HomeworkLib
Question

In which of the following reactions does water act as a Lewis Base? And reasons why?...

In which of the following reactions does water act as a Lewis Base? And reasons why?

1. HB+(aq)+H20(l)<---->B(aq)+H3O+(aq)

2.NH3(aq)+H2O(l)<--->NH4+(aq)+OH^-1(l)

3. Al^3+(aq)+6H20(l)<----->[Al(H2o)6]^3+(aq)

4.CO2(g)+H20(l)<------->H2CO3(aq)

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

According to lewis acid-base theory, which accepts a proton is a base.

HB+(aq)+H2O(l)<---->B(aq)+H3O+(aq) in this reaction, H2O accepting a proton from HB+ and forming H3O+. so here it is acting as a lewis base.

Thank you and good luck.

0 0
Add a comment
Know the answer?
Add Answer to:
In which of the following reactions does water act as a Lewis Base? And reasons why?...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • For each of the following reactions, identify which reactant is the Lewis base. Select 1 if...

    For each of the following reactions, identify which reactant is the Lewis base. Select 1 if the first listed reactant is the Lewis base or 2 if the second listed reactant is the Lewis base. 2F- + SiF4 --> SiF62- H3O+ + N2H4 --> N2H5+ + H2O Zn2+ + 4NH3 --> Zn(NH3)42+ OH- + CO2 --> HCO3-

  • Can someone explain why the answer is E? 1.) For which of the following equilibria does...

    Can someone explain why the answer is E? 1.) For which of the following equilibria does Ka correspond to an acid-ionization constant, Ka? А NH3(aq) H3O (aq) NH4 (aq) H20() В NH4 (aq)OH (aq) NH3(aq) + H2O( С F(aq)H20()= HF(aq)OH(aq) HF(aq) OH(aq) H20()F(aq) NH4 (aq)H20() NH3(aq) H30*(aq)

  • Identify conjugate acid-base pairs in each of the following reactions. NH3(aq) + H2O(l) = NH4+ (aq)...

    Identify conjugate acid-base pairs in each of the following reactions. NH3(aq) + H2O(l) = NH4+ (aq) + OH- (aq) Check all that apply. H2O/NH3 NH4+/NH3 H2O/OH NH4+/OH- Submit Request Answer Part B OH(aq) + HF(aq) = H20(1)+F- (aq) Check all that apply. H2O/F- H20/OH HF/F- HF/OH

  • 12. The pK, for NH4 is 9.26. This expression refers to which of the following reactions?...

    12. The pK, for NH4 is 9.26. This expression refers to which of the following reactions? A. NH4+ (aq) + OH(aq) + NH3(aq) + H2O(aq) B. NH4+ (aq) + H2O(l) NH3(aq) + H30+(aq) C. H3O+(aq) + OH(aq) → 2H2O(1) D. NH3(aq) + H30+(aq) NH4+ (aq) + H2O(l) E. NH3(aq) + H2O(1) NH4+ (aq) + OH (aq)

  • Calculate the pH of a 0.10 M solution of aluminum chloride, which dissolves completely in water...

    Calculate the pH of a 0.10 M solution of aluminum chloride, which dissolves completely in water to give the hydrated aluminum ion [Al(H2O)6]3+ in solution. Al3+(aq) + H2O(l) → [Al(H2O)6]3+(aq) [Al(H2O)6]3+(aq) + H2O(l) → [Al(H2O)5OH]2+(aq) + H3O+(aq) Ka = 1.4 x 10-5 Soda water (carbonated water) is a solution of carbon dioxide in water. The solution is acidic because CO2 reacts with water to form carbonic acid, H2CO3. What are [H3O+], [HCO3-], [CO3-2] in a saturated solution of CO2 with...

  • Identify conjugate acid-base pairs in each of the following reactions.

    Identify conjugate acid-base pairs in each of the following reactions. NH3(aq) + H2O(l) ⇌ NH4+ (aq) + OH- (aq) Check all that apply. H2O/NH3 NH4+/NH3 H2O/OH NH4+/OH- Part B OH-(aq) + HF(aq) ⇌ H2O(1)+F- (aq) Check all that apply. H2O/F- H2O/OH HF/F- HF/OH-

  • Answer the question below: 1: i) Identify the Lewis acids and bases in each of the...

    Answer the question below: 1: i) Identify the Lewis acids and bases in each of the following reactions: a. NH3 + BF3 → F3B NH3 b. H2O + SO3 → H2SO4 c. NH4+ + OH- → NH3 + H2O d. CO2 + H2O → H2CO3 e. OH−+H+→H2O ii) Identify the following compounds as either a Lewis acid or Lewis base and as either Soft or Hard: a. Cr3+ b. SO3 c. SCN− d. I

  • 1. Which of the followi ch of the following reactions is not readily explained by the...

    1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...

  • 1. For each reaction below Classify each acid, base, conjugate acid, and conjugate base as a...

    1. For each reaction below Classify each acid, base, conjugate acid, and conjugate base as a strong acid, weak acid, strong base, or a weak base. Calculate the value of the equilibrium constant II. I. Determine if these reactions need to be treated as an equilibrium (needing an ICE table) or a stoichiometry problem (assuming the reaction goes essentially to completion) a. F-(aq) H2O() HF(aq) + H3O*(aq) + H2O(1) NH3(aq) + b. NH4 (aq) OH (aq) + H3O*(aq) NH3(aq) +...

  • 6. Complete the following acid base reactions, indicate the conjugate acid-base pairs, and state whether the...

    6. Complete the following acid base reactions, indicate the conjugate acid-base pairs, and state whether the reaction has a large or small equilibrium constant. a. CH3COOH(aq) + NH3(aq) = b. H2CO3 (aq) + NO3- (aq) = H2CO3 (aq) + H20 (0) = d. HCO3- (aq) + H2O (1) = (HCO3- is amphoteric!) e. NH3 (aq) + H20 (1) =

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT