Question

In: Chemistry

A 0.10 mol sample of AgNO3 is dissolved in a 1.00 L of 1.00 M NH3...

A 0.10 mol sample of AgNO3 is dissolved in a 1.00 L of 1.00 M NH3 (aq) solution. If 0.010 mol NaCl is added to this solution, will AgCl(s) precipitate? Show the procedure by which you arrive at your answer. Given that Kf of [Ag(NH3)2] + = 1.6 x 10^7 and Ksp of AgCl = 1.8 x 10^10 .

Solutions

Expert Solution

any query please comment.

If satisfied please rate it thanks.


Related Solutions

What is the pH of a 1.00 L buffer solution that is 0.80 mol L-1 NH3...
What is the pH of a 1.00 L buffer solution that is 0.80 mol L-1 NH3 and 1.00 mol L-1 NH4Cl after the addition of 0.070 mol of NaOH(s)? Kb(NH3) = 1.76 ? 10?5
Q4, A 100.0mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3 Determine the...
Q4, A 100.0mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3 Determine the pH of the solution after addition of 100ml of HNO3 The kb of NH3 is 1.8x10-5
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the...
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 50.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the...
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 50.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.
1. A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Kb,...
1. A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Kb, NH3 = 1.8 × 10−5. Determine the pH of the solution at each of the following points in the titration: (a) before addition of any HNO3 (b) after the addition of 50.0 mL HNO3 (c) after the addition of 75.0 mL HNO3 (d) at the equivalence point (e) after the addition of 150.0 mL HNO3 2. (12 points) Consider the titration of 37.0 mL...
A) 1 L of solution contains 0.10 mol Ag+ and 0.10 mol of Ba2+. If a...
A) 1 L of solution contains 0.10 mol Ag+ and 0.10 mol of Ba2+. If a highly concentrated solution of K2CrO4 is added drop by drop, which will precipitate first, Ag2CrO4 or BaCrO4? Ksp for AgCrO4 = 2.0 x 10^-12; Ksp for BaCrO4= 1.2 x 10^-10 B) If the solution in part "A" contains 0.0010 Ag+ and 0.0010 mol of Ba2+ instead, which will precipiate first, Ag2CrO4 or BaCrO4? Answers: A) Ag2CrO4 and B) BaCrO4
A buffer is 0.10 M in NH3 and 0.10 M in NH4Cl. What is the pH...
A buffer is 0.10 M in NH3 and 0.10 M in NH4Cl. What is the pH of the solution after the addition of 10.0 mL of 0.20 M of HCl to 100.0 mL of the buffer?
Consider the compression at 15.6 C of 0.35 mol H2O(l) from 0.10 atm to 1.00 atm....
Consider the compression at 15.6 C of 0.35 mol H2O(l) from 0.10 atm to 1.00 atm. Calculate the values of ΔG when the process is carried out: (a) isothermally and reversibly and (b) isothermally and irreversibly under a constant external pressure of 1.00 atm. Take the density of water at this temperature to be equal to 999.1 kg/m3.
Calculate the solubility (a) in mol/L and (b) in g/L of AgCl in 2.0 M NH3(aq)....
Calculate the solubility (a) in mol/L and (b) in g/L of AgCl in 2.0 M NH3(aq). What is the concentration of Ag+ in this solution? (Ksp = 1.6 x 10-10; Kf = 1.7 x 107 for Ag(NH3)2+
1.00 mol of A and 1.00 mol of B are placed in a 4.00-L container. After...
1.00 mol of A and 1.00 mol of B are placed in a 4.00-L container. After equilibrium is established, 0.400 mol of D is present in the container. Calculate the equilibrium constant for the reaction: A(g) + 3 B(g) <---> C(g) + 2 D(g)
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT