Answer Questions #27 through #31 about the titration curves below (labeled a and b) for two differentbases. The titrant acid used in both cases was 0.100 M HCl and the volume of the base solutions in bothcases was 75.0 mL mL.14141212 -10-108-6.4.2-2-2040608010020406080100Volume of acid added (mL)(a)(b)Volume of acid added (mL)2014 Pearson Education IncP Type here to search11:17 AM(?3/18/2021->ort sc806.ecenumER/TY ||на0 04 2CHd 28. Which of the two titrations has a base solution that is more concentrated?A) (a)B) (b)C) Both (a) and (b) are the same concentrationD) It is impossible to say without knowing the exact Kp values of the two bases.E) Titrating with HCl won't work. You need to use another acid in the titration.29. Which titration has the stronger base (larger Kb value)? Be careful: Make sure you compare the Kp values ofthe bases, not the Ka values of the conjugate acids. Also, don't forget the relationship between Kband pKb.A) (a)B) (b)C) Both (a) and (b) are the same pKp.D) It is impossible to say without knowing the exact Kb values of the two bases.E) Titrating with HCl won't work. You need to use another acid in the titration.30. Could the base titrated in (b) be used as part of a buffer? If so, what pH could be maintained by this buffer?A) Yes, pH = 10Yes, pH = 8C) Yes, pH = 5D) NoE) It is impossible to say because the titration curve is for a strong base.31. Choose an indicator from the table on p. 817 of your textbook that would be suitable to signal theequivalence point of titration (b).A) crystal violetB) bromphenol blueC) phenol redD) phenolphthaleinE) alizarin yellow R

More concentrated the base, the greater amount of acid will be required to neutralize it and reach…

Answer Questions #27 through #31 about the titration curves below (labeled a and b) for two different bases. The titrant acid used in both cases was 0.100 M HCI and the volume of the base solutions in both cases was 75.0 mL mL. 14 14 12- 12 - 10- 10 8- 8. 6. 6. 4- 4- 2- 0. 0 20 40 60 80 100 20 40 60 80 100 (a) Volume of acid added (mL) Volume of acid added (mL) (b) 2014 Peaon Education nc Hd Hd

Answer Questions #27 through #31 about the titration curves below (labeled a and b) for two different bases. The titrant acid used in both cases was 0.100 M HCI and the volume of the base solutions in both cases was 75.0 mL mL. 14 14 12- 12 - 10- 10 8- 8. 6. 6. 4- 4- 2- 0. 0 20 40 60 80 100 20 40 60 80 100 (a) Volume of acid added (mL) Volume of acid added (mL) (b) 2014 Peaon Education nc Hd Hd

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A 22.9 mL sample of a 0.390 M aqueous hydrofluoric acid solution is titrated with a 0.354 M aqueous

A: Solution: To calculate the pH of solution we need to check the pair of acid and base. From the…

Q: Which of the following aqueous solutions are good buffer systems? 0.11 M acetic acid + 0.15 M nitric…

Q: TITRATION First: 10 mL - unknown acid + 0.15 Phenolphthalein solution = 10.150 mL Next: 10.150 mL…

Q: 9. Figure 6 shows 4 titration curves of monoprotic strong acids titrated with 0.10 M NaOH. • As a…

Q: Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The Ka of hypobromous acid…

A: At equivalence point, Number of equivalents of acid =Number of equivalents of base The balanced…

Q: Payal

A: The objective of this question is to calculate the pH of a solution after a certain volume of base…

Q: temine the concentration of a NaOH(ag) solution, s student titreted a 50. ml. sample with 0.10…

Q: 4. Calculate the Al+3 ion concentration in Al(OH)3 if the [OH*] is 2.9 x 10-³ M 5. The solubility of…

Q: c. How does the number of moles of hydronium ions and hydroxide ions compare at the equivalence…

A: The question is based on the concept of titrations. we have to analyse the given titration curve and…

Q: Consider the titration of 300.0 mL of 0.450 M NH 3 ( K b = 1.8 × 10 –5) with 0.450 M HNO 3. How…

A: Given: Concentration of NH3 = 0.450 M Volume of NH3 solution = 300.0 mL And concentration of HNO3 =…

Q: Write the reaction that takes place when OHa) is added to a basic buffer solution containing…

A: Given: Buffer solution of HONH2 and HONH3+. And OH- is added in the solution.

Q: Ка 1.0 x 103 Acid Sulfuric Acid Sulfurous Acid Propionic Acid Ammonium 1.3 x 102 1.34 x 105 5.8 x…

Q: Using the table of indicators identify which of the given indicators would be appropriate for the…

A: From the Titration curve it has been seen that initially a fast drop in pH takes place but slows…

Q: What is the pH of the titration mixture when 30.00 mL of 0.085 M Hydrofluoric acid (HF; Ka = 6.8 x…

Q: Which of the following is the strongest base? The Ka's listed are for the conjugate acid of the base…

A: Since you have asked multiple question as per our company guidelines we are supposed to answer the…

Q: What is the pH at the equivalence point in the titration of a 22.4 mL sample of a 0.326 M aqueous…

A: Concentration of HF(M1) = 0.326 MConcentration of KOH(M2) = 0.484 MVolume of HF(V1) = 22.4 mL

Q: Hd 12 10 8 6 4 2 BA с D E + 0 2 4 6 8 10 12 14 16 18 20 22 24 26 28 30 mL base 6. In a different…

A: Answer: When acid is being titrated against base then neutralization reaction in the solution takes…

Q: The titrant in Graph A is v weak acid strong base strong acid weak base The titrant in Graph B is a…

Q: 6. It takes 14.5 mL of 0.475 M NaOH to reach the equivalence point of a titration with 10.0 mL of a…

Q: A possible titrant for graph B is NaOH + A possible sample solution for graph B ír H;0 HBr кон

A: I am supposed to solve the question for graph B

Q: Calculate the molar solubility and solubility product of Ca(OH)2 for each trial.

