nemistLIWhat is the approximate concentration of free Ni²+ ion at equilibrium when 1.61×10-2 mol nickel nitrate is added to 1.00 L of solution that is 1.010 M inCN. For [Ni(CN)41², Kf= 2.0x1031.[Ni²*] =MSubmit Answer

As we have to find approximate concentration of Ni+2 ion, we will find it as below-

What is the approximate concentration of free Ni?+ ion at equilibrium when 1.61x10-2 mol nickel nitrate is added to 1.00 L of solution that is 1.010 M in CN. For [Ni(CN)4], Kf= 2.0x1031. (N*"] =| M Submit Answer

What is the approximate concentration of free Ni?+ ion at equilibrium when 1.61x10-2 mol nickel nitrate is added to 1.00 L of solution that is 1.010 M in CN. For [Ni(CN)4], Kf= 2.0x1031. (N*"] =| M Submit Answer

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 52E: The concentration of Mg2+ in seawater is 0.052 M. At what pH will 99% of the Mg2+ be precipitated as...

See similar textbooks

Related questions

Q: A student determines [FeSCN2+] is 0.00011 M at equilibrium. If the initial concentration of Fe3+ was…

Q: A 6.42% (w/v) Fe(NO3)3 (241.86g/mol) solution has a density of 1.059 g/ml. Calculate: a. the molar…

A: Given: Density=1.059 g/mLMolar mass=241.86 g/mol(w/v) of Fe(NO3)2=241.86 g/mol

Q: A solution prepared in the lab contains 3.5 x 10* M Sr2* and 0.0010 M F. Will a precipitate form?…

A: A precipitation occurs when Q > Ksp Q = [Sr2+] [F-]2

Q: The equilibrium constant, Ko, for the following reaction is 7.00×10-5 at 673 K. NH4I(s) =NH3(g) +…

Q: A saturated solution of iron(II) oxalate contains 0.0659 g FeC2O4 in 1.00 L of solution. What is the…

Q: A.) What is the approximate concentration of free Ag+ ion at equilibrium when 1.43×10-2 mol silver…

A: The amount of moles in the solution are constant irrespective of the change in the concentration of…

Q: The solubility-product constant for K,PdCl6 is 6.0 × 10-6 (K2PdCl6(s) = 2K* (aq) + PdCl,- (aq)).…

Q: The Kf for the dicyanosilver complex ion, [Ag(CN)2]-, is 5.6 x 1018. When solid NaCN is added to a…

A: Given [AgNO3] = 0.010 M [CN-] = 0.5 M Kf of [Ag(CN)2]- = 5.6*1018

Q: set up end up with an equilibrium concentration of [Fe(SCN)]2+ of 8.3x10-5 M. Based on these…

Q: The formation constant* of [M(CN) 2 ]^ - is 5.30 * 10 ^ 18 , where M is a generic metal. A 0.140…

A: The question is based on the concept of complex formation. metal iron reacts with cyanide to form…

Q: 03)3 and U. along with some distilled water, into three separate containers. Then, to each…

A: Chemical equilibrium is the state in where both the reactants and products are have no net change…

Q: Consider the following reaction:Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq)Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq)A solution…

A: First, the Kc expression for given reaction is determined as follows,

Q: Consider the reaction: Fe* (ag) + SCN (aq) = FESCN?* (ag) A solution is made containing an initial…

A: Given: Concentration of Fe3+= 1.0×10-3MConcentration of SCN-= 8.0×10-4MConcentration of FeSCN2+=…

Q: akeAssighmenytakeCovalenhtActivity.do?locator=assignment-take [References) A 55.0-mL sample of…

Q: Gallium sulphate is sparingly soluble salt in equilibrium with its ions in solution. a) Wrie the…

Q: Consider the reaction between Fe* and NCs ions. The equilibrium constant for this reaction is 620.4.…

A: Given that : Equilibrium constant Kc = 620.4 Volume of Fe+3 = 10 mL molarity of Fe+3 = 0.05 M Volume…

Q: Given the equation Ag*(aq) + 2 NH3 (aq) → [Ag(NH3),]*(aq) K = 2.00 × 107 determine the concentration…

A: Ksp of AgCl = 1.77 × 10-10 Kf = 2.00 × 107 Mass of AgCl = 767 mg = 0.767 g Volume = 100.0 mL =…

Q: Calculate the concentration of [Ag(S2O3)2]3- in a solution which contains 8.5E-6 M Ag+ ions and…

Q: The solubility product constant of Ag,CO3 o is 8.1×10-12 at 25°C. Calculate [Ag*] and [CO-2] in the…

A: Given: Ksp of Ag2CO3 = 8.1 X 10-12 Concentration of Ag+ coming from AgNO3 taken = Concentration of…

Q: The equilibrium constant, Kc, for the following reaction is 7.00×10-5 at 673 K. NH4I(s) NH3(g) +…

A: We are given The equilibrium constant, Kc, for the following reaction is 7.00×10-5 at 673 K. NH4I(s)…

