**Problem Statement:**Determine the approximate concentration of free \( \text{Al}^{3+} \) ion at equilibrium under the given conditions. - **Initial Conditions:** - \( 1.06 \times 10^{-2} \) mol of aluminum nitrate is added to \( 1.00 \) L of solution. - The solution has a concentration of \( 1.390 \) M in hydroxide ions (\( \text{OH}^- \)).- **Equilibrium Expression:** - \([\text{Al(OH)}_4]^-\) - Formation constant (\( K_f \)) is given as \( 1.1 \times 10^{33} \).**Required:**Calculate the concentration of \( \text{Al}^{3+} \) ions:\[ [\text{Al}^{3+}] = \text{_____ M} \]

Answered: Image /qna-images/answer/396bf52a-8948-4be6-915f-0829cc372c02.jpg

What is the approximate concentration of free Al³+ ion at equilibrium when 1.06x10-2 mol aluminum nitrate is added to 1.00 L of solution that is 1.390 M in OH-. For [Al(OH)4], Kf = 1.1×10³3. [A1³+] = M

What is the approximate concentration of free Al³+ ion at equilibrium when 1.06x10-2 mol aluminum nitrate is added to 1.00 L of solution that is 1.390 M in OH-. For [Al(OH)4], Kf = 1.1×10³3. [A1³+] = M

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: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: We know that, pH can be expressed as negative logarithm of H+. i.e., pH = -…

Q: At a particular temperature, 3.31 g of Gd,(SO), will dissolve in 200 mL of water. What is the K of…

A: Given -> Mass of Gd2(SO4)3=3.31g Volume of water=200mL= 0.200 L (1L = 1000ml) Ksp of…

Q: A 125.0-mL sample of a solution that is 2.7×10−3M in AgNO3 is mixed with a 230.0-mL sample of a…

A: The balanced equilibrium reaction for the formation of Ag(CN)2-(aq) is: Ag+(aq) + 2CN-(aq) →…

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

Q: The following reaction is at equilibrium in a closed 4L vessel: N,(g) + 3H,(g)= 2NH,(g) What will…

A: Equilibrium is a state at which the rate of formation of the product becomes equal to the rate of…

Q: 4. A solution at 25°C is prepared in which a very small amount of Fe2+ is added to a much larger…

Q: Express the equilibrium constant for the following reaction. O O N2(g) + 3H2(g) ⇒ 2NH3(g) K = K = K…

Q: Solid barium carbonate and solid nickel(II) carbonate are in equilibrium with a solution containing…

A: The solubility product constant is an equilibrium constant, which represents the dissolution of a…

Q: The equilibrium concentration of copper(II) ion in a saturated copper(II) sulfide solution is M.

Q: What is the equilibrium molar concentration of Cu+ in a solution prepared by adding 0.1558 mol of…

A: The reaction is as follows Cu+(aq) + 2CN-(aq) [Cu(CN)2]-(aq)

Q: Write the solubility product reaction and the equilibrium constant expression, Ksp, for CaF2(s)

A: Some compound does not get much dissociated in water, their equilibrium constant will become Ksp

Q: . You determined the equilbrium constant, K eq^ prime for the reaction using a number of different…

A: K'eq. means equilibrium for the reverse reaction. It is equal to reverse of equilibrium constant.…

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

Q: (a) In the determination of chloride by the Mohr method, what will be the equilibrium concentration…

A: The objective of the question is to determine the equilibrium concentration of silver ions in the…

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: moles

Q: One millimole of Ni(NO3)2 dissolves in 240.0 mL of a solution that is 0.500 M in ammonia. The…

A: we need to calculate initial concentration of Ni(NO3)2 equilibrium concentration of Ni2+(aq )

Q: 460 mL of a 0.150 mol/L Pb(NO3)2 solution is mixed with 640 mL of a 0.420 mol/L NaI solution. The…

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 equilibrium concentration of phosphate ion in a saturated chromium(III) phosphate solution is

A: Using the solubility product to calculate the concentration required.

