Equal volumes of a 0.020 M Zn^2+ solution and a 2.0 M NH3 solution are mixed....

Equal volumes of a 0.020 M Zn^2+ solution and a 2.0 M NH3 solution are mixed. Kf for [Zn(NH3)4]^2+ is 4.1 × 10^8. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC2O4 precipitate? What is Q? Ksp ZnC2O4 = 2.7 × 10^-8

Answer: no, Q = 2.9 × 10^-12

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Equal volumes of 0.180 M AgNO3 and 0.160 M ZnCl2 solution are mixed. Calculate the equilibrium...

Equal volumes of 0.180 M AgNO3 and 0.160 M ZnCl2 solution are mixed. Calculate the equilibrium concentrations of Ag+ and Zn2+.

Denis titrates 25 mL of a 0.060 M solution of ammonia (NH3) with a 0.020 M...

Denis titrates 25 mL of a 0.060 M solution of ammonia (NH3) with a 0.020 M solution of hydrochloric acid. A) Write the chemical equation that occurs B) Do you expect the pH of the solution to be acidic, basic or neutral at the equivalence point? Explain. C) Calculate the pH after 20 mL of HCl solution have been added. Hint: Kb(NH3)=1.8*10-5

A solution is made that is 1.1×10−3 M in Zn(NO3)2 and 0.140 M in NH3. Part...

A solution is made that is 1.1×10−3 M in Zn(NO3)2 and 0.140 M in NH3. Part A After the solution reaches equilibrium, what concentration of Zn2+(aq) remains? Express your answer using two significant figures.

A solution is made of 1.1 x 10-3M in Zn(NO3)2 and 0.150 M in NH3. After...

A solution is made of 1.1 x 10-3M in Zn(NO3)2 and 0.150 M in NH3. After the solution reaches equilibrium, what concentration of Zn2+(aq) remains? Kf (Zn(NH3)42+) = 2.8 x 109

A 200 mL solution of 0.100 M solution of Ammonia, NH3 , is slowly mixed with...

A 200 mL solution of 0.100 M solution of Ammonia, NH3 , is slowly mixed with 0.100 M HCl. Determine the pH after addition of: 0 mL of HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, 250 mL of HCl 4. Describe in exact detail (including gram quantities and identity of species) how you would create a 500 mL solution of buffer with a pH 8.0 ?

A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100...

A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100 M HCl. Determine the pH after addition of: 0 ml of HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, and 250 mL of HCl.

A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100...

A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100 M HCl. Determine the pH after addition of: 0 ml of HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, and 250 mL of HCl.

PART A) A solution is prepared by mixing equal volumes of 0.17 M HCl and 0.42...

PART A) A solution is prepared by mixing equal volumes of 0.17 M HCl and 0.42 M HNO3. (Assume that volumes are additive.) Express the pH to two decimal places. PART B) Using the chart Estimate [H3O+] in a 1.5 M solution of each acid. Express the molar concentrations to two significant figures separated by commas. I'm stuck on the one that says very large. For all the other ones I multiplied the Ka by the 1.5M. The answer for...

Question 6 Calculate the pH of a solution prepared by mixing equal volumes of 0.050 M...

Question 6 Calculate the pH of a solution prepared by mixing equal volumes of 0.050 M sodium oxalate, Na2C2O4 (aq), and 0.010 M ammonium chloride, NH4Cl (aq). For ammonium, Ka = 5.70 × 10–10; for oxalic acid, Ka,1 = 5.60 × 10–2and Ka,2 = 5.42 × 10–5. Hint #1: Use the charge balance equation as your main equation. Use the mass balance and equilibrium equations to find an expression for each species in terms of [H3O+] or [OH–], then substitute...

The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO3)2 are mixed...

The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C2O4. The oxalate ion, C2O4, acts as a ligand to form a complex ion with the Mn2+ ion with a coordination number of two. Mn2+ + C2O42

Subjects