Q: A solution is prepared such that the initial concentration of Cd2+ is 3.80×10-2 M and the initial…

A: The reaction is as:- Cd2+(aq) + 4Br-(aq) <-----> CdBr42-(aq) Kf = [CdBr42-][Cd2+][Br-]4

Q: You have a saturated aqueous solution of magnesium fluoride. The Kp of magnesium fluoride is 7.4 x…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: How do you do problem 1

A: Kc is the ratio of the equilibrium concentrations of product over equilibrium concentrations of…

Q: Initially, a mixture of 0.100 M NO, 0.050 M H2, 0.100 M H2O taken. At equilibrium the concentration…

A: Given information: A mixture of 0.100 M NO, 0.050 M H2, 0.100 M H2O taken. At equilibrium the…

Q: 3. Changing Reaction Equilibrium Conditions - Le Chatelier's Principle 3A. Effect of Changing…

A: Few questions based on Le-Chatlier principle, which are to be accomplished.

Q: Consider the following scenerio in answering Questions 2 through 4: An equilibrium mixture of the…

A: This is an example of dilution law which state that moles of solute before and after dilution remain…

Q: You have a test tube in which the following equilibrium is established. Fe* (aq) + SCN (ag) = FESCN*…

A: Since, the equilibrium is established so by adding common ion will disturb the equilibrium. We have…

Q: equilibirum, v

A: Yes pressure of Methane is given initially and kp also given hence we can calculate the equilibrium…

Q: aching and lea x + nent/takeCovalentActivity.do?locator=assignment-take [Review Topics] [References)…

Q: At 503 K the equilibrium constant Kc for the dissociation of N2O4, N2O4(g) ⇄ 2 NO2(g) has the…

A: Since,Concentration = No. of molesVolume

Q: A precipitate of Pbl, is formed when 5 mL of 0.012 M Pb(NO,), is added to 5 mL of 0.030 M KI. t was…

Q: A solution is prepared by mixing 50.0 mL of 0.20 M Pb(NO3)2 with 50.0 mL of 0.75 M KCl. (Ksp for…

Q: Solid calcium sulfate and solid calcium chromate are in equilibrium with a solution containing…

A: Sodium chromate is soluble in water and it ionizes completely in water. The solubility product of…

Q: What are the concentrations of Cu", NH3, and Cu(NH,)," at equilibrium when 18.8 g of Cu(NO,), is…

Q: S°

Q: What is the concentration of [Ag(S2O3)2]3- in a solution which contains 7.5 x 10-7 M Ag+ ions and…

A: Ag+ (aq.) + 2S2032-(aq.) → Ag(S2O3)23-(aq.) Given in the question, Kf for [Ag(S2O3)2]3- = 4.7 x…

Q: A student ran the following reaction in the laboratory at 637 K: 2HI(g) H2(g) + I2(g) When she…

Q: meeded for this qustion. Solid copper(II) hydroxide and solid zinc hydroxide are in equilibrium with…

A: The value of Ksp can be written as" Cu(OH)2, ksp = 1.6×10-19 Zn(OH)2, Ksp = 3.0×10-17 Now, find out…

Q: A student determines [FeSCN2+] is 0.00016 M at equilibrium. If the initial concentration of Fe3+ was…

A: Given, Initial concentration of Fe3+ = 0.00080M. Initial concentration of SCN- = 0.0012M.…

Q: A 6.42% (w/w) Fe(NO3)3 solution has a density of 1.059 g/mL. (MM of Fe(NO3)3 = 241.86 g/mol).…

Q: What is the approximate concentration of free Ag* ion at equilibrium when 1.85x102 mol silver…

A: Given: The number of moles of silver nitrate is 1.85 x 10-2 mol The volume of the solution is 1.0 L…

Q: At 25 °C, an aqueous solution has an equilibrium concentration of 0.00425 M for a generic cation,…

Q: At the start of the reaction, there was 0.976 mol of NOCI in a 1.50 L reaction chamber. At…

A: Balance chemical equation: 2 NOCl (g) ⇌ 2 NO…

Q: The formation constant* of [M(CN) 2 ]^ - is 5.30 * 10 ^ 18 , where M is a generic metal. A 0.140…

Q: You mix a 110.0-mL sample of a solution that is 0.0124 M in NiCl2 with a 185.0-mL sample of a…

A: The question is based on the concept of chemical equilibrium . we have to calculate Nickel ion…

Q: Given these initial concentrations: [SCN-] = 0.000644 M, [Fe3+] = 0.000505 M, and [Fe(SCN)2+] =…

A: Initial concentration of SCN- is 0.000644μ ∴SCN-=0.000644μ Initial concentration of…

Q: What is the approximate concentration of free Ag+ ion at equilibrium when 1.43×10-2 mol silver…

A: Given : Moles of AgNO3 = 1.43 X 10-2 mol Concentration of CN- ions = 1.080 M And volume of solution…

Q: The equilibrium constant of the reaction 2002 - 200+02 is 1.08. If the concentrations of CO and 02…

A: ⁷

Q: onsider the following reaction: p(g) + B2(g) → 2 AB(g) AH°rxn=-8.06 kJ mol1 he equilibrium constant,…

A: Equilibrium constant is directly proportional to the temperature

Question

nemistLI
What is the approximate concentration of free Ni²+ ion at equilibrium when 1.61×10-2 mol nickel nitrate is added to 1.00 L of solution that is 1.010 M in
CN. For [Ni(CN)41², Kf= 2.0x1031.
[Ni²*] =
M
Submit Answer

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

. Approximately 1.5103of iron(II) hydroxide. Fe(OH)2(s), dissolves per liter of water at 18 °C. Calculate Kspfor Fe(OH)2(s) at this temperature.
The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem: MgF2(s)Mg2+(aq)+2F(aq) In a saturated solution of MgF2 at 18 C, the concentration of Mg2+ is 1.21103M . The equilibrium is represented by the preceding equation. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. (c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00103 -M solution of Mg(NO3)2 is mixed with 200.0 mL of a .2.00103 -M solution of NaF at 18 C. Show the calculations to support your prediction.. (d) At 27 C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17103M . Is the dissolving of MgF2 in water all endothermic or an exothermic process? Give an explanation to support your conclusion.
. Lead(II) chloride, PbCl2(s), dissolves in water to the extent of approximately 3.6102Mat 20 °C. Calculate Kspfor PbCl2(s), and calculate its solubility in grams per liter.
Consider the equilibrium curve for AgCl shown below. Which of the following statements about a solution at point A on the curve are true? (a) The solution is saturated and at equilibrium. (b) Addition of NaCl increases the concentration of Cl- in solution. (c) Addition of NaCl increases the concentration of in solution. (d) Addition of Ag+ results in the precipitation of AgCl. (e) Addition of solid NaNO3 to the solution without change in volume does not change [Ag+] or [Cl-].
A solution is formed by mixing 50.0 mL of 10.0 M NaX with 50.0 mL of 2.0 103 M CuNO3. Assume that Cu+ forms complex ions with X as follows: Cu+(aq)+X(aq)CuX(aq)K1=1.0102CuX(aq)+X(aq)CuX2(aq)K2=1.0104CuX2(aq)+X(aq)CuX32(aq)K3=1.0103 with an overall reaction Cu+(aq)+3X(aq)CuX32(aq)K=1.0109 Calculate the following concentrations at equilibrium. a. Cux32 b. CuX2 c. Cu+
A solution contains 1.0 105 M Ag+ and 2.0 106 M CN. Will AgCN(s) precipitate? (Ksp for AgCN(s) is 2.2 1012.
Hydrogen iodide gas decomposes to hydrogen gas and iodine gas: 2HI(g)H2(g)+I2(g)To determine the equilibrium constant of the system, identical one-liter glass bulbs are filled with 3.20 g of HI and maintained at a certain temperature. Each bulb is periodically opened and analyzed for iodine formation by titration with sodium thiosulfate, Na2S2O3. I2(aq)+2S2O32(aq)S4O62(aq)+2 I(aq)It is determined that when equilibrium is reached, 37.0 mL of 0.200 M Na2S2O3 is required to titrate the iodine. What is K at the temperature of the experiment?
. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
A scientist was interested in how soluble rust is in acidic soils, so she set up an idealized problem to get an initial feel for the situation. A fairly acidic soil has a pH of 4.50. Also, rust is essentially Fe(OH)3. Therefore, she considered the following problem: Suppose a 1.00-g sample of iron(III) hydroxide is exposed to 1.00 L of a buffer with a pH of 4.50. She then calculated the nanograms of Fe3+ that dissolve in a liter of this buffer. Show how you would do this problem. Explain your work.
. Chromiurn(III) hydroxide dissolves in water only to the extent of 8.21105M at 25 °C. Calculate Kspfor Cr(OH)3at this temperature.
The concentration of Mg2+ in seawater is 0.052 M. At what pH will 99% of the Mg2+ be precipitated as the hydroxide salt? [Ksp for Mg(OH)2 = 8.9 1012.]
Calculate the equilibrium concentrations of NH3, Cu2+, Cu(NH3)2+, Cu(NH3)22+, Cu(NH3)32+, and Cu(NH3)42+ in a solution prepared by mixing 500.0 mL of 3.00 M NH3 with 500.0 mL of 2.00 103 M Cu(NO3)2. The stepwise equilibria are Cu2+(aq)+NH3(aq)CuNH32+(aq)K1=1.86104CuNH32+(aq)+NH3(aq)Cu(NH3)22+(aq)K2=3.88103Cu(NH3)22+(aq)+NH3(aq)Cu(NH3)32+(aq)K3=1.00103Cu(NH3)22+(aq)+NH3(aq)Cu(NH3)42+(aq)K4=1.55102