The overall formation constant for Fe(CN)6³ is 1.0x1042. K₁= [Fe(CN)6³-] [Fe³+][CN16 =1.0x104² 3- What will be the equilibrium concentrations of Fe³+, CN- and Fe(CN)6³ in 500.0 mL of a solution that was originally 0.15 M Fe³+ and 1.20 M CN-? a. [Fe3+] b. [CN-] c. [Fe(CN)6³-]

The overall formation constant for Fe(CN)6³ is 1.0x1042. K₁= [Fe(CN)6³-] [Fe³+][CN16 =1.0x104² 3- What will be the equilibrium concentrations of Fe³+, CN- and Fe(CN)6³ in 500.0 mL of a solution that was originally 0.15 M Fe³+ and 1.20 M CN-? a. [Fe3+] b. [CN-] c. [Fe(CN)6³-]

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: What is the approximate concentration of free Al3+ ion at equilibrium when 1.54x102 mol aluminum…

Q: studying the equalibrium of Fe3+ and SCN- with FeSCN2+ Fe3+ (aq) + SCN- (aq) =FeSCN2+ (aq) a.…

A: When the net concentration change of reaction's species gets vanished and no observable decline in…

Q: What is the approximate concentration of free Cd2+ ion at equilibrium when 1.18x102 mol cadmium(II)…

Q: How do I fill in the ICE tables?

A: Please see the attached photo for the solution.To calculate the equilibrium constant, Kc, first…

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: In a saturated solution of cadmium carbonate at 25 °C both [Cd²+] and [CO]= 1.0 x 10-6 M. Write an…

Q: A 0.100 L solution of 0.310 M AgNO, is combined with a 0.100 L solution of 1.00 M Na, PO4. Calculate…

A: The chemical reaction taking place is: 3AgNO3 + Na3PO4 → Ag3PO4 + 3NaNO3 The given information is:…

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: 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: When AgCl(s) is dissolved in a solution of NH3, the complex ion Ag(NH3)2+ forms as shown in the…

A: we need to calculate Kf for Ag(NH3)2+

Q: 14. Calculate the solubility product constant for copper(ll) iodate, Cu(1O3)2. The solubility of…

A: As per the given data Solubility of copper (II)Iodate=0.13g/100ml We need to convert to solubility…

Q: Which of the following equilibrium constants corresponds to a situation where AG = 0? OK>1 ОК»»»1…

Q: Sufficient sodium cyanide, N&CN, was added to 1.0 x 10- M silver nitrate, AGNO3, to give a solution…

A: Given that, concentration of AgNO3= 1.0×10-2 M = 0.01 M The NaCN and AgNO3 solution react to form a…

Q: What is the approximate concentration of free Zn2+ ion at equilibrium when 1.00×10-2 mol zinc…

A: To determine: Approximate concentration of free Zn2+ ions at equilibrium when 1.00×10-2 mol zinc…

Q: What is the approximate concentration of free Zn2+ ion at equilibrium when 1.00×10-2 mol zinc…

A: The equilibrium reaction for the [Zn(OH)4]2- is as follows:

Q: Silver and ammonia may react to form Ag(NH₃)₂⁺ complex (Kf = 1.66 x 107). A 500 mL of 0.10 mol Ag⁺…

A: Given, A 500 mL of 0.10 mol Ag⁺ and 500 mL of 0.70 mol NH₃ are mixed together, The concentration of…

Q: 2. How many moles of Ag Br can dissolve in 1.0 L of 0.40M NH;? Kr [Ag(NH3)2] *= 1.7 x 107 Ksp(AgBr)…

A: Given: Kf [Ag(NH3)2]+ = 1.7×107 Ksp(AgBr) = 5.0×10-13 We have to calculate the number of moles of…

Q: The formation constant* of [M(CN)2]¯ is 5.30 × 10'8, where M is a generic metal. A 0.150 mole…

A: Given, [M(CN)2]- M+ + 2CN- ---> [M(CN)2]- Formation constant, Kf = 5.30 x 1018 Kf = [M(CN)2]- /…

Q: Given that the value of Kc is 199.90, calculate the equilibrium concentrations of Fe+3 and SCN- if…

A: Well, First we need to reverse the reaction so that construction of ICE table will be easy. Kc for…

Q: What is the concentration of free Ag+(aq) in a solution that is initially 0.01254 M in AgNO3 and…

A: · Concentration of AgNO3 = 0.01254 M· Concentration of NH3 = 1.04842 M· Kf of AgNH32+ = 1.600×107

