Natalia wish to sketch a weak acid-strong base titration curve. Before that, she needs to collect some data points. In a case scenario where 25 mL of 0.50 M CH3COOH (Ka = 1.80 x 10-5 ) was titrated with 0.10 M NaOH, deduce the pH after addition of different volumes of NaOH. (i) 0 mL NaOH

Natalia wish to sketch a weak acid-strong base titration curve. Before that, she needs to collect some data points. In a case scenario where 25 mL of 0.50 M CH3COOH (Ka = 1.80 x 10-5 ) was titrated with 0.10 M NaOH, deduce the pH after addition of different volumes of NaOH. (i) 0 mL NaOH

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 16.53QE

See similar textbooks

Related questions

Q: Construct a titration curve by reacting a 50.00mL aliquot of NaCN 0.0500M with the 0.100M HCl…

A: we need to calculate pH of the solution after addition of given amount of HCl to NaCN solution

Q: In titration of strong acids such as HCI with bases, which one of the following is not correct about…

A: Given the titration of a strong acid vs a base. Among the given statements, which one is not…

Q: A di-protic weak acid was titrated with NaOH. After ploting the titration profile and the first and…

Q: Generate a titration curve for the titration of 100 ml of 0.15M acetic acid with 0.30M NaOH. Show…

A: The balanced equation for the reaction of acetic acid, CH3COOH and NaOH is: CH3COOH(aq) + NaOH(aq)…

Q: 10.Calculate the pH of the solution prepared by dissolving 0.48 mol of NH3(Kb=1.77x10-5) and 0.750…

A: The given buffer solution is basic so first we calculate pOH and then pH of given solution.

Q: 5. A 100.0 mL aliquot of 0.100 M diprotic acid H2A (pK1 = 4.00, pK2 = 8.00) was titrated with 1.00 M…

A: Solution- Given-pK1 = 4.00 and pK2 = 8.00, 0.100 M diprotic acid, 1.00 M NaOH aliquot = 100.0ml

Q: mine the pH during the titration of 39.3 mL of 0.315 M trimethylamine ((CH3)3N, K = 6.3×10) by 0.315…

Q: 50.0 mL of 0.0500 M HCN (K3=4.9x10-10) is being titrated with 0.0500 M Ba(OH)2 . Please answer the…

A: Given, Molarity of HCN = 0.0500 M Volume = 50.0 mL Acid dissociation constant of HCN = Ka = 4.9 x…

Q: A 52.0-mL volume of 0.35 M CH3 COOH (Ka = 1.8 x 10-5) is titrated with 0.40 M NaOH. Calculate the pH…

A: The pH of a solution helps us to determine the acidity or alkalinity of a solution. A buffer is a…

Q: A 20.0-mL sample of a 0.125 M diprotic acid (H2A) solution is titrated with 0.1019 M KOH. The acid…

A: The neutralisation reaction taking place to reach first equivalence point is given by H2A + KOH…

Q: Select Weak Acid as the analyte in the titration interactive. Determine the pK, of this weak acid.…

A: A question based on equilibrium concept, which is to be accomplished.

Q: volume of NaOH (mL) Concentration of Weak Acid (M) pH Indicator endpoint Titration curve equivalence…

Q: Instrumental acid-base titrations use a pH meter to monitor the changes in pH and volume. The…

A: (a)

Q: In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one…

A: Given: Weak base = 0.0200 M Volume of weak base = 50.0 mL Concentration of base = 0.0150 M pKb of…

Q: c) Jack and Helen wish to sketch a weak acid strong base titration curve. Before they can do so,…

Q: Given the following experimental data, calculate the molarity and the pKa of the acid analyte (HA)…

A: Solution is given below in next step in jpeg format

Q: 1. What will be the remaining bromide ion concentration after addition of 20.00 mL AgNO₃? 2. At what…

Q: 5==== A strong acid and a monoprotic weak acid are separately potentiometrically itrated with a…

A: Potentiometric Titration is done via the usage of two electrodes – an indicator electrode and a…

Q: While preparing the samples for analysis, you forgot that you already added phenolphthalein…

A: 1. When the Phenopthalein indicator is added more it results in the acid compound into more acidic…

Q: Suppose 50.0 mL of a 0.100 M solution of the weak acid HA is titrated with a 0.100 M solution of…

Q: Calculate the pH at 0, 10, 90, 100, 110 (% of the equivalence point volume) for the titration of…

A: pH is used to determine the concentration of hydronium ion.

Q: Show all work and ICE tables. 60.00 mL of 1.000 M acetic acid, HC2H3O2, is titrated with 0.6500 M…

A: Answer :- pH = 9.17 The pH of a solution when 60.00 mL of 1.000 M acetic acid, HC2H3O2, is titrated…

Q: explain if this is true or false 1. in the potentiometric titration curve of salicylic acid, the…

A: Salicylic Acid have Both OH and COOH group connected ortho to Each other.

Q: 80.00 mL of 0.1000 M NaOH was be needed to reach the equivalence point in a titration with 25.00 mL…

A: Titration is a common laboratory method of quantitative analysis of the concentration of the…

Q: Calculate the equivalence point volumes for a titration of 25.00 mL of 0.060 M HCl and 01.0 M H3PO4…

A: HCl vs NaOH Volume of HCl ( Va ) =25.00 mL Molarity of HCl ( Ma ) = 0.060 M Molarity of NaOH ( Mb…

Q: 2. 20.0 mL of 0.1000 M Benzoic Acid (HC7H5O2) in a flask is being titrated with 0.1000 M NaOH…

A: Note: Since you have posted multiple independent questions in the same request, we will solve the…

Q: 25 mL of a mixture of NaOH and Na 2 CO 3 was titrated with 0.1 HCI using enolphthalein indicator…

A: This question belongs to the titration of a mixture of the strong and weak base against strong acid…

Q: 3) Consider the titration of 40.0 mL of 0.100 M maleic acid (HzM) with 0.200 M NaOH. Maleic acid is…

A: Given: Volume of maleic acid i.e. H2M = 40.0 mL = 0.040 L (Since 1 L =…

Q: The pH at one-half the equivalence point in an acid-base titration was found to be 5.67. What is the…

A: Given pH = 5.67 Ka = ?

Q: What is the pH at the equivalence point

Q: A series of solutions containing NaOH, Na2CO3, and NaHCO3, alone or in compatible combination, was…

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

Q: A chemist generates the titration curve shown by slowly 12 adding 1.0 M sodium hydroxide (NaOH) to…

A: Titration curve is the graph in which volume of titrant plotted against pH.

Q: Sketch the titration curve that will be obtained when 50 mL of 0.05 M glycine at pH 1.5 is titrated…

A: Equivalence point: It is a point in titration at which the amount of titrant added is just enough to…

Q: m doing a lab for chemistry and need help answering numers 1 and 2 below using the data provided.…

A: Molarity Of NaOH = 0.1 M For your coarse titration, record the following results. initial…

Q: 10-13. Describe how you would prepare exactly 100 mL of 0.100 M picolinate buffer, pH 5.50. Possible…

A: Step 1 : Dissolve 10.0mmole (1.23g ) picolinic acid in 75ml water in a beaker. Step 2. Then add…

Q: 25.00 mL of 0.1000 M NH3 is titrated with 0.1000 M HCI. The K₁ of NH3 is 1.75 × 10¹5. Calculate pH…

Q: Complete the following table and answer the questions, showing all of your calculations. Trial…

Q: (2) A student titrates 25.00 ml of 0.200 M acetic acid (Ka = 1.8 x 10) with 0.200 M NaOH. Calculate…

A: Balanced equation for the reaction of NaOH and acetic acid(AcH) is: AcH(aq) + NaOH(aq) ---->…

Q: The titration of a polyprotic acid with sufficiently different pKa ’s displays two equivalence…

A: Polyprotic acid produces two different H+ ions upon ionization like diprotic acid.

Q: What would be an appropriate indicator to use to measure the endpoint volume for a titration with a…

A: While choosing an indicator for acid-base titrations, an indicator whose pH range falls within the…

Q: Derive a curve for the titration of 50.00 ml 0.1000 M solution of compound A with a 0.2000 M…

A: Answer - According to the question - Given - Calculate the pH after the addition of the following…

Q: sample of 100.00mL of 0.100 M HC2H3O2 is titrated with 0.100 M NaOH. Find the pH of the solution…

Q: In the titration of 50.0 mL of 1.0 M methylamine, CH,NH, (K, = 4.4 × 10-4), with 0.50 M HCI,…

Q: A 25.00-mL aliquot of 0.1000 M maleic acid was titrated with 0.1000 M NaOH. The pH values at the…

A: For maleic acid, pKa1 = 1.9, and pKa2 = 6.07

Q: What is the pH at 35.00 mL of titrant in the titration of 60.00 mL of 0.200 M HA (a generic acid…

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

Q: Stårting with 0.750L of a buffer solution containing 0.35 M benzoic acid (CH5COOH) and 0.30 M sodium…

A: Concentration of HCl added in the solution = Moles of HCl/Volume = 0.12mol/0.750L = 0.16M From the…

Q: What is the pH at 90.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with…

A: pH is the negative logarithm of hydrogen ion concentration. Given data: *Volume of base is 50.0 mL…

Q: When titrating 25 mL of an approximately 0.1 M solution of a triprotic acid solution with 0.1052 M…

A: Let the triprotic acid be H3A. The balanced equation for the neutralization is: H3A + 3NaOH(aq)…

Q: What is the pH in titration of 100 ml 0.01 M benzoic acid with 0.02 M NaOH at equivalence point?

A: Volume of benzoic acid is 100ml and molarity = 0.01 M NaoH molarity = 0.02M Calculate the PH 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

Natalia wish to sketch a weak acid-strong base titration curve. Before that, she needs to
collect some data points. In a case scenario where 25 mL of 0.50 M CH3COOH (Ka = 1.80
x 10-5
) was titrated with 0.10 M NaOH, deduce the pH after addition of different volumes
of NaOH.
(i) 0 mL NaOH
(ii) 100 mL NaOH
(iii) 125 mL NaOH

Definition Definition Method of quantitative analysis for determining the concentration of an acid or base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 3 images

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

Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Above is the titration curve of a weak acid (200 mM acetic acid) and strong acid (0.1 M sodium hydroxide). How would you prepare a 50 mL of the 200 mM acetic acid solution from a concentrated reagent grade acetic acid if pKa of acetic acid is 4.75, acetic acid glacial concentration is 99.8%, density of acetic acid is 1.05g/cm3, molecular weight is 60.05g/mol
The dissociation constants for citric acid are 7.4E-4, 1.7E-5 and 4.0E-7. How many useable end points will occur in an acid/base titration involving it?
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base:(a) 0 mL(b) 25.00 mL(c) 39.00 mL(d) 39.90 mL(e) 40.00 mL(f ) 40.10 mL(g) 50.00 mL Use the values obtained to sketch a curveof [H₃O⁺] vs. mL of added titrant. Are there advantages or dis-advantages to viewing the results in this form? Explain.
When titrating 25 mL of an approximately 0.1 M solution of a triprotic acid solution with 0.1052 M NaOH, a student calculates that the end point will be reached after the addition of approximately x mL of NaOH. However, after the addition of 2x mL of sodium hydroxide, no colour change is observed. Which of the following errors could not account for this obervation? using a 3 mole acid : 1 mole base ratio in the calculation washing the sides of the flask with DI water during the titration and diluting the analyte solution mistakenly using a 0.01000 M NaOH solution in the titration failing to add an indicator to the analyte solution mistakenly using a primary standard solution of > 1.0 M in the titration
The titration of a polyprotic acid with sufficiently different pKa ’s displays two equivalence points. Why?
Generate a titration curve for the titration of 100 ml of 0.15M acetic acid with 0.30M NaOH. Show the pre, the equivalence, and post equivalence. Use an interval of 10mL addition of titrant.
When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5 1) Calculate the pH at this point 2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?
A student is preparing to titrate 25.00 mL of 0.2 M NaOH. He has options to use among 3 weak monoprotic acid at same concentration, with different acid dissociation constants, WA1= 1 X 10-4, WA2= 1 X 10-5 , WA3= 1 X 10-8. Which is the best acid titrant you would recommend ?
Consider the titration of 20 mL of 0.10 M base with 0.20 M HCl. The analyte is dibasic withpKb1 = 5.00 and pKb2 = 10.00. Calculate the pH at the following volumes of HCl0 mL, 5 mL, 10 mL, 15 mL, 20 mL
Construct the titration curve for the titration of 26.0 mL of 0.100 M KOH with 0.0600 M HNO3
Calculate the equivalence point volumes for a titration of 25.00 mL of 0.060 M HCl and 01.0 M H3PO4 with 0.075M NaOH. There will be two of them.