From the value \( K_f = 1.2 \times 10^9 \) for Ni(NH\(_3\))\(_6\) \(^{2+}\), calculate the concentration of NH\(_3\) required to just dissolve 0.014 mol of NiC\(_2\)O\(_4\) (\( K_{sp} = 4 \times 10^{-10} \)) in 1.00 L of solution. (*Hint: You can neglect the hydrolysis of C\(_2\)O\(_4^{2-}\) because the solution will be quite basic.*)

Answered: Image /qna-images/answer/07a3ea61-3908-4f21-b36d-16ce7c09953e.jpg

From the value Kf = 1.2 × 10º for Ni(NH3)62+ , calculate the concentration of NH3 required to just dissolve 0.014 mol of NiC2O4 (Ksp = 4 × 10-10 ) in 1.00 L 2- because the solution will of solution. (Hint: You can neglect the hydrolysis of C2 04 be quite basic.)

From the value Kf = 1.2 × 10º for Ni(NH3)62+ , calculate the concentration of NH3 required to just dissolve 0.014 mol of NiC2O4 (Ksp = 4 × 10-10 ) in 1.00 L 2- because the solution will of solution. (Hint: You can neglect the hydrolysis of C2 04 be quite basic.)

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: A buffer solution is made that is 0.310 M in H₂CO3 and 0.310 M in KHCO3. If Kal for H₂CO3 is 4.20 ×…

A: GIven: The concentration of H2CO3 in the buffer = 0.310 M The concentration of KHCO3 in the buffer =…

Q: What is the approximate concentration of free Cu²+ ion at equilibrium when 1.05x10-2 mol copper(II)…

Q: What is the equilibrium constant for the solubility of Ag2CO3 (Ksp = 8.1 × 10−¹²) in NH³? (Kf of…

Q: mine the pH during the titration of 39.3 mL of 0.315 M trimethylamine ((CH3)3N, K = 6.3×10) by 0.315…

Q: Sulfate buffer? Your laboratory is out of materials to make phosphate buffer and you are…

A: A buffer solution is formed by the weak acid and its conjugate base or weak base and its conjugate…

Q: [Zn2+] = M

Q: When 1.95 g of Co(NO3)2 is dissolved in 0.250 L of 0.220 M KOH, what are [Co2+], [Co(OH)42−], and…

A: When 1.95 g of Co(NO3)2 is dissolved in 0.250 L of 0.220 M KOH, [Co2+], [Co(OH)42−], and [OH−] are…

Q: If a solution of 0.15 MMn² and 0.15 M Cd is gradually made basic, what will the concentration of Cd…

A: Answer: Precipitation of a sparingly soluble salt begins when its solubility products becomes equal…

Q: Can you explain it step by step? What if the problem is about kb instead?

A: Step 1:Balanced reaction isC6H5COOH (aq) + KOH(aq) → C6H5COOK(aq) + H2O(l)net ionic equation…

Q: 8. The following questions concern the reaction HA(aq) + B(aq) 2 HB1+(aq) + A1-(aq). What can you…

Q: 1 2 3 4 5 6 7 8 = 9 =10 In aqueous solution the Feion forms a complex with six cyanide anions. Write…

A: To describe the equilibrium between the hydrated Fe2+ ion and the complex with six cyanide anions in…

Q: Activity 5 More on Solubility, and LeChatelier's Principle (5a) What is the molar solubility of CaF2…

A: Answer: According to Le-chatalier's principle, when we change parameter of the system which is in…

Q: What ratio of CH.NH2 to CH.NH3 is needed to prepare a pH 10.00 buffer? (Kb for CH:NH2 is 4.4 x 10-4)

Q: What is the pH of a saturated solution of Ca(OH)₂? Ca(OH)₂ (s) Ca²+ (aq) + 2 OH- (aq) Ksp = 3.7 x 10…

A: Solubility reaction:- Ca(OH)2(s) -------------> Ca2+(aq) + 2OH-(aq) Ksp = 3.7×10-6

Q: In 6.0 M NaOH, M(OH)3 has a solubility of 1.0 M due to the formation of the [M(0H)4]¯ ion. Calculate…

A: Interpretation - To calculate the Ksp of M(OH)3 when In a 6M NaOH , M(OH)3 has a solubility of 1M…

Q: What is the equilibrium concentration of H3O+ in 0.1564 M HNO2 ? See reaction below HNO2 + H2O ↔…

Q: Can you help calculate the concentrations for 5 and explain to me what effect did NH4+ have on the…

A: pH of a solution is calculated as:Buffer: A buffer is a solution that can resist changes in pH when…

Q: 3. Calculate the molar solubility of Cr (OH)3 in a solution buffered at (a) a pH of 5.00 and (b) a…

Q: None

A: 1. **Initial Reaction with 6M NH\(_3\)**: - **PbCl\(_2\)** and **AgCl** are both insoluble in…