Q: What is the approximate concentration of free Al³+ ion at equilibrium when 1.13×10-² mol aluminum…

Q: Co(NH,), complex K,= 1.58 × 10 at 25 °C. For the aqueous %3D Suppose equal volumes of 0.0028M…

A: As Equal volume are taken Concentration of Co(NO3)3 = 0.0028 M2 = [Co3+]Concentration of Co(NO3)3…

Q: iClicker: To 120.0 ml 2.8 x 10-3 M AgNO3 solution 0.030 mol solid NaCN is added. What is the…

A: The reaction that occurs when NaCN is added to solution can be represented as follows:

Q: 6. In an experiment, pH meters were created using indicators and the pH value was found to be 11 for…

A: The dissociation constant of a base gives measure of the strength of the base. More the value of…

Q: Lead (II) fluoride has a Ksp value of 2.7x10-8. What is the concentration of Pb2+ and F- ions in a…

A: The solubility product constant (Ksp) describes the equilibrium between a solid and its constituent…

Q: Initial Concentration 9.091x10-4 1.818x10-4 0 Change in Concentration Equilibrium…

Q: 3. Complex ion formation. Calculate the equilibrium concentration of Ag+(aq) in a solution that is…

A: We have find out the answer

Q: [Fe(CN),] complex K, = 1.0 × 105 For the aqueous at 25 °C. Suppose equal volumes of 0.0090M Fe(NO,)…

Q: Sufficient sodium cyanide, NaCN, was added to 2.5x10^-2 M silver nitrate, AgNO3, to give a solution…

A: Given: Molarity of AgNO3 = 2.5×10-2 MMolarity of CN- ion = 0.193 MKf for Ag(CN)2- = 5.6×1018

Q: Describe how concentrations of Fe3

A: Given: Fe3+(aq)+SCN-(aq)↔FeSCN2+(aq)

Q: For the aqueous [Hgl, complex K,= 6.76 x 1029 at 25 °C. Suppose equal volumes of 0.0098 M Hg(NO,)…

A: After mixing equal volume of Hg(NO3)2 and KIConcentration of Hg(NO3)2 = 0.0098 M2 = 0.0049 M = [Hg2+…

Q: 2. Given that KspNi(OH)2] = 5.50 x 10-16, Ksp[Mg(OH)2] = 8.9 x 10-12, and Ksp[Ca(OH)2] = 4.7 x 10-4,…

A: correct option [c] Ni(OH)2⇌Ni+2 + 2OH- Ksp=[Ni+2]× [OH-]2 Given Ksp=5.50×10-16Let [Ni+2]…

Q: To 200.0 ml of a solution of Al(NO3)3 with concentration (1.000x10^-3) mol L-1, (3.0x10^2) ml of…

A: Step 1:Given information:Initial volume of Al(NO₃)₃ solution = 200 mL = 0.2 LConcentration of…

Q: The generic metal A forms an insoluble salt AB(s) and a complex AC, (aq). The equilibrium…

Q: What is the approximate concentration of free Ag+ ion at equilibrium when 1.36x10-² mol silver…

A: Given data, Silver nitrate added at equilibrium 1.36×10-2 mol to 1 L of solution that is 1.2 M in…

Q: A solution contains 3.8 x 102 M in A³ and 0.29 M in NaF. If the K, for AIF 3 is 7 x 10¹9, how much…

A: The question is based on the concept of chemical equilibrium.We need to calculate equilibrium…

Q: The overall formation constant for Fe(CN)6³- is 1.0x104². K₁= [Fe(CN)6³-] [Fe³+][CN 16 -=1.0×104² 3-…

A: Given : Kf = 1.0 x 1042 [Fe+3] = 0.15 M [CN-] = 1.20 M

Q: What is the initial concentration of Ni(NO3)2 in the solution? M What is the equilibrium…

Q: Silver and ammonia may react to form Ag(NH₃)₂⁺ complex (Kf = 1.66 x 107). A 500 mL of 0.10 mol Ag⁺…

A: The complexation reaction will be Ag+ (aq) + 2NH3 (aq) ------------------ [Ag(NH3 )2]+ (aq) The…

Q: For Agl, Ksp = 8.5 x 10-17. For [Ag(CN)2]¯ Kf = 1.0 x 1021. What is the value of K. of the following…

Q: One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.400 M in ammonia. The…

A: Given, initial mole of Ni(NO3)2 = 1 milli mole Volume of solution = 230.0 mL Concentration of NH3 =…

Q: We have a blue colored solution of CuSO4 in a concentration of 0.1 M. What is the necessary…

A: Since initial moles of Cu2+ taken = moles of CuSO4 = concentration of CuSO4 X volume of solution =…

Q: 22. example also given, thank you!