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: 500 mL of 0.12 M Pb(NO3)2 were mixed with 200 mL of 0.14 M KBr. Ksp for PbBr2 = 6.6x10-8. How many…

A: The objective of the question is to determine the mass of .It is given that,The volume of is .The…

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: 15) Determine the equilibrium concentrations of both Cu(NH3)4 2+ and Cu²+ in a solution made…

A: To determine the equilibrium concentrations of Cu(NH3)2+ and Cu²+ in the solution, we'll use the…

Q: If the solubility of silver carbonate (Ag2CO3) is 1.3 x 10-4 mol/L, calculate the Kps.

Q: Which of the following is more likely to precipitate the hydorxide ion? (a) Cu(OH)2(s) = Cu2+(aq) +…

A: Actually, the molar solubility is the amount of solutes that can be dissolved in per liter of…

Q: An aqueous solution is made by dissolving 1.1 x 10-³ moles of Zn(NO3)2 and 0.150 moles of NH3 in…

A: Given: Number of moles of Zn(NO3)2 is 1.1 x 10-3. Number of moles of NH3 is 0.150 moles. Volume of…

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: In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoC14². Co²+…

A: We would use the given observation at low and high temperature to answer these questions.

Q: Calculate the concentration of free, uncomplexed Cu2+ ions in a solution that originally contains a…

Q: What is the approximate concentration of free Al³+ ion at equilibrium when 1.86x10-² mol aluminum…

Q: Solid magnesium fluoride and solid magnesium carbonate are in equilibrium with a solution containing…

A: Stoichiometry is the method which is applied to determine the mass of substance existing in the…

Concept explainers

Coordination Chemistry

It is a part of chemistry, in which the study of compounds that have central atoms surrounded by molecules or ions, known as ligand, is known as coordination chemistry.

Question

**Problem Statement:**

Determine the approximate concentration of free \( \text{Al}^{3+} \) ion at equilibrium under the given conditions.

- **Initial Conditions:**
- \( 1.06 \times 10^{-2} \) mol of aluminum nitrate is added to \( 1.00 \) L of solution.
- The solution has a concentration of \( 1.390 \) M in hydroxide ions (\( \text{OH}^- \)).

- **Equilibrium Expression:**
- \([\text{Al(OH)}_4]^-\)
- Formation constant (\( K_f \)) is given as \( 1.1 \times 10^{33} \).

**Required:**

Calculate the concentration of \( \text{Al}^{3+} \) ions:
\[ [\text{Al}^{3+}] = \text{_____ M} \]

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 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

Solve this question
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 =
questions are in the image
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)
An equilibrium reaction between chromate ions, CrO4 2- (yellow), and H+ ions is established to produce dichromate, Cr₂072- (orange). Note the colours. A student adds NaOH to a test tube containing an orange mixture of the above reagents. What is observed? 01. The solution turns from orange to yellow O 2.A precipitate forms 3. The solution tuimns from orange to colourless O4. The solution remains orange
Determine the equilibrium concentration of chloride ions when solid AgCl is dissolved in 0.10 M NH3. Ksp for AgCl is 1.8 × 10-10 and the Kf for Ag(NH3)2+ is 1.7 × 107. 1.3 x 10-5 M O 5.0 × 10-8 M 5.5 x 10-2 M 5.5 x 10-3 M
Silver carbonate has a K = 5.65×10-¹2 and a solubility of 0.0001122 M in water. Solid silver sp carbonate is placed into a silver nitrate solution. What concentration of silver nitrate is necessary to reduce the solubility of the silver carbonate to 1×109 M? [AgNO,]= M
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
The equilibrium concentration of cobalt(II) ion in a saturated cobalt(II) sulfide solution is M.
What is the approximate concentration of free Fe2+ ion at equilibrium when 1.90×10-2 mol iron(II) nitrate is added to 1.00 L of solution that is 1.480 M in CN. For [Fe(CN)6l+, Kf= 1.0×1035. [Fe²*] = [ M