3. Propanoic acid (abbreviated as HPro; Ka = 1.3 x 10-5) is produced naturally by a bacterium that is also responsible for forming the holes in Swiss cheese. An extract of 45.0 mL of HPro from some cheese had a propanoic acid molarity of 0.0150 M. This was titrated with 0.034 M NaOH. The entire titration would require 20.0 mL of NaOH. (A) The initial pH of the propanoic acid solution is 3.355. What is the pH of the solution at the halfway point in the titration? (B) What is the pH after 18.0 mL of the NaOH solution has been added? (C) What is the pH at the equivalence point? (D) Based on your results from part "D", which of the following indicators would be the best one to select to show the end point of this titration? (Just circle your choice, no calculation required) (i) Cresol Purple: Transition range 1.2 - 2.8 (ii) Cresol Red: Transition range 7.2 -8.8 (iii) Alizarin Yellow: Transition range 10.1 - 12.0

3. Propanoic acid (abbreviated as HPro; Ka = 1.3 x 10-5) is produced naturally by a bacterium that is also responsible for forming the holes in Swiss cheese. An extract of 45.0 mL of HPro from some cheese had a propanoic acid molarity of 0.0150 M. This was titrated with 0.034 M NaOH. The entire titration would require 20.0 mL of NaOH. (A) The initial pH of the propanoic acid solution is 3.355. What is the pH of the solution at the halfway point in the titration? (B) What is the pH after 18.0 mL of the NaOH solution has been added? (C) What is the pH at the equivalence point? (D) Based on your results from part "D", which of the following indicators would be the best one to select to show the end point of this titration? (Just circle your choice, no calculation required) (i) Cresol Purple: Transition range 1.2 - 2.8 (ii) Cresol Red: Transition range 7.2 -8.8 (iii) Alizarin Yellow: Transition range 10.1 - 12.0

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: b. CH3CH2OH + NaOH --> CH3CH2O - + NaOH2 + c. CH3COOH + NaOH --> CH3COONa + H2O d.…

A: We have to find out correct reaction between acetic acid and sodium hydroxide solution

Q: An aqueous solution of Ca(OH)2with a concentration of 0.146 M was used to titrate 25.00 mL of…

A: Answer:- This question is answered by using the simple concept of chemical reaction between acid and…

Q: To determine the concentration of citric acid, you will need to titrate this solution with 0.100 M…

A: Relation between molarity, volume for reaction between two solutions- M1V1=M2V2 Where,…

Q: 30 mL of an unknown concentration of phosphoric acid (triprotic) was titrated with 10 mL 0.05 M…

A: We have to predict the concentration of the acid

Q: A mass of 0.640 g of an unknown monoprotic acid, HA, was titrated with KOH. Given that the acid…

A: The molar mass of the monoprotic acid HA will be 151 g/mol (after rounding off).

Q: The flask contains 10.0 mL of HCl and a few drops of indicator. The buret contains phenolphthalein…

Q: 4. If some of the calcium metal remains unreacted when you start the titration, the calcium will…

A: During the titration, you're trying to determine the amount of acid needed to neutralize the calcium…

Q: Lactic acid is a monoprotic acid with the formula C3H6O3. You have a 25.00 mL sample of lactic acid…

A: The concentration of acids is determined by a neutralization reaction with a base of known…

Q: A student titrates a weak acid with 0.100 M NaOH, adding 31.65 mL before a dark pink color is seen.…

A: The mole of H+ ion the weak acid is equal to the mole of NaOH used in the titration. The molarity…

Q: the molarity of the NaOH solution used

Q: 3NaOH(aq) + FeCl3 3NaCl(aq) + Fe(OH)3(s) A. Calculate the volume of 0.200M FeCl3 solution needed to…

A: The balanced reaction taking place is given as, => 3 NaOH (aq) + FeCl3 (aq) ------> 3 NaCl…

Q: Suppose 0.347 grams of a solid monoprotic acid are titrated with 14.82 mL of 0.117 M NaOH. What is…