Question

The overall formation constant for Fe(CN)6³ is 1.0x1042.
K₁=
[Fe(CN)6³-]
[Fe³+][CN16
=1.0x104²
3-
What will be the equilibrium concentrations of Fe³+, CN- and Fe(CN)6³ in 500.0 mL of a solution that
was originally 0.15 M Fe³+ and 1.20 M CN-?
a. [Fe3+]
b. [CN-]
c. [Fe(CN)6³-]

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

Equilibrium Concepts in Analytical Chemistry

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

Calculate the concentration of free, uncomplexed Cu2+ ions in a solution that originally contains a total of 1.0 × 10-3 M copper (II) ions and an equilibrium concentration of 0.10 M NH3. (Kf=4.8 x 1012)
The equilibrium constant for: Als) / Al*3 (bb), aq) // Mg*2 (aa) / Mg(s) is (ab), 3A. 1.02 x 10-72 B. 5.02 x 10-15 C. 0.46 D. 9.25
What is the approximate concentration of free Al³+ ion at equilibrium when 1.86×10-2 mol aluminum nitrate is added to 1.00 L of solution that is 1.440 M in F. For [AIF6]³, Kf = 6.9x10¹⁹. [A1³+] = M
vs Question 13 Silver ions form a complex ion in the presence of cyanide ions, according to the following equation: Shift to the right Agt (aq) + 2 CN- (aq) 1.0m Ke 6.04 If 0.040 mol of AgNO, is added to one liter of 1.0 M KCN, what are the equilibrium concentrations of each species in the reaction? [Ag*] = [CN] = [[Ag(CN)₂]] = M M O [Ag(CN)₂] M 1.1 x 1018
An acidic solution containing 0.015 M La³ + is treated with NaOH until La(OH), precipitates. At which pH does this occur? Kp for La(OH), is 2 x 10-21. pH =
11. The Kf for [AIF6]³- is 7.0 x 101⁹ and the corresponding equilibrium is shown below. Calculate the concentration of Al³+ ions in a solution that is initially 0.83 M in [AlF6]³-. Al³+ (aq) + 6 F-(aq) [AIF6]³(aq)
Choose the best answer below. Consider the following complex ion formation equilibrium and it's equilibrium constant, Kf. Which of the following statements is FALSE? Cu2+ (aq) + 4CN" (aq) Û Cu(CN)42- (aq) Kf = 1.0x1025 O Adding more CN- will cause more complex ion to form The equilibrium lies in favor of the complex ion Cu2+ is a Lewis acid in the reaction, and CN is a Lewis base Removing some of the Cu2* (e.g., by precipitation) will cause some of the complex ion to dissociate The complex ion is a Lewis acid-base adduct O If enough CN- is added, the equilibrium mixture would contain zero Cu2+
question 4 only
The molecular complex between silver ion and cyanide ion forms by the reactionAg+(aq) + 2 CN-(aq) ⇌ Ag(CN)2-(aq) Kf = 1.0 x 10^21A solution initially has [Ag+] = 2.0 x 104 M, and [CN-] = 0.0400 M. What will be the concentration ofAg+ ion at equilibrium?
8. You mix a 200.0-mL sample of a solution that is 1.5 X 10-³ M in Cu(NO3)2 with a 250.0-mL sample of a solution that is 0.20 M in NH3. After the solution reaches equilibrium, what concentration of Cu²+ (aq) remains? For [Cu(NH3)4]²+, Kf = 1.7 x 1013 me that
Two students conducted an experiment, where they mixed 6 ml of 0.002M Fe(NO with 3 ml of 0.050 M HNO, A1 ml of 0.002 M NasCN was then added. Assuming that the equilibrium of FeSCN" concentrate is 7.96x 10 M. Determine Keg for the formation of FeSCN O 741 10-4 O 169 10-3 O 3.32 102 O 5.90 10 2 O 117 105
A.) What is the approximate concentration of free Ag+ ion at equilibrium when 1.43×10-2 mol silver nitrate is added to 1.00 L of solution that is 1.080 M in CN-. For [Ag(CN)2]-, Kf = 1.3×1021.