A: please find the answer attached here

Q: A 20.00 mL solution of a weak acid (0.05 M) weak acid was titrated with an aqueous solution of 0.01M…

A: Part A-Concentration of acetic acid= 0.05 MVolume of acetic acid = 20.00 mLConcentration of NaOH =…

Q: magnesium nitrate, Mg(NO,),(aq), solution

A: This question is related to precipitation.

Q: 48.1 mL sample of a 0.431 M aqueous hydrofluoric acid solution is titrated with a 0.345 M aqueous…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K₂ of hypobromous acid…

A: The question is based on the concept of pH of the solution. it is defined as a negative logarithm…

Q: A 52.0-mLmL volume of 0.35 MM CH3COOHCH3COOH (Ka=1.8×10−5Ka=1.8×10−5) is titrated with 0.40 MM…

Q: A technician mixes 0.10 L of 0.10 M NaCl with 0.30 L of 0.20 M AgNO3. Which of the following…

A: The total volume (VT) of the solution after mixing is 0.40 L. The concentration of NaCl, MNaCl, in…

Q: 1. Write the chemical reaction for the titration of the filtered KHT solution in pure water.…

A: Given chemical reaction is: KHC4H4O6 --------------> K+(aq) + HC4H4O6-(aq).

Q: titration between 20.0 mL of a weak base (Kb= 4.7*10-6) and 0.150 Mhydrochloric acid A.What is the…

Q: What is the concentration of H2SO4 (in mol/L) based on the data from their second titration? Report…

Q: A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is…

A: Answer: When base is gradually added in the acid solution then it neutralizes the acid and forms…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

28. Which of the two titrations has a base solution that is more concentrated?
A) (a)
B) (b)
C) Both (a) and (b) are the same concentration
D) It is impossible to say without knowing the exact Kp values of the two bases.
E) Titrating with HCl won't work. You need to use another acid in the titration.
29. Which titration has the stronger base (larger Kb value)? Be careful: Make sure you compare the Kp values of
the bases, not the Ka values of the conjugate acids. Also, don't forget the relationship between Kband pKb.
A) (a)
B) (b)
C) Both (a) and (b) are the same pKp.
D) It is impossible to say without knowing the exact Kb values of the two bases.
E) Titrating with HCl won't work. You need to use another acid in the titration.
30. Could the base titrated in (b) be used as part of a buffer? If so, what pH could be maintained by this buffer?
A) Yes, pH = 10
Yes, pH = 8
C) Yes, pH = 5
D) No
E) It is impossible to say because the titration curve is for a strong base.
31. Choose an indicator from the table on p. 817 of your textbook that would be suitable to signal the
equivalence point of titration (b).
A) crystal violet
B) bromphenol blue
C) phenol red
D) phenolphthalein
E) alizarin yellow R

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Question no 28

Question no 29

Question no 30

Question no 31

Step by step

Solved in 4 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

please answer all of them especially at 50 ml. Thank you. Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl . Calculate the pH of the resulting solution after the following volumes of have been added. 0.0 mL pH = 20.0 mL pH = 30.0 mL pH = 40.0 mL pH = 50.0 mL pH =
11
What are some steps needed to solve the following question? "A 6.90 g sample of sodium nitrite (NaNO2) was dissolved in about 100. mL of water. To this was added 500. mL of 0.200 M nitrous acid (HNO2) and the total volume was brought to 1.00 L by adding distilled water. To 100.0 mL of this resulting buffer solution was added 1.00 mL of 5.00 M HBr (aq). Find the pH." [H30*) = 10-PH McVc = MaVd %3D Henderson-Hasselbalch Equation g -> mol calculation mol -> g conversion
Precipitation Determine if a precipitate occurs when mixing o 40.0 mL 3.00 x 10-3 M BaCl2 • 50.0 mL 3.00 x 10-3 M Na2CO3 BaCl2 + Na2CO3 → 2NaCl + BaCO3 BaCO3 Ksp = 1.1 x 10-10 If so, what is the [Ba²+] after the precipitation?
A student performed titration to determine the concentration of potassium permanganate solution with oxalic acid. The net ionic equation is as follows: 2MnO4– + 16H+ + 5C2O42- → 2Mn2+ + 10CO2 + 8H2O The titration consumed 42.31 mL of 0.1001 M oxalate solution to reach the endpoint. Determine the concentration of permanganate (M) if 25 mL was used.
You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?
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: _______________
I titrate a 5.00mL aliquot of Arsenic acid with 36.09 mL 0.126M sodium hydroxide. Calculate the molarity of the arsenic acid sample.
Fill out the tables and find pH
You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?
Two 25.0-mL. samples of unknown monoprotic weak acids, A and B, are titrated with 0.100 M NAOH solutions. The titration curve for each acid is shown below ACID A ACID B 14 14 12 12 10 10 10 15 20 25 30 35 40 45 30 5 10 15 20 25 30 33 40 45 30 Vohume of NaOH added (ml) Volume of NaOH added (ml ) Part A Which of the two weak acid solutions is less concentrated? B A. Submit Bequest Answer
Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g