A: The monoprotic acid reacts with sodium hydroxide as follows: HA + NaOH → NaA + H2O The…

Q: A student evaluated a gel antacid. The student dissolved 3.0 mL in 25.00 mL of a standardized HCl…

A: Neutralization finds its use in calculating the potential of one compound exist i.e. analyte in a…

Q: A solution of HCl is prepared for titration of unknown Na2CO3 samples, by standardization with pure…

A: Mass of Na2CO3 = 0.4453 g Molar mass of Na2CO3 = 105.99 g/mole Mole of Na2CO3 =…

Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…

A: We have to write the balanced equation for the reaction and calculate :- moles of HNO₃ moles of…

Q: A student titrates a weak acid with 0.100 M NaOH, adding 34.84 mL before a dark pink color is seen.…

A: Calculation of no. of mol of NaOH: No. of mol=Molarity×Volume=0.100 mol/L×34.84×10-3 L=3.484 ×10-3…

Q: student is asked to standardize a solution of barium hydroxide. He weighs out 0.952 g potassium…

A: Given that: Mass of potassium hydrogen phthalate(KHP) = 0.952g Molar mass of KHP = 204.2 g/mol…

Q: 25.00 mL of a solution containing 25.7 g/L of an unknown acid is titrated with 0.114 M NaOH. It…

Q: A 25.00 ml solution of acetic acid of unknown concentration is titrated with 0.1000 M KOH. The end…

Q: You have a solution of NaOH of unknown concentration. A 15.98 mL sample of the NaOH solution was…

A: Concentration of NaOH = To be determined Volume of NaOH = 15.98 mLMolarity of HNO3 = 0.377 MVolume…

Q: n the titration of 10.00 mL sample of vinegar solution with 0.35 M NaOH as titrant, the initial…

A: The question is based on the quantitative analysis. we have to calculate percentage acid present in…

Q: A 0.1240 M NaOH(aq) solution was used to titrate 20.00 mL of an acetic acid (CH3COOH) solution that…

A: Recall the following relation MNaOH×VNaOH=MCH3COOHVCH3COOHGiven that,concentration of…

Q: An analytical chemist weighs out 0.066 g of an unknown monoprotic acid into a 250 mL volumetric…

A: Given:-analytical chemist weighs = 0.066 gMolarity = 0.1700MV = 8.4 mLCalculate molar mass of the…

Q: A solution of H2C2O4 is used to titrate a 18.42 mL sample of a 0.2079 M KOH solution. If the…

A: The given data contains, Volume of H2C2O4 = 13.51 ml. Volume of KOH = 18.42 ml. Molarity of KOH =…

Q: 50.00 mL of an acetic acid solution is titrated with 0.1000 M NaOH. 23.90 mL NaOH is required to…

A: Given : Volume of acetic acid = 50 ml Volume of NaOH = 23.90 ml Molarity of NaOH = 0.1000M

Q: The titration of 25.0 mL of an unknown concentration H 2SO 4 solution requires 83.6 mL of 0.12 M…

A: Given Volume of H2SO4 ( V1 ) = 25 mL Volume of NaOH ( V2 ) = 83.6 mL Molarity of NaOH ( M2…

Q: 5. The concentration of an unknown sample of sulfuric acid was determined by the method used in this…

A: The question is based on the concept of molarity.molarity is a method of expressing concentration of…

Concept explainers

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

3. Propanoic acid (abbreviated as HPro; Ka = 1.3 x 10-5) is produced naturally by a bacterium
that is also responsible for forming the holes in Swiss cheese. An extract of 45.0 mL of HPro
from some cheese had a propanoic acid molarity of 0.0150 M. This was titrated with 0.034 M
NaOH. The entire titration would require 20.0 mL of NaOH.
(A) The initial pH of the propanoic acid solution is 3.355. What is the pH of the solution at
the halfway point in the titration?
(B) What is the pH after 18.0 mL of the NaOH solution has been added?
(C) What is the pH at the equivalence point?
(D) Based on your results from part "D", which of the following indicators would be the best one
to select to show the end point of this titration? (Just circle your choice, no calculation required)
(i) Cresol Purple: Transition range 1.2 - 2.8
(ii) Cresol Red: Transition range 7.2 -8.8
(iii) Alizarin Yellow: Transition range 10.1 - 12.0

