5 drops of AgNO3 must be added to 1 L of a water sample: 46.1 mg SO42-/L and 30.6 mg Cl -/L.

What will be the precipitate that forms?

You need to know the molarity of the AgNO3 being added.

sorry, the molarity was .0010 M (moles/Liter)

5 drops : 1 drop = 0.5 mL

See above at your re-post.

To determine the precipitate that forms when 5 drops of AgNO3 are added to a water sample containing 46.1 mg SO42-/L and 30.6 mg Cl -/L, we need to consider the solubility rules for common ions.

1. Start by determining the ions present in AgNO3. AgNO3 dissociates into Ag+ and NO3- ions.

2. Next, consider the possible combinations of these ions with the ions present in the water sample. The possible combinations are Ag+ with SO42- and Ag+ with Cl-.

3. Refer to the solubility rules to determine if any of these combinations will form a precipitate.

- Solubility rule 1: Most nitrate (NO3-) salts are soluble.
- Solubility rule 4: Most sulfate (SO42-) salts are soluble, except those of silver, lead, barium, and strontium.
- Solubility rule 7: Most chloride (Cl-) salts are soluble, except those of silver, lead, and mercury.

Based on these solubility rules, we can conclude that AgNO3 will form a precipitate with either the sulfate (SO42-) or chloride (Cl-) ions, as both are insoluble salts with silver.

Since AgNO3 can form a precipitate with either SO42- or Cl-, we need to determine which of these ions will react first with the available Ag+ ions.

To do this, compare the concentrations of the SO42- and Cl- ions to the solubility product (Ksp) of their respective salts with Ag+. The solubility product (Ksp) for Ag2SO4 is 1.2 x 10^-5, and for AgCl, it is 1.8 x 10^-10.

Calculate the molar concentration of each ion based on the given milligram-per-liter concentrations.

Concentration of SO42- = (46.1 mg/L) / (96.06 g/mol)
Concentration of Cl- = (30.6 mg/L) / (35.45 g/mol)

Now compare the calculated concentrations with the solubility product (Ksp) values.

For Ag2SO4:
[Ag+]^2 * [SO42-] = (Ag+ concentration) * [(SO42-) concentration]

For AgCl:
[Ag+] * [Cl-] = (Ag+ concentration) * [(Cl-) concentration]

Compare the calculated values for both reactions and see which combination exceeds the product value:

(Ag+ concentration) * [(SO42-) concentration] > Ksp(Ag2SO4)
(Ag+ concentration) * [(Cl-) concentration] > Ksp(AgCl)

Based on this comparison, we can determine which precipitate will form. The combination that exceeds the respective Ksp value will form a precipitate.