help Which one of the following indicators would be the best choice for a strong acid-weak base titration?Multiple Choicebromocresol green (Ka = 2.5 x 105)thymol blue (Ka = 2.5 × 10-2)bromothymol blue (Ka = 7.9 × 10-8)alizarin yellow R (Ka = 8.9 × 10-12)phenolphthalein (Ką = 5.0 × 10-10)%3D

A suitable indicator for the titration of the weak acid CH3COOH(aq) and the strong base NaOH(aq)…

h one of the following indicators would be the best choice for a strong acid-weak base titration? Multiple Choice bromocresol green (Ka = 2.5 × 10-5) thymol blue (Ka = 2.5 × 10-2) bromothymol blue (Ką = 7.9 × 10-8) alizarin yellow R (Ka = 8.9 x 10-12) phenolphthalein (Ką = 5.0 × 10-10)

h one of the following indicators would be the best choice for a strong acid-weak base titration? Multiple Choice bromocresol green (Ka = 2.5 × 10-5) thymol blue (Ka = 2.5 × 10-2) bromothymol blue (Ką = 7.9 × 10-8) alizarin yellow R (Ka = 8.9 x 10-12) phenolphthalein (Ką = 5.0 × 10-10)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.85QE

See similar textbooks

Related questions

Q: What is the buffer range for a benzoic acid/sodium benzoate buffer (Ka for benzoic acid = 6.3 x 10-5…

A: Using Henderson Hesselblack equation PH = Pka + log Salt/acid PH = -log Ka + log salt/acid

Q: 50.00 mL of benzoic acid (HC7H5O2) 0.1000 mol L-1 are titrated with NaOH 0.1000 mol L-1. Calculate…

A: Given: Volume of benzoic acid = 50.00 mL Concentration of benzoic acid = 0.100 mol/L Concentration…

Q: The indicator thymol pink has a Ka = 2 x 10-4. At pH =1 it is yellow and at pH=14 it is pink.…

A: This question belongs to strong acid and weak base titration using a thymol pink indicator. find the…

Q: Identify which of the graphs represent the given titration experiments best. Graph A Graph B 12 12…

A: Titration is a process in which amount of solute in a solution of unknown concentration is…

Q: Which indicator should you use for a titration between a strong acid and a strong base? A.)…

A: Since we know that for a strong acid-strong base titration, the equivalence point is at pH 7.

Q: A 50.00-mL sample of a 1.00 M solution of the diprotic acid H2A (Ka1 = 1.0 × 10–6 and Ka2 = 1.0 ×…

Q: Construct a curve for the titration of 15.00 mL 0.1500 M HCN using 0.1500 M KOH as titrant. Use MS…

A: In strong acid -strong base titration, neutral solution is formed on neutralization. At equivalence…

Q: 1. On each graph, identify an indicator that could be used in the titration, and write the name of…

A: A suitable indicator is the one, that gives color change during equivalence point. Equivalence…

Q: pH vs. VB 14 12 10 4 25 50 75 100 VBase (mL) Based on the titration curve, which acid was most…

A: pKa = -log(Ka) For Ascorbic acid, pKa = -log(7.9*10-⁵) =4.10 Chloroacetic acid, pKa = -log(1.4*10-³)…

Q: Identify each type of titration curve. Note that the analyte is stated first, followed by the…

A: Equivalence point of strong acid and strong base will at pH = 7, resulting solution be neutral.…

Q: Please click on an indicator which would be appropriate for the titration illustrated in the plot on…

A: A question based on analytical process that is to be accomplished.

Q: pH Indicator 1 7 8. 9 10 11 12 Colorless Phenolphtalein Bromthymol Blue Methyl Orange Pink Yellow…

A: Given that :

Q: How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M hypochlorous acid…

A: Given: Molarity of NaOH = 0.120 M (i.e. mol/L) Molarity of hypochlorous acid [HOCl] = 0.0998 M (i.e.…

Q: What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to…

Q: Hydrofluoric acid (HF) has a Ka value of 7.2 x 10^-4. What is the pH to 2 decimal places of a 27.5…

A: NOTE: for second question concentration of sodium hydroxide is not provided. So that question could…

Q: circle green: ph 1 of weak acid as the analyte and a strong base as the titrant. Dark green square:…

A: The question is based on the concept of titrations. We are titrating different kind of acid with a…

Q: 3) Calculate the pH after titration of 30.00 mL of 0.10 M HOCl solution (ka=2.9x10^-8) with 25.00 mL…

Q: 1. On each graph, identify an indicator that could be used in the titration, and write the name of…

A: An indicator is a substance which is used to determine the end point of titration, it changes its…

Q: Which one of the following indicators would be best to use when titrating 0.1M morphine (Kb = 1.6 ×…

A: pH is a measure of hydrogen ion concentration in solution and it measures acidity or alkalinity of a…

Q: A solution has a pH of 4.5. What would be the color of the solution if each of the following…