Q: 2-)

Q: What reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M…

A: The solubility of an ionic compound depends on its corresponding solubility product.The higher the…

Q: When 20 mmol Pb(NO3)2 is added to 250 mL of 1.0 M NaX, the [PbX4]²- ion forms. At equilibrium,…

A: To calculate Kf for [PbX4]2- , we would first calculate moles of both reactants used . The. We would…

Q: What concentration of SO3 is in equilibrium with Ag₂ SO, (s) and 7.10 x 10-3 M Ag+? The Ksp of Ag₂…

A: Molarity of Ag+ = 7.10 × 10-3 M-> Ksp not given in question so used here from textbook.Ksp of…

Q: What is the pH of a 1.0 L solution that is 0.50 M PO43- and 0.50 M HPO42-? (The pKa values for…

A: As per the Henderson–Hasselbalch equation:pH = pKa + log [PO4-3]/[HPO4-2]pKa = 12.4 as ( third…

Q: 3. The Ka and K, for bicarbonate. NaHCos + 4. The Kp for sulfate. 5. The K, for CH3NH3*.

Q: Calculate the mas of KC2H3O2 that must be added to 500.0mL of a 0.200 M HC2H3O2 (Ka = 1.8 x 10-5)…

A: Given→ Volume of HC2H3O2 = 500.0 mL Molarity of HC2H3O2 = 0.200 M Ka…

Q: What is the organic product formed in the following reaction? 1 HO да OH HO OH || _OH H* IV OH ч

A: This is an example of acetal formation from hemiacetal

Q: Calculate the concentrations of H₂C₂O4, HC₂04, C₂042, and H* ions in a 0.261 M oxalic acid solution…

Q: Given that carbonic acid, H₂CO3, has a pka1 = 6.37 and a pka2 = 10.33, answer the following. (a) If…

A: Answer: Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: BaSO4(s) = Ba²+ (aq) + SO2 (aq) Ksp = 1.5 x 10-9 @ 25 °C [Ba2+] = 3.9 x 10-5 M What is the…

A: Let the solubility of the ions (formed by dissociation of BaSO4) be "S". The relation between ksp…

Q: At a certain temperature, nickel(II) hydroxide, Ni(OH)2, has a value of Ksp = 8.9 x 10-16. At this…

Q: Calculate the solubility of BaCO3 in a solution that has a fixed H3O+ concentration of 1.00x10-9 .

A: We need to calculate the solubility of BaCO3 in a solution that has a fixed H3O+ concentration of…

Q: A solution is prepared that is initially 0.46M in trimethylamine ((CH3)3N), a weak base, and 0.49M…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Two students conducted an experiment, where they mixed 6 ml of 0.002M Fe(NO3)3 with 3 ml of 0.050 M…

A: Total volume = 6ml + 3ml + 1ml = 10mlMoles of Fe(NO3)3 solution:

Question

100%

From the value \( K_f = 1.2 \times 10^9 \) for Ni(NH\(_3\))\(_6\) \(^{2+}\), calculate the concentration of NH\(_3\) required to just dissolve 0.014 mol of NiC\(_2\)O\(_4\) (\( K_{sp} = 4 \times 10^{-10} \)) in 1.00 L of solution. (*Hint: You can neglect the hydrolysis of C\(_2\)O\(_4^{2-}\) because the solution will be quite basic.*)

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

C6H4NH₂COOH, para-aminobenzoic acid (PABA) is used in some sunscreens. Calculate the concentrations of hydronium ion and para-aminobenzoate ion, C6H4NH₂COO- in a 0.055 mol dm-³ solution of the acid. Ka-2.2 x 10-5
Eu3* + 3 OH- K = 9.83x10-27 Eu(OH), Calculate equilibrium [Eu³*] and [OH] Cal sp (Csand ic 8
4) Using the information from 1 and 2 above, calculate the concentrations of [Ag*] and [Cr0,2-] if the Ksp of Ag.CrO, is 9.0 x10-12. Hint: Assume [Ag*] = 2x and [CrO,] = x and then solve for x after setting up equilibrium constant expression.
Provide right answers please
a) Pb2+(aq) + Ni(s) -> Ni2+(aq) + Pb(s) b) 0.00010 M Pb2+, 0.20 M Ni2+
What is the solubility of PbCl2 in 0.1429 M NaCl? Ksp(PbCl2) = 1.600e-5.
Please help asap
Taking the Ksp of Zn(OH)2 as 4.0 x 10^-3 and the Kf of [Zn(NH3)6] as 1.0x 10^8, determine how many moles of Zn(OH)2 can dissolve in 0.6 L of 1.2M NH3.
When 2.3 moles of HBrO2 is dissolved in 2 liters of solution it is found at equilibrium that [H3O+] = . 067, calculate ki for HBrO2