Question

A buffer consists of NH4 and NH3 (ammonia). Write the equation for the reaction that occurs...

A buffer consists of NH4 and NH3 (ammonia). Write the equation for the reaction that occurs when strong base (OH–) is added to the buffer.

Write the equation for the reaction that occurs when strong acid (H3O ) is added to the buffer.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

When a Strong Base (OH-) is added in the Buffer the basicity has to be controlled by absorbing (OH-). The reaction taking place will be as following:

            NH4+ (aq.) + OH- (aq.) = NH3 (aq.) + H2O (aq.)

When a Strong Acid (H3O+) is added in the Buffer the acidity has to be controlled by absorbing (H+). The reaction taking place will be as following:

            NH3 (aq.) + H3O+ (aq.) = NH4+ (aq.) + H2O (aq.)

0 0
Know the answer?
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
Similar Questions
You have a buffer composed of NH3 and NH4Cl. Write the reaction that will occur when...
You have a buffer composed of NH3 and NH4Cl. Write the reaction that will occur when some strong acid, H+, is added to the solution. Write the reaction that Will occur when some strong base, OH- is added to the solution.
A buffer contains significant amounts of ammonia and ammonium chloride. Write a net ionic equation showing...
A buffer contains significant amounts of ammonia and ammonium chloride. Write a net ionic equation showing how this buffer neutralizes added acid (HI). Write a net ionic equation showing how this buffer neutralizes added base (Ba(OH)2).
For the following equation label the conjugate acid-base pairs. HC2H3O2 + NH3 <===> NH4+ + C2H3O2-...
For the following equation label the conjugate acid-base pairs. HC2H3O2 + NH3 <===> NH4+ + C2H3O2- 2. The formation of products is strongly favored in this acid-base system: HX + B- <===> HB + X- a) Identify the bases competing for protons. b) Which is the weaker acid in the above equation? Explain. c) Which base is the stronger? Explain. d) How would the equilibrium be affected by the addition of the soluble salt, NaB? e) Would the Keq for...
Write the balanced NET IONIC equation for the reaction that occurs when perchloric acid and sodium...
Write the balanced NET IONIC equation for the reaction that occurs when perchloric acid and sodium hypochlorite are combined. Specify specific states (s) (aq) etc. Use H3O+ instead of H+ This reaction is classified as a: A. Strong Acid + Strong Base B. Weak Acid + Strong Base C. Strong Acid + Weak Base D. Weak Acid + Weak Base The extent of this reaction is: A. ... Below 50% B. ... 50% C. ... Above 50% D. ... 100%
Write a net ionic equation for the reaction that occurs when aqueous solutions of barium hydroxide...
Write a net ionic equation for the reaction that occurs when aqueous solutions of barium hydroxide and perchloric acid are combined. (Use H+ instead of H3O+.) Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrofluoric acid and sodium hydroxide are combined. Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and perchloric acid are combined. Write a net ionic equation for the reaction that occurs when aqueous solutions...
A) Write the balanced NET IONIC equation for the reaction that occurs when nitrous acid and...
A) Write the balanced NET IONIC equation for the reaction that occurs when nitrous acid and potassium hydroxide are combined. This reaction is classified as: _________Strong Acid + Strong Base, Weak Acid + Strong Base, Strong Acid + Weak Base, Weak Acid + Weak Base. The extent of this reaction is: _________Below 50%, 50%, Above 50%, 100%. B) Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and potassium hydroxide are combined. This reaction is...
Part A The following equation shows the equilibrium in an aqueous solution of ammonia: NH3(aq)+H2O(l)⇌NH4+(aq)+OH−(aq) Which...
Part A The following equation shows the equilibrium in an aqueous solution of ammonia: NH3(aq)+H2O(l)⇌NH4+(aq)+OH−(aq) Which of the following represents a conjugate acid-base pair? The following equation shows the equilibrium in an aqueous solution of ammonia: Which of the following represents a conjugate acid-base pair? NH3 and H2O NH4+ and OH− H2O and OH− NH3 and OH− Part Part B What is the conjugate base of HCO3−? Express your answer as a chemical formula. Part Part C What is the...
If a buffer is prepared using 0.55 mol NH4+ and 0.40 mol NH3 in 1 liter...
If a buffer is prepared using 0.55 mol NH4+ and 0.40 mol NH3 in 1 liter of aqueous solution, is the buffering capacity of the solution great enough to maintain its pH if 30 g HI is added? Select one: a. Yes, the concentration of ammonia in the solution is great enough toneutralize the acid. b. Yes, the concentration of ammonium ions in the solution is great enough toneutralize the acid. c. No, the concentration of ammonia in the solution...
Ammonia is a weak base that reacts with water according to this equation: NH3(aq)+H2O(l)<-->NH4+ + OH-(aq)....
Ammonia is a weak base that reacts with water according to this equation: NH3(aq)+H2O(l)<-->NH4+ + OH-(aq). Will any of of the following incrase the percentage of ammonia that is converted to the ammonium ion in water. a) Addition of NaOH b) Addition of HCl c) Addition of NH4Cl
1. what chemical reaction is responsible for the endpoint observed when the NH3/NH4Cl buffer solution is...
1. what chemical reaction is responsible for the endpoint observed when the NH3/NH4Cl buffer solution is titrated with HCl? Write a balanced ionic equation for the reaction. 2. Compare the rate at which pH changes when HCl is added to the buffer solution to the rate of change when no buffer or base is present (distilled water). 3. What effect does dilution of the buffer have on the initial pH, On the pH at the endpoint? On the volume of...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT