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.

queen_honey_blossom answered 2 years ago
Next > < Previous

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?
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)
When 10.0 mL of 1.00 M AgNO3 solution is added to 10.0 mL of 1.00 M...
When 10.0 mL of 1.00 M AgNO3 solution is added to 10.0 mL of 1.00 M NaCl solution at 25.0 ° C in a calorimeter, a white precipitate of AgCl forms and the temperature of the aqueous mixture increases to 32.6 ° C. Assuming that the specific heat of the aqueous mixture is 4.18 J/(g °C), the density of the mixture is 1.00 g/mL, and the calorimeter itself absorbs a negligible amount of heat, what is ΔH in kJ/mol AgCl...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT