50 ml of 0.1 M NaCl is mixed with 50 ml of 0.2 M AgNO3 predict whethera ppt of AgCl is formed or not
The NaCl is the limiting reageant, check that.
so you make .1*.05 moles of AgCl in 100 ml of solution
so convert that many moles of AgCl to grams, and check the solubility tables, you didn't specify temperature, but I suspect temperature is not a factor.
Solubility of AgCl in water is 520 μg/100 g at 50 °C
To predict whether a precipitate of AgCl will form when 50 ml of 0.1 M NaCl is mixed with 50 ml of 0.2 M AgNO3, we can use the concept of solubility rules.
1. Write down the balanced chemical equation for the reaction between NaCl and AgNO3:
AgNO3 + NaCl → AgCl + NaNO3
2. Check the solubility rules for AgCl:
According to the solubility rules, AgCl is insoluble in water.
3. Determine the net ionic equation:
Ag⁺ + Cl⁻ → AgCl
4. Compare the concentrations of the ions in the mixture:
- The concentration of Ag⁺ from AgNO3 is 0.2 M.
- The concentration of Cl⁻ from NaCl is 0.1 M.
5. Check if the product of the concentrations of Ag⁺ and Cl⁻ exceeds the solubility product constant (Ksp) for AgCl:
The Ksp for AgCl is 1.8 x 10⁻¹⁰.
[Ag⁺] × [Cl⁻] = (0.2 M) × (0.1 M) = 0.02 M²
Since 0.02 M² is less than 1.8 x 10⁻¹⁰, there will be no visible precipitate of AgCl formed. The ions will remain dissolved in the solution.
Therefore, when 50 ml of 0.1 M NaCl is mixed with 50 ml of 0.2 M AgNO3, no precipitate of AgCl will form.