HomeworkLib
Question

Titration Solution: KOH -H2O -HCl Titration Solution: HCl -H2O -NaOH -Tris Base Titration Solution: KOH -Vinegar...

Titration Solution: KOH

-H2O

-HCl

Titration Solution: HCl

-H2O

-NaOH

-Tris Base

Titration Solution: KOH

-Vinegar

-HCOOH

Titration Solution: KOH

-H3PO4

-H2SO4

- Which of these are buffering solutions? Of the buffering solutions what are their buffering ranges?

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

Homework Answers

Answer #1

KOH + HCOOH = acidic buffer having PH 5 - 6.5

Because it is mixture of weak acid and strong base. here strong base( KOH ) are present in small amount which react with weak acid HCOOH and form salt of weak acid with strong base which is neutral . but here still HCOOH are present so final solution is acidic. and since HCOOH is not 100% ionizable acid so PH is also near 5 to <7.

KOH + H3PO4 = Acidic buffer.

here H3PO4 is weak acid which mixed with strong base nd form salt. same explanation as explained in above case.

0 0
Add a comment
Know the answer?
Add Answer to:
Titration Solution: KOH -H2O -HCl Titration Solution: HCl -H2O -NaOH -Tris Base Titration Solution: KOH -Vinegar...
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

  • KOH was titrated into H2O and then KOH was titrated into HCl, HCl was titrated into...

    KOH was titrated into H2O and then KOH was titrated into HCl, HCl was titrated into H2O and then HCl was titrated into NaOH and then HCl was titrated into tris base, KOH was titrated into vinegar and then KOH was titrated into HCOOH, KOH was titrated into H3PO4 and KOH was then titrated into H2SO4. I do not know which of these would be a buffer to answer the question below. Which are these would be buffers? Of the...

  • A titration of vinegar with a solution of NaOH was performed. If 3.35 mL of vinegar...

    A titration of vinegar with a solution of NaOH was performed. If 3.35 mL of vinegar needs 45.0 mL of 0.135 M NaOH to reach the equivalence point in a titration CH3COOH(aq)+NaOH(aq)→H2O(l)+NaC2H3O2(aq) Part A: Calculate the mass of acetic acid present in the vinegar sample? Part B: How many grams of acetic acid are in each mL of vinegar? Part C:How many grams of acetic acid would be in a 1.60 qt sample of this vinegar? Part D: How many...

  • Tris-HCI in solution will produce a pH of approximately 4.7 and Tris-Base in solution will produce...

    Tris-HCI in solution will produce a pH of approximately 4.7 and Tris-Base in solution will produce a pH of approximately 10.4. Which one has the better buffering capacity?

  • Titration of a Weak Base Prelaboratory Questions 1. Will addition of HCl to a solution make...

    Titration of a Weak Base Prelaboratory Questions 1. Will addition of HCl to a solution make it more acidic or more basic? Will the pH increase or decrease? How does an end point differ from an equivalence point? 2. were titrated with a standard HCl solution: 3. Aliquots of an unknown tris sample Use the balanced equation to set up the string calculation showing how the tris a. mol of acid, L of acid. mo of base, and L of...

  • (HOCH2)3CNH2 + H2O = (HOCH2)2CNH3+ + OH amonia, tris reacts with HCl to form a hydrochloride...

    (HOCH2)3CNH2 + H2O = (HOCH2)2CNH3+ + OH amonia, tris reacts with HCl to form a hydrochloride salt, tris-HÇi. (HOCH2)3CNH2 + HCl → (HOCH2)3CNH3* + Cl-, Aliquots of an unknown tris sample were titrated with a standard HCl solution: a. Use the balanced equation to set up the string calculation showing how the tris concentration will be calculated. Use of acid, L of acid, " of base, and L of base to represent the reactants. Remember the calculation must include a...

  • a) Calculate the pH of a titration of 100 mL 1.5M HCl with 1.25M NaOH at...

    a) Calculate the pH of a titration of 100 mL 1.5M HCl with 1.25M NaOH at equivalence. WHY is the pH what it is (if it’s 7, why is the solution neutral? If not 7, why?) b) Calculate the pH of a titration of 100 mL 1.5M HCOOH (Ka = 1.8 x 10-4) when 75 mL 1.25M NaOH has been added. c) What volume of 1.25M NaOH must be added to 100 mL of 1.5M HCOOH to reach equivalence?

  • A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution....

    A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution. 19.6 mL HCl was required to reach equivalence point. In a separate titration, a 10.0 mL H3PO4 solution was titrated with the same NaOH solution. This time, 34.9 mL NaOH was required to reach the equivalence point. What is the concentration of the H3PO4 solution?

  • The vinegar in this titration was distilled vinegar which is colorless. what modifications would we need...

    The vinegar in this titration was distilled vinegar which is colorless. what modifications would we need to do in this procedure so that we could test OTHER solutions such as cider vinegar or pickling liquor which both have a SIGNIFICANT COLOR it requiretion? (All of the hydrofion of this reacti la S- g the Solution. The water does not Cause any any no matter che change how in the # of er moles of CH₃COOH how much water is thing...

  • A. Titration of a 11.0 mL solution of KOH requires 12.0 mL of 0.0310 M H2SO4 solution. B. If 28.0 mL of a 0.200 N acid solution is needed to reach the end point in titration of 17.5 mL of a base solut...

    A. Titration of a 11.0 mL solution of KOH requires 12.0 mL of 0.0310 M H2SO4 solution. B. If 28.0 mL of a 0.200 N acid solution is needed to reach the end point in titration of 17.5 mL of a base solution, what is the normality of the base solution?

  • In an acid base titration 22.13 ml of an NAOH

    In an acid-base titration, 22.13 mL of an NaOH solution arc needed to neutralize 24.65 mL of a 0.1094 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of M_H+ in the HCl solution. ________ M Find M_OH^- in the NaOH solution. (Use Eq. 3.) ________ M Obtain M_NaOH from M_OH^-. ________ M In an acid-base titration, 22.13 mL of an NaOH solution arc needed to neutralize 24.65...

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