of silver chloride (AgCl), while SO4 2- will form a white precipitate of barium sulfate (BaSO4).

d. S2 - and I -
- Test: Add a small amount of lead nitrate (Pb(NO3)2) solution to each anion separately.
- Observation: S2 - will form a black precipitate of lead sulfide (PbS), while I - will form a yellow precipitate of lead iodide (PbI2).

2. Cations:
a. Ag+ and Cu 2+
- Test: Add a small amount of hydrochloric acid (HCl) to each cation separately.
- Observation: Ag+ will not produce any observable reaction, while Cu 2+ will produce a brown gas due to the formation of copper chloride (CuCl2).

b. Ca 2+ and Zn 2+
- Test: Add a small amount of sodium hydroxide (NaOH) solution to each cation separately.
- Observation: Ca 2+ will form a white precipitate of calcium hydroxide (Ca(OH)2), while Zn 2+ will not show any visible precipitate.

c. Fe 3+ and Al 3+
- Test: Add a small amount of sodium hydroxide (NaOH) solution to each cation separately.
- Observation: Fe 3+ will form a reddish-brown precipitate of iron(III) hydroxide (Fe(OH)3), while Al 3+ will form a white precipitate of aluminum hydroxide (Al(OH)3).

d. Al 3+ and Zn 2+
- Test: Add a small amount of sodium hydroxide (NaOH) solution to each cation separately.
- Observation: Al 3+ will form a white precipitate of aluminum hydroxide (Al(OH)3), while Zn 2+ will not show any visible precipitate.

Remember, these tests provide general indications and may not be definitive or conclusive. If accurate identification is crucial, it's recommended to use specific confirmatory tests or consult a trained professional.