Question

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.

Homework Answers

Answer #1

NH3(aq) + H+(aq) --------> NH4+(aq)

NH4+(aq) + OH-(aq) --------> NH3(aq) + H2O(l)

Explanation

A buffer is a combination of weak acid and its salt with strong base or weak base and its salt with strong acid

NH3 is weak base and NH4Cl is the salt of the reaction between NH3 and strong acid HCl

NH4+ is conjucate acid of weak base NH3

when H+ ions are added it reacts with NH3

NH3(aq) + H+(aq) --------> NH4+(aq)

when OH- ions are added it reacts with

NH4+(aq) + OH​​​​​​-(aq) -------> NH3(aq) + H2O(l)

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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.
You have a 750mL of a buffer solution that is composed of NH3 and NH4Cl with...
You have a 750mL of a buffer solution that is composed of NH3 and NH4Cl with a Kb value 1.8x 10^5 and a pH 9.43...... How many mL of 6.00M NaOH can be added before the buffer is exhausted?
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...
Compare the rate at which pH changes when HCl is added to the buffer solution(NH3/NH4Cl) to...
Compare the rate at which pH changes when HCl is added to the buffer solution(NH3/NH4Cl) to the rate of change when no buffer or base is present (distilled water).
An ammonium buffer was prepared from 50.0ml of 0.145M NH3 and 25.0ml of 0.254M NH4Cl. a)...
An ammonium buffer was prepared from 50.0ml of 0.145M NH3 and 25.0ml of 0.254M NH4Cl. a) Write out the reactions involved in the above solution. (can be more than one) b) what is the pH of initial buffer, NH3 Kb = 1.8 e^-5 c) what is the pH of this solution if you add 2.0ml of a strong acid, 1.1M HCl, to above buffer. Show all reactions.
A buffer consists of 0.26 M NH4Cl and 0.36 M NH3. What is the pH of...
A buffer consists of 0.26 M NH4Cl and 0.36 M NH3. What is the pH of the buffer after 0.003 moles of Ca(OH)2 are added to 0.10 L of this buffer solution. Kb for NH3 is 1.8×10‒5.
a buffer solution is prepared by mixing 45.0 mL of 0.100M NH3 are mixed with 25.0...
a buffer solution is prepared by mixing 45.0 mL of 0.100M NH3 are mixed with 25.0 mL of 0.200M NH4Cl. calculate the pH of the solution and, with the help of appropriate chemical equations, describe how this buffer works. Include some comments about its capacity for absorbtion of strong acid and strong base.
A buffer is prepared by adding 12.0g of ammonium chloride (NH4Cl) to 240mL of 1.00 M...
A buffer is prepared by adding 12.0g of ammonium chloride (NH4Cl) to 240mL of 1.00 M NH3 solution. Part A What is the pH of this buffer? Part B Write the complete ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. Express your answer as a chemical equation. Identify all of the phases in your answer. Part C Write the complete ionic equation for the reaction that occurs when a...
Write chemical equation to show a buffer made of a mixture of a solution of acetic...
Write chemical equation to show a buffer made of a mixture of a solution of acetic acid CH3COOH and its sodium salt CH3COONa can resist changes in pH, when H+ or OH- ions are added to the buffer system. Buffer +Acid Buffer +base
1. What is the pH of a buffer solution that is .24M NH3 and .20M NH4Cl?...
1. What is the pH of a buffer solution that is .24M NH3 and .20M NH4Cl? If .005 mol of NaOH is added to .50L of the buffer solution from question 1, what is the resulting pH? If .03 mol of HCl is added to .05L of the buffer solution from question 1, what is the resulting pH?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT