In order to form [Ni(CN),?], 5.20 mol of KCN are added to 600. ml of 0.100 M Ni(NO)2. Assuming the total volume stays at 600. mL, calculate the equilibrium concentration of Ni2* in that solution. [Kf of Ni(CN),21-1.0 x 10313 O 9.3 x 1091 O 14 x 10 34 O 44 x 1045 O 21x 10 36 O 67 x 1024

In order to form [Ni(CN),?], 5.20 mol of KCN are added to 600. ml of 0.100 M Ni(NO)2. Assuming the total volume stays at 600. mL, calculate the equilibrium concentration of Ni2* in that solution. [Kf of Ni(CN),21-1.0 x 10313 O 9.3 x 1091 O 14 x 10 34 O 44 x 1045 O 21x 10 36 O 67 x 1024

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: The fictitious complex M(SCN)2 can be produced from an aqueous equilibrium in which the M2+ ion is…

Q: Consider the insoluble compound nickel(II) carbonate , NiCO3 . The nickel ion also forms a complex…

A: answer of the question is given below

Q: A 1.0 L solution contains 3.00×10-4 M Cu(NO3)2 and 1.35×10-3 M ethylenediamine (en). The Kf for…

Q: Consider the insoluble compound silver hydroxide , AgOH . The silver ion also forms a complex with…

A: Equilibrium constant tells about the direction of a reaction. Solubility product of an insoluble…

Q: Consider the following expression for the equilibrium constant that represents the dissociation of…

A: Given-> Weight of iodic acid = 176 gm Volume= 1.00 L Molar mass of iodic acid = 175.91 g/mole

Q: At the Oak Ridge National Laboratory in Tennessee, soils are heavily contaminated with mercury…

A: The complete balanced reaction = HgS (s) + H+ ↔ Hg+2 + HS-Given the temperature = 25∘CFor a general…

Q: Consider the equilibrium reaction below. [Cu(H₂O)6]²+ (aq) + 4 Cl (aq) light blue 1. A test tube in…

A: The question is based on the concept of Le-chatlier principle.It States that when a system at…

Q: The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, i.e., -log[Cu2+], in…

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

Q: The fictitious complex M(SCN)2 can be produced from an aqueous equilibrium in which the M2+ ion is…

A: Since the reaction taking place will be M2+ + 2 SCN- ----> M(SCN)2 hence from the above…

Q: For the following reaction, determine the value of Kc using the given equilibrium concentrations.…

A: Given that : The given equilibrium concentrations for the reaction is : [Co(H2O)62+] = 0.294 M [Cl-]…

Q: For the aqueOuS [Ni(NH3)6] 2+ complex Kf= 5.50 x 10^8 at 25 °C. Suppose equal volumes of 0.0016 M…

Q: Consider the insoluble compound iron(II) sulfide , FeS . The iron(II) ion also forms a complex with…

Q: Consider the insoluble compound silver bromide, AgBr. The silver ion also forms a complex with…

A: We need to write the equilibrium reactions for the dissolution of AgBr(s) in pure water and in…

Q: Calculate the equilibrium constant (Keq) for the following reaction. At equilibrium the [N2O4 ] =…

Q: Consider the insoluble compound cobalt(II) carbonate, COCO3. The cobalt(II) ion also forms a complex…

A: To write a balanced net ionic equation to show why the solubility of CoCO3 (s) increases in the…

Q: An aqueous solution is prepared in which 0.00113 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a…

Q: 15. Initially a solution consists of NO2 at a concentration of 1.5M. After some time, the reaction…

A: After some point in time, for a reversible reaction, the rate of the forward reaction is equal to…

Q: The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+,…

A: we have to calculate the value of pCu2+

Q: Consider the insoluble compound silver bromide, AgBr. The silver ion also forms a complex with…

A: Answer:When cyanide ion is added in a solution containing silver ion, they form a stable complex and…

Q: Calculate the molar solubility of aluminum hydroxide, Al(OH),, in a solution buffered at pH 12.00 Kp…

Q: solution containing copper(II) nitrate (aq) first has some aqueous ammonia added to it. A white…

A: The question is based on the concept of qualitative analysis. to identify the copper ions in the…

Q: Consider the insoluble compound nickel(II) hydroxide, Ni(OH)2. The nickel ion also forms a complex…

A: We need to write the net ionic equation and the value of equilibrium constant in this problem. We…

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

Q: Consider the insoluble compound silver chloride , AgCl . The silver ion also forms a complex with…

A: We need to write the equilibrium reactions for the dissolution of AgCl(s) in pure water and in…

Q: Consider the insoluble compound silver iodide , AgI . The silver ion also forms a complex with…

A: The answer of the following question is given below

Q: A 1.00 L solution contains 4.00×10-4 M Cu(NO3)2 and 3,000×10-3 Methylenediamine (en). The Kf for…

A: Volume of solution = 1 LConcentration of Cu(NO3)2 = 4.00 X 10-4 MConcentration of ethylene diamine…

Q: Using the dissociation constant, K, = 2.2 x 10 34, calculate the equilibrium concentration of NH, in…

A: Let x amount is dissociates

Q: Look at the cobalt equilibrium and decide which is pink (I or II) and which is blue? Co(H2O)62+ +…

A: The question is based on the concept of Le-chatlier principle.It States that when a system at…

Q: Consider the insoluble compound nickel(II) hydroxide, Ni(OH)2. The nickel ion also forms a complex…

Q: Consider the insoluble compound copper(II) hydroxide, Cu(OH)2. The copper (II) ion also forms a…

