Question

Would this result in a buffer solution? 0.1 M HCl (aq) and 0.1 M NaOH (aq)

Would this result in a buffer solution?

0.1 M HCl (aq) and 0.1 M NaOH (aq)
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

A buffer is any type of substance that will resist pH change when H+ or OH- is added.

This is typically achieved with equilibrium equations. Both type of buffer will resist both type of additions.

When a weak acid and its conjugate base are added, they will form a buffer

The equations:

The Weak acid equilibrium:

HA(aq) <-> H+(aq) + A-(aq)

Weak acid = HA(aq)

Conjugate base = A-(aq)

Neutralization of H+ ions:

A-(aq) + H+(aq) <-> HA(aq); in this case, HA is formed, H+ is neutralized as well as A-, the conjugate

Neutralization of OH- ions:

HA(aq) + OH-(aq) <-> H2O(l) + A-(aq) ; in this case; A- is formed, OH- is neutralized as well as HA.

Now,

NaOH = strong base

HCl = strong acid

this will NEVER form a buffer

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
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution? 2. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with...
0.1 M NaOH(aq) and HCl (aq). Both solutions are assumed to have a specific heat capacity...
0.1 M NaOH(aq) and HCl (aq). Both solutions are assumed to have a specific heat capacity of 4.184 J g-1 °C-1. Calculate the ΔH of neutralization for HCl in this reaction and determine whether it’s exothermic or endothermic.
Aspirin Determination using Back Titration Began with 0.1 M HCl solution and 0.1 M NaOH solution....
Aspirin Determination using Back Titration Began with 0.1 M HCl solution and 0.1 M NaOH solution. 1:2 aspirin to NaOH mole ratio, therefore, mol HCl (back titration) = excess mol NaOH AND total mol NaOH used - excess mol NaOH=required mol NaOH AND required mol NaOH (1 mol aspirin / 2 mol NaOH) = mol aspirin. Each step builds off the last 1) Determination of HCl Concentration. This was the first titration. Concentrated HCl was diluted to .1M before titrating....
A 100 mL of buffer solution contains 0.100 M in NH3 (aq) and 0.100 M in...
A 100 mL of buffer solution contains 0.100 M in NH3 (aq) and 0.100 M in NH4Cl. (Q7 ‒ Q9) 7. Calculate pH of the buffer solution. 8. Calculate the change of pH when 4.00 mL of 0.100 M HCl (aq) is added to the buffer solution. 9. Calculate the pH of the solution when 4.00 mL of 0.100 M NaOH is added to the original buffer solution. Please show steps and explain so I can understand how. thank you
A buffer solution is prepared by mixing 50.0 mL of 0.300 M NH3(aq) with 50.0 mL...
A buffer solution is prepared by mixing 50.0 mL of 0.300 M NH3(aq) with 50.0 mL of 0.300 M NH4Cl(aq). The pKb of NH3  is 4.74. 7.50 mL of 0.125 M NaOH is added to the 100.0 mL of the original buffer solution prepared in Question 1 (no HCl added). Calculate the new NH3 concentration for the buffer solution. Calculate the new NH4Cl concentration for the buffer solution. Calculate the new pH of the solution.
a) Calculate the change in pH when 8.00 mL of 0.100 M HCl(aq) is added to...
a) Calculate the change in pH when 8.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). b) Calculate the change in pH when 8.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
A 45.0 mL buffer solution is 0.430 M Na2HPO4 (aq) and 0.330 M KH2PO4 (aq). The...
A 45.0 mL buffer solution is 0.430 M Na2HPO4 (aq) and 0.330 M KH2PO4 (aq). The ka for H2PO4- is 6.2*10-8 a. what is the pH of the buffer solution b. what are the pH and the pH change resulting from the addition of 9.0*10-4 mol of NaOH to the buffer solution c. what are the pH and the pH change resulting from the addition of 9.5*10-4 mol of nitric acid to the initial buffer system d. how many mL...
1) Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to...
1) Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). 2) Calculate the change in pH when 3.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq) 4.00 mL of an unknown...
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq) 4.00 mL of an unknown acid solution containing HCl was added to flask containing 30.00 mL of deionized water and two drops of an indicator. The solution was mixed and then titrated with NaOH until the end point was reached. Use the following titration data to determine the mass percent of HCl in the acid solution. Mass of flask: 125.59 g Mass of flask + acid solution: 129.50 g...
Calculate the change in pH when 5.00 mL of 0.100 M HCl(aq) is added to 100.0...
Calculate the change in pH when 5.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq) Change in pH = _____ Calculate the change in pH when 5.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution. Change in pH= _______
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT