Does it produce precipitate if 1.7 g of AgNO3 and 14.5 g of NaCl solvated in 200 mL water to get a solution in 25 oC ?
thank you
AgCl --> Ag^+ + Cl^-
Ksp = (Ag^+)(Cl^-) = about1.8E-10
Compare Qsp with Ksp.
In soution (and I'm assuming that adding the salts to 200 mL H2O is the same as producing 200 mL solution).
Ag^+ = 1.7/170 = about 0.01 mols.
You should go through these calculations yourself; I've rounded molar masses and the answers.
Cl^- = 14.5/58.5 = about 0.25 mols.
(Ag^+) = 0.01 mols/0.200L = about 0.05M
(Cl^-) = 0.25 mols/0.200L = about 1.25M
Qsp = (0.05)(1.25) = 0.06 which is larger than Ksp at 1.8E-10 and a ppt should occur.
To determine if a precipitate will form when 1.7 g of AgNO3 and 14.5 g of NaCl are dissolved in 200 mL of water at 25°C, we need to consider the solubility of the resulting compounds.
1. Begin by calculating the moles of AgNO3 and NaCl:
Moles of AgNO3 = mass of AgNO3 / molar mass of AgNO3
Moles of NaCl = mass of NaCl / molar mass of NaCl
The molar masses of AgNO3 and NaCl are:
AgNO3: Ag (107.87 g/mol) + N (14.01 g/mol) + 3O (16.00 g/mol) = 169.87 g/mol
NaCl: Na (22.99 g/mol) + Cl (35.45 g/mol) = 58.44 g/mol
Using these values:
Moles of AgNO3 = 1.7 g / 169.87 g/mol
Moles of NaCl = 14.5 g / 58.44 g/mol
2. Next, calculate the concentration of the solutions:
Concentration (Molarity) = Moles / Volume (in liters)
The volume of the solution is given as 200 mL, which is equal to 0.2 L.
Concentration of AgNO3 = Moles of AgNO3 / Volume of solution
Concentration of NaCl = Moles of NaCl / Volume of solution
3. Determine the solubility of AgNO3 and NaCl at 25°C:
Consult a solubility chart to determine the solubility of AgNO3 and NaCl at the given temperature. If the concentrations calculated in step 2 are below the solubility values, a precipitate will not form. If the concentrations are above the solubility values, a precipitate may form.
4. Compare the calculated concentrations to the solubility values:
If the calculated concentrations of AgNO3 and NaCl are below their respective solubilities, then no precipitate will form. However, if the concentrations exceed the solubilities, a precipitate may form.
It's important to note that the solubility of NaCl is much higher than that of AgNO3. Therefore, if there is any excess AgNO3 after both compounds have dissolved, it will most likely precipitate out.
By following these steps, you should be able to determine whether a precipitate will form when 1.7 g of AgNO3 and 14.5 g of NaCl are dissolved in 200 mL of water at 25°C.