Log in
Chemistry
1
answer
0
watching
447
views
13 Dec 2019

a) Write the dissolution reaction for lead(II) iodide. How many grams of lead(II) iodide will dissolve in 250.0 mL of water? What are the molarities of lead(II) ion and iodide ion? Neglect any volume change due to the lead(II) iodide. Ksp of lead(II) iodide = 1.4 x 10-8

b) How many grams of lead(II) iodide will dissolve in 250.0 mL of 0.35 M HI?

c) Will the solubility of lead(II) iodide in 250.0 mL of 0.35 M HNO3 be the same as (a) or (b) ?

d ) How would the answers to (a) and (c) have compared if the salt under consideration were lead(II) fluoride, rather than lead(II) iodide? Ksp PbF2 = 7.1 x 10-7 KaHF = 7.2 x 10-4

e ) Lead(II) ion forms a 1:1 complex with a particular ligand, L (forms PbL2+) . Write the reaction for formation of the complex ion using “L” as the ligand. If the formation constant for this complex is 2.9 x 104 , calculate the solubility of lead(II) iodide in a 1.5 M solution of L.

Watch
1
answer
0
watching
447
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Elin Hessel
Elin HesselLv2
17 Dec 2019

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

1-A 3.744 g sample of copper(II) nitrate is dissolved in water and 2.000 g of copper(II) arsenate (Ksp = 7.6 x 10-36) is added so that the total solution volume is exactly 1 L. What is the concentration of the arsenate ion in the solution (assuming the arsenate ion does not react with water)? (b) If the arsenate ion does react with water, write the principal chemical equation and determine K.

2- Argentous iodide (Ksp = 8.32 x 10-17) is considerably less soluble than argentous chloride (Ksp = 1.82 x 10-10). Determine the stoichiometric concentration of (a) ammonia and (b) sodium thiosulfate that is required to dissolve argentous iodide, such that the total dissolved silver concentration is 0.100 M. (The equilibrium constants (K1, K2) for the stepwise formation of the argentous-ammine and argentous-thiosulfate complexes are 2.1 x 103 , 8.2 x 103 and 7.4 x 108 , 3.9 x 104 , respectively.)

Write the balanced chemical equation for the reaction between aqueous lead (II) nitrate and aqueous sodium chloride: The Ksp for PbCl2 is 1.6 x 10-5 at 25°C. a. Write the Ksp expression: b. Will a precipitate form when 100. mL of .400 M lead (II) nitrate and 100. mL of .200 M sodium chloride are mixed? How do you know? c. What is the concentration of all ions present after the reaction occurs?

(2) Citric acid (H3C6H5O7) occurs in plants. The acid is added to beverages and candy. An aqueous solution is 0.710 m in citric acid. The density is 1.049 g/mL. Calculate the concentration of this solution as: (w/w %) (w/v %) M Mole Fraction (citric acid) 2

(3) When 75.0 mL of a 0.100 M lead (II) nitrate solution is mixed with 100.0 mL of a 0.190 M potassium iodide solution, a yellow-orange precipitate of lead (II) iodide is formed. a. Write the balanced molecular and net-ionic equation. b. Assuming 100% yield calculate the mass of lead (II) iodide formed. c. Determine the molarities of ions left in solution after the reaction.

(4) A 15.00 mL solution of KNO3 was diluted to 125.0 mL and 25.00 mL of this solution was then diluted to 1000. mL. The concentration of KNO3 in the 1000. mL is 0.00383 M. What was the M of KNO3 in the original solution? 3

(5) How many grams of pure H2SO4 can be obtained from 250 g of iron ore if the ore is 82.0 % (w/w %) FeS2. The reactions involved are given below: 4FeS2 + 11O2 → 2Fe2O3 + 8SO2 (95.0% efficient) 2SO2 + O2 → 2SO3 (90.0 % efficient) SO3 + H2O → H2SO4 (90.0 % efficient)

(6) 30.0 mL of 0.512 M sulfuric acid was added to 25.0 mL of 0.666 M sodium hydroxide. a. Write the balanced chemical equation. b. Determine the molarity of either acid or base remaining after the reaction. c. Find the molarity if a 50.00 mL aliquot of this solution is diluted to 250. mL.

(8) Oxygen is produced by the reaction: 2KClO3 (s) →2KCl (s) + 3O2 (g)  The oxygen produced was collected over water. A sample of KClO3 produced 705 mL of oxygen saturated with water vapor at 20.0 °C where the vapor pressure of water is 17.54 mm Hg. The total gas pressure was 1.104 atm. What mass of KClO3 decomposed?

(9) How many grams of C2H2 must burn according to the equation below in order to heat 2.34 × 104 g of H2O from 25.0 °C to 35.0 °C? C2H2 (g) + O2 (g) →H2O (l) + CO2 (g), Δ = – 1212 kJ

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in