🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
Chemistry
1
answer
0
watching
141
views
13 Dec 2019

1.Determine how many of the following salts are acidic.

NH4Br

AlCl3

KClO4

NaClO

Li2C2O4

Na2SO3

2.The pKa for the ammonium ion (NH4+) in water is 9.3. What is the pH of a 100mL solution that contains 0.20M ammonium ion and 0.10M ammonia?

NH4+(aq) + H2O(l) ? H3O+(aq) + NH3(aq)

Watch
1
answer
0
watching
141
views

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

Deanna Hettinger
Deanna HettingerLv2
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
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
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. Liquid Plumber, a drain cleaner, has a pH of 14.32. What is the pOH of this solution and what is the hydroxide ion concentration?answer pOH -0.33 [OH^+]2.1M

2. A solution is made with [Pb2+] = 2.5x10-3 M and [I-] = 4.0x10-3M. What is the reaction quotient, Q, for the dissolution of PbI2(s) in water? Do you expect PbI2(s) to precipitate? Ksp(PbI2) = 6.5x10-4

answer) Q=4.0X10^-8 precipitate:no

3.The pKa for the ammonium ion (NH4+) in water is 9.3. What is the pH of a 100mL solution that contains 0.20M ammonium ion and 0.10M ammonia?

NH4+(aq) + H2O(l) ? H3O+(aq) + NH3(aq)

Answer:9.0

i just need explanations.. answer provided

1) Find the pH of 0.151 M phenol, C6H5OH. The H bonded to the O is acidic, that is,
C6H5OH(aq) + H2O(l) ↔ H3O+(aq) + C6H5O-(aq). Ka = 1.0 x 10-10 M.

2) Calculate the approximate [OH-] and [NH4+] in a 0.15 M ammonia solution, NH3(aq).
NH3(aq) + H2O(l) ↔ OH-(aq) + NH4+(aq). Kb = 1.75 x 10-5M.

3) Calculate the pH of 0.197 M ammonia.
NH3(aq) + H2O(l) ↔ OH-(aq) + NH4+(aq) Kb = 1.75 x 10-5

4) Calculate the pH of 0.124 M phosphoric acid (H3PO4, a triprotic acid). Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13.

1. A solution has [H3O+] = 5.4×10−5 M . Use the ion product constant of water Kw=[H3O+][OH−] to find the [OH−] of the solution. Express your answer to two significant figures.

2.A solution has [OH−] = 2.1×10−2M . Use the ion product constant of water Kw=[H3O+][OH−] to find the [H3O+] of the solution. Express your answer to two significant figures.

3. An ammonia/ammonium buffer solution contains 0.27 M NH3 and 0.79 M NH4+. The Kb value of ammonia is 1.8×10−5. Calculate the pH of this buffer. Express the pH numerically.

Weekly leaderboard

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