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

A technician would like to standardize an unknown Ca(OH)2 solution. It takes 22.41 mL of a 0.155 M solution of HCl to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution. Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2.
A student is asked to standardize a solution of calcium hydroxide. He weighs out 0.952 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid).It requires 35.7 mL of calcium hydroxide to reach the endpoint.A. What is the molarity of the calcium hydroxide solution? This calcium hydroxide solution is then used to titrate an unknown solution of nitric acid.B. If 15.6 mL of the calcium hydroxide solution is required to neutralize 29.1 mL of nitric acid, what is the molarity of the nitric acid solution?
You are running an acid-base titration with hydrochloric acid and calcium hydroxide. The calcium hydroxide is your titrant; it has a known concentration of 0.0891 M. You have added 25.0 mL of the hydrochloric acid solution to an Erlenmeyer flask along with 2 drops of phenolphthalein (fee’-nol-thay-leen) indicator. To begin your first trial, you fill a clean 50 mL buret with the calcium hydroxide solution. Your starting volume is 0.25 mL. After the addition of solution from the buret, you see a color change in the flask, and the end point of the reaction is reached. You note the final volume in the buret to be 18.75 mL. You begin again for your second titration trial. You add 24.8 mL of the hydrochloric acid solution to a clean flask along with 2 drops of indicator. You refill the buret to an initial volume of 1.42 mL. When the reaction is complete, you note the final volume in the buret at 16.74 mL. Then you complete a third trial. You add 25.6 mL of hydrochloric acid solution…
A sample weighing 10.91 g containing an unknown amount of H3PO4 was diluted with water and titrated with a standardized concentration of 0.7255 M NaOH. The endpoint was reached after 27.03 mL of the titrant was added. What is the % H3PO4 (97.994 g/mole) in the sample? H3PO4 + 2 NaOH --> Na2HPO4 + 2H2O ROUND OFF FINAL ANSWER TO FOUR (4) SIG FIGS
A titration was done using 32.83mL of a weak acid and 0.141 M NaOH. If 32.81 mL of the NaOH was required to reach the equivalence point, what was the initial concentration of the weak acid?
O SIMPLE REACTIONS Determining the molar mass of an acid by titration Jacque An analytical chemist weighs out 0.279 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1400M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 33.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. mol fo Exnation Check |Privecy 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use MacBook Air
5. What volume of 0.550 M NaOH do you need to titrate 40.0 mL of 0.260 M H&PO4. R-0
25.0-mL samples "A" and "B" (both containing HCl) were titrated with 0.100 M NaOH. When titrating sample "A", it took 23.8 mL of titrant to reach the endpoint. When titrating sample "B", it also took 23.8 mL of titrant to reach the endpoint. Which of the following is correct? a. Sample A has a higher concentration of HCl b. Sample B has a higher concentration of HCl c. Sample A has the same concentration as Sample B d. We are unable to deduce the concentration of either sample.
A student is asked to standardize a solution of sodium hydroxide. He weighs out 1.09 g potassium hydrogen phthalate (KHC8H404, treat this as a monoprotic acid). It requires 33.5 mL of sodium hydroxide to reach the endpoint. Use the References to access important values if needed for this question. A. What is the molarity of the sodium hydroxide solution? This sodium hydroxide solution is then used to titrate an unknown solution of nitric acid. Submit Answer M B. If 18.7 mL of the sodium hydroxide solution is required to neutralize 10.3 mL of nitric acid, what is the molarity of the nitric acid solution? 2 question attempts remaining M
help
Potassium hydrogen phthalate (KHPKHP) is often used as a primary standard in acid–base titrations. If 20.05 mL NaOH20.05 mL NaOH is required to neutralize 0.397 g KHP,0.397 g KHP, what is the concentration of the NaOH?