A: From the standard table Ksp value of Cu(OH)2 = 1.6 × 10-19

Q: When 15.11 ml of 0.102 M K2SO4 solution reacts with 35.00 ml of 0.114 M Pb(C2H3O2)2. predict the…

A: Data given: Volume of K2SO4 solution = 15.11 mL = 0.01511 L (1 L = 1000 mL) Concentration of K2SO4…

Q: E. Consider the slightly soluble salt PbI2. a) It is found that the solubility of PbI2 is 1.2 X 10-3…

Q: A 1.00 L solution contains 3.50×10-4 M Cu(NO3)2 and 2.500×10-3 M ethylenediamine (en). The Kf for…

A: Given data :

Q: Consider the insoluble compound cobalt(II) hydroxide , Co(OH)2 . The cobalt(II) ion also forms a…

A: Given compound is: cobalt(II) hydroxide , Co(OH)2 . The cobalt(II) ion also forms a complex with…

Q: A 1.00 L solution contains 2.25×10-4 M Cu(NO3)2 and 1.000×10-3 M ethylenediamine (en). The Kf for…

Q: Consider the insoluble compound cobalt(II) hydroxide , Co(OH)2 . The cobalt(II) ion also forms a…

A: Knet = 4.56 × 10-10

Q: Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with…

Q: Write a balanced net ionic equation to show why the solubility of Fe(OH)2(s) increases in the…

A: The objective of this question is to define the interaction between the strong acid and the…

Q: What is the approximate concentration of free Cu+ ion at equilibrium when 1.91x10-2 mol copper(I)…

A: Answer:- This question is answered by using the simple concept of calculation of equilibrium…

Q: To oxidize the iron in 1.00 gram of FeSO4·(NH4)2SO4·6 H2O requires 5.00 mL of HNO3. (Fe 2++ NO3― +…

A: The concentration of the solution provides information about the quantity of the substance present…

Q: Consider the insoluble compound Iron(II) hydroxide, Fe(OH)2. The iron(II) ion also forms a complex…

Q: Consider the insoluble compound nickel(II) carbonate, NICO3. The nickel ion also forms a complex…

A: The equation for the dissociation of NiCO3(s) is: NiCO3(s) ⇌ Ni2+(aq) + CO32-(aq) ; Ksp = 1.42*10-7…

Q: 11.) If the equilibrium constant for the reaction in part c.) in the previous problem is 5.0 x 104…

A: kc= [Ni(CO)4]/ [CO]4 5.0 x 104 =[Ni(CO)4]/ 5.0 x 104

Q: f 4.00 g of CuSO4 are dissolved in 8.5 × 102 mL of 0.25 M NH3 solution, what are the concentrations…

A: To find concentration of Cu2+, [Cu(NH3)4]2+, and NH3 in the solution when 4.00 g of CuSO4 is…

Question

In order to form [Ni(CN),2], 5.20 mol of KCN are added to 600. mL of 0.10OM Ni(NO3)2.
Assuming the total volume stays at 600. mL, calculate the equilibrium concentration of Ni2* in
that solution.
[Kf of Ni(CN),1 = 1.0 x 1031)
O 9.3 x 1031
O 14 x 10 34
0 44 x 1045
O 21x 10 36
O 67 x 1024

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

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

Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with cyanide ions. Write a net ionic equation to show why the solubility of AgCl(s) increases in the presence of cyanide and calculate the equilibrium constant for this reaction. Solubility product constant data is found in the Chemistry References. For Ag(CN)₂, Kf = 1.3×1021. Be sure to specify states such as (aq) or (s). K = + +
Consider the insoluble compound zinc cyanide, Zn(CN)2. The zinc ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Zn (CN)2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH3)4²+, K₁ = 2.9×10⁹. Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group 1 more group attempt remaining
Consider the insoluble compound nickel(II) carbonate, NiCO3 . The nickel ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of NICO3 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN)4²-, Kf = 1.0×10³1 . Be sure to specify states such as (aq) or (s). K= Submit Answer + + Retry Entire Group 9 more group attempts remaining
ess Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3)2+, Kf = 1.1×107. Be sure to specify states such as (aq) or (s). Knet + +
The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A]=0.100 M, [C]=0.0340 M, and [AC5]=0.100 M. Determine the formation constant, Kf, of AC5. The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.1580.158 M. What is the Ksp of AB?
Consider the insoluble compound silver hydroxide , AgOH . The silver ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction.For Ag(CN)2- , Kf = 5.6×1018 . Be sure to specify states such as (aq) or (s). Net Equation= _________ K = ________
Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)
Consider the insoluble compound cobalt(II) carbonate, CoCO3. The cobalt(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of CoCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Co(NH3)2+, K = 7.7x104. Be sure to specify states such as (aq) or (s). K= Submit Answer Retry Entire Group 3 more group attempts remaining
Consider the insoluble compound zinc carbonate, ZnCO3. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) in presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)42, K₁= 2.9x1015. Be sure to specify states such as (aq) or (s). K=
The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if 2.21 g of CuCl2 is dissolved in 1.000 L of a 0.926 M solution by NaCN. The addition of CuCl2 does not affect the volume (the final volume is always 1,000 L).
3. Calculate the [Ag"] in a solution prepared by dissolving 1.00 g of AgNO3 and 10.0g KCN in enough water to make 1.00 L of solution. Kf[Ag(CN)2] = 1.0 x 102 1-
Consider the insoluble compound nickel (II) hydroxide, Ni(OH)2. The nickel ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Ni(OH)2 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN)4²-, Kf = 1.0×10³¹ . Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group No more group attempts remain