A: (a) bromphenol blue blue color (b) bromthymol blue colorless

Q: Determine the Ka of each solution Sol. A – 20 mL of 1.00 NaA and 10 mL of 1.00 M HA Sol. B – 20…

A: Acidic buffer and use of Henderson hasselbalch equation for pH calculation:

Q: Below is a titration curve for the titration of 50.0 mL of a 0.100 M solution of the weak acid HA…

Q: 13,How many milliliters of 0.0854 M NaOH are required to titrate 25.00 mL of 0.1250M HI to the…

Q: Consider the titration of 50.00 mL of 0.100 M CH3CO2H with 0.200 M KOH, calculate the pH after…

Q: A buffer solution with pH = 5.0 is required, which one of the following acid, together with its…

A: The pH value of a buffer solution mainly depends upon the pKa value of the acid. If the pKa value of…

Q: The pH of the buffer containing 0.0005 M acetic acid and 0.00045 M sodium acetate

A: Given :- [Acetic acid] = 0.0005 M [Sodium acetate] = 0.00045 M Ka = 1.75 × 10-5 To calculate :-…

Q: Consider the titration of 50.00 mL of 0.100 M CH3CO2H with 0.200 M KOH, calculate the pH after…

A: The question is based on the concept of titrations. we are titrating a weak acetic acid with a…

Q: Given the following buffer systems, the acetate buffer system would be the best choice to create a…

A: Answer: A buffer solution is the type of solution that resist the change in its pH on adding small…

Q: 3. Formic acid is a weak acid with Ka = 1.7 x 10-4, How would you make 50 mL of a pH 4.00 buffer…

Q: A 50.0 ml of acidic solute (Ka = 1.20 x 10-2) is titrated with a %3D 2.50 mL of 1.00 x 10-5 M NAOH…

A: Given: Ka of acid solute = 1.20 X 10-2 Volume of acid solution = 50.0 mL = 0.050 L…

Q: CH3COOH+ NaOH The first titration used phenolphthalein, the endpoint was 43.5ml The second titration…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: 2 of 14 Another student is investigating the change in pH during a titration where sodium hydroxide…

Q: A mixture of NaOH (M.wt = 40) and Na2CO3 (M.wt = 106) is titrated with 0.3 M HCl, requiring 30 mL…

A: The equations of titration are : For the titration using phenolphthalein indicator,…

Q: Suppose that you titrate 50.0 mL of 0.15 M HNO2 with 0.20 M NaOH. Given that the Ka for HNO2 is 4.0…

A: Since you have asked a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka = 1.54 ×…

Q: Consider the following indicators: dinitrophenol (pKIn = 3.5), bromothymol blue (pKIn = 7),…

A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: Answer the following question about a titration between 25.0 mL of a weak acid (Ka= 6.2*10-5) and…

A: Given: Ka of weak acid = 6.2*10-5 Concentration of NaOH = 0.120 M pKa of resorcin blue ~ 5.3 pKa of…

Q: One erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other erlenmeyer contains 50 mL of 0.1 M…

A: A question based on concentration terms that is to be accomplished.

Q: Let HA represent a weak acid. A 10.0 mL sample of 0.60 M HA was titrated with 0.30 M NaOH. The…

A: The pH of a weak acid and dissociation constant (Ka) are related by the following Henderson…

Q: Propanoic acid has a Ka=1.3x10-5. The titration starts with 40.00 mL of 0.1000 M propanoic acid…

A: The question is based on the concept of titrations. we are titrating a weak propanoic acid with a…

Q: The indicator thymol pink has a Ka = 2 x 104. At pH =1 it is yellow and at pH=14 it is pink. Which…

A: The indicator thymol pink gives yellow colour in a solution with a pH = 1 and gives a pink colour at…

Q: What is the pKa of an acid titrated with 1.0 M NaOH that generates a titration curve shown below? 14…

Q: 15 10 10 12 16 18 20 22 24 Volume of NaOH Added (mL) Where is the equivalence point?

A: Equivalence point: The point at which the moles of acid added equals the moles of base that you…

Q: What is the pH of 50.00 mL buffer solution which is 2.00M of HC2H3O2 and NaC2H3O2 each? (Ka=1.8x…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: Aniline, the molecule pictured above, is 0.125 M with a volume of 350 mL and is titrated with 0.250…

A: Given data,Molarity of aniline=0.125MVolume of aniline=300mLMolarity of HBr=0.250MKb of…

Q: Propanoic acid has a Ka=1.3x10-5. The titration starts with 40.00 mL of 0.1000 M propanoic acid…

A: Titration is a quantitative analysis in which the concentration of unknown solution can be find by…

Q: A buffer solution containing equimolar amounts of the base, aniline, and the salt of its conjugate…

A: Interpretation: The given statement is true or false is to be determined. Given statement: A buffer…

Q: A titration experiment has an equivalence point near pH = 9.0. What indicator should be used for…

Q: What should be the pH range of an indicator that has a Kb of 5.21x104? Hide answer choices A 3.28 to…

A: Kb = 5.21 × 10-4 M

Question

help

Which one of the following indicators would be the best choice for a strong acid-weak base titration?
Multiple Choice
bromocresol green (Ka = 2.5 x 105)
thymol blue (Ka = 2.5 × 10-2)
bromothymol blue (Ka = 7.9 × 10-8)
alizarin yellow R (Ka = 8.9 × 10-12)
phenolphthalein (Ką = 5.0 × 10-10)
%3D

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the following indicators: dinitrophenol (pKIn = 3.5), bromothymol blue (pKIn = 7), thymolphthalein (pKIn = 10). Match each titration below with its most-likely best indicator. (A specific indicator choice may be used more than once.) Group of answer choices titration of HF with NaOH [ Choose ] dinitrophenol bromothymol blue thymolphthalein titration of RbOH with HNO3 [ Choose ] dinitrophenol bromothymol blue thymolphthalein titration of HI with KOH [ Choose ] dinitrophenol bromothymol blue thymolphthalein titration of NH3 with HBr [ Choose ] dinitrophenol bromothymol blue thymolphthalein
Titration 1 Titration 2 Titration 3 Volume of HCl solution (mL) 5.0 ml 5.0 ml 5.0 ml Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 45.61 ml 45.56 ml 45.64 ml Volume of NaOH used (mL)
Which of the following indicators would be the best to use when 0.050 M benzoic acid (Ka = 6.6 × 10-5) is titrated with 0.05 M NaOH? alizarin, pH range: 5.7-7.2 bromocresol green, pH range: 3.8-5.4 phenol red, pH range: 6.4-8.0 methyl yellow, pH range: 2.7-4.0 naphtholphthalein, pH range: 7.3-8.7
circle green: ph 1 of weak acid as the analyte and a strong base as the titrant. Dark green square: ph 2 of strong acid as the analyte and the strong base as a titrant.
Given the transition range for the pH indicators below, which indicator is most appropriate for the titration of a weak acid with a strong base? cresol purple transition 1.2-2.8; bromocresol purple pH transition: 5.2-6.8; cresol red pH transition: 7.0-8.8 a. cresol purple b. bromocresol purple c. cresol red
The indicator thymol pink has a Ka = 2 x 10-4. At pH =1 it is yellow and at pH=14 it is pink. Which of the following statements are true (select all that apply) It is a good indicator for a weak acid with strong base titration at pH = 4 it will be yellow its end point will occur when the pH is approximately equal to 9 It is a good indicator for strong acid with weak base titration If it is added to a solution of 1 M sodium nitrite the solution will turn pink
An employer is interviewing 4 applicants for a job as a laboratory technician and askseach of them how to prepare a buffer solution with a pH close to 11.000.Use these ka’s to help you: Show your workPropionic Acid, CH3CH2COOH, ka = 1.34 x 10-5 Ethanamine, CH3CH2NH2, kb = 6.3 x 10-4 Jung says he would mix CH3CH2COOH & CH4CH3COOHDominique says she would mix CH3CH2 NH2 & CH3CH2COOHJoshua says he would mix CH3CH2COOH & CH3COONaKyla says she would mix CH3CH2NH2 & CH3CH2NH3BrWho would you hire based on their ability to make a buffer?_________________________
Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________
1Upon the addition of 30.00 mL of 0.350 M HCl to a 80.00-mL of the weak base amine (Kb = 4.95 x 10-10) whose concentration is 0.530M, the resulting pH is then equal to 8.80. True or False? 2.When 100 mL of a 1.0M strong acid is 50% titrated with 1.0M strong base, the volume of the base should be added is 50mL and this corresponds the equivalence point. True or False? 3. The pH of a buffer can be calculated using the formula: 14-pOH = pKb + log of [proton acceptor]/[acid component]. True or False?
Using the letters on the image, identify each component of the titration set-up. Buret clamped to a ring stand with a beaker underneath. The letter A appears at the top of the buret, the letter B appears midway down the buret, the letter C appears at the bottom of the buret, the letter D appears next to the beaker, and the letter E appears on the other side of the buret, near the ring stand.
analytical chemistry. Given the following titration curve, what is the suitable indicator for this titration? a) thymolphthaline; pH range (9.3-10.5) b) bromothymol blue; pH range (6.2-7.6) c) Thymol blue; pH range (1.2-2.8) d) bromcresol green; pH range (4.1-5.4) e) phenolphthalein; pH range (8.6-10.2)
1.Which of the following substances have a solvatochromic property? a.potassium hydrogen phthalate b.sodium carbonate c.sodium bicarbonate d.bromocresol green 2.If the pKa of the indicator is approximately 6, to which of the following equivalence point will it be most suitable? a.pH 10 b.pH 13 c.pH 4 d.pH 53. Referring to the figure below, what volume of the titrant was used to reach half-neutralization equivalence point? a.25 mLb.20 mLc.50 mLd.56 mL