Use the References to access important values if needed for this question.A 30.0 mL sample of 0.316 M diethylamine, (C₂H5)2NH, is titrated with 0.245 M hydroiodic acid.At the titration midpoint, the pH isUse the Tables link in the References for any equilibrium constants that are required.Submit AnswerRetry Entire Group 8 more group attempts remainingPreviousEmail InstructorNexSav

we have to calculate the value of pH

Answered: A 30.0 mL sample of 0.316 M…

A 30.0 mL sample of 0.316 M diethylamine, (C₂H5)2NH, is titrated with 0.245 M hydroiodic acid. At the titration midpoint, the pH is

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 16.58QE

See similar textbooks

Related questions

Q: A 28.4 mL sample of 0.379 M trimethylamine, (CH3)3N, is titrated with 0.318 M hydrobromic acid. At…

Q: A 20.6 mL sample of 0.377 M methylamine, CH3NH2, is titrated with 0.364 M perchloric acid. After…

A: Number of moles of CH3NH2= M*V = 0.377 M* 20.6 mL = 7.7662 mmol Number of moles of HClO4 = M*V =…

Q: A 29.8 mL sample of 0.247 M triethylamine, (C2H5)3N, is titrated with 0.396 M hydroiodic acid.…

Q: Methyl red has a pk, of 5.0 and is red in its acid form and yellow in its basic form. If several…

Q: A 29.1 mL sample of 0.263 M trimethylamine, (CH3)3N, is titrated with 0.281 M hydrobromic acid.…

Q: A 1.46 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with…

A: Titration is a volumetric analysis where the unknown concentration of the compounds is carried out…

Q: What are the molar concentrations of acetic acid (CH,COOH) and sodium acetate (CH, COONA) in an…

Q: What is the pH after the addition of 0.010 mol HCl to a 500.0 mL of a buffer solution that is 0.125M…

A: Buffer is a type of solution pH of which does not change significantly after addition of base or…

Q: 29.3 mL sample of 0.365 M dimethylamine, (CH3)2NH, is titrated with 0.362 M hydrochloric acid. At…

Q: A 50.0 mL sample of 0.350 M HBr is titrated with 0.200 M KOH. What is the pH when 50.0 mL of KOH has…

Q: Determine the pH of a buffer solution that is a mixture containing 0.10M acetic acid and 0.050 M…

Q: In the titration of 60.0 mL of 1.0 M methylamine, CH3NH₂ (Kb = 4.4 x 10-4), with 0.50 M HCI,…

A: Note: Since you have posted a question with multiple sub parts, we will provide the solution only to…

Q: A 27.6 mL sample of 0.275 M methylamine, CH3NH2, is titrated with 0.275 M hydroiodic acid. After…

A: This question can be solved using Henderson-Hesselbech equation as:

Q: In the titration of 50.0 mL 0.0200 M HCl using 0.0150 M NaOH, what is the solution pH after 100 mL…

A: The titration reaction taking place can be written as, => HCl + NaOH -------> NaCl + H2O Given…

Q: A buffer solution contains 0.202 M of a weak acid and 0.224 M of its conjugate base. The K, of the…

A: Buffer solution is a solution whose pH does not changes on standing as well as on addition of small…

Q: Which of the following solutions will have the greatest buffer capacity? 1) 0.0100 M CH3COOH and…

Q: A 29.8 mL sample of 0.252 M dimethylamine, (CH3)2NH, is titrated with 0.242 M hydrochloric acid. At…

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

Q: A 0.804 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with…

A: Given data :

Q: 2) For the titration 100 mL of 0.1 M NH3 with 0.2 M HCI, what will be the pH of the solution after…

A: Solution : pH pH is a quantitative measure for the acidity or basicity of the solution. This…

Q: Determine the pH during the titration of 13.8 mL of 0.191 M nitric acid by 8.64×10² M sodium…

A: (1) pH = 0.7190(2) pH = 1.3453(3) pH = 7.00(4) pH = 12.0868Explanation:This problem is a case of the…

Q: A 28.8 mL sample of 0.304 M dimethylamine, (CH3)2NH, is titrated with 0.378 M hydrobromic acid. At…

Q: A chemist wishes to prepare 121.00 mL of acetic acid/sodium acetate buffer solution with a pH of…

A: Given, A chemist wishes to prepare 121.00 mL of acetic acid/sodium acetate buffer solution with a…

Q: A 0.0415 L volume of 0.11 M hypochlorous acid (HCIO), a weak acid with K₂ = 4.0x108, is titrated…

A: Given,molarity of HClO = 0.11 MVolume of HClO = 0.0415 LKa of HClO = 4.0 x 10-8Molarity of KOH =…

Q: A 26.2 mL sample of 0.253 M trimethylamine, (CH3)3N, is titrated with 0.306 M hydroiodic acid. At…

A: Given data : 1. 26.2 mL sample of 0.253 M trimethylamine, (CH3)3N 2 . 0.306 M hydroiodic acid. To…

Q: Express the solubility equilibrium of the generally insoluble salt CuOH.

A: Solubility equilibrium is the equilibrium associated with the dissolving solid in water to form…

Q: A 23.1 mL sample of 0.205 M methylamine, CH3NH2, is titrated with 0.341 M nitric acid. At the…

A: Given: The volume of 0.205 M methylamine is 23.1 mL. The molarity of nitric acid is 0.341 M.

Q: A 25.5 mL sample of 0.362 M triethylamine, (C2H5)3N, is titrated with 0.285 M hydroiodic acid.…

A: Given data,Molarity of triethylamine=0.362MVolume of triethylamine=25.5mL=0.0255LMolarity of…

Q: A chemistry graduate student is given 300. ml of a 0.90M dimethylamine ((CH) NH) solution.…

A: Henderson-Hasselbalch equation The equation which is used to find the pH of a buffer system is…

Q: An analytical chemist is titrating 152.0 mL of a 0.2100 M solution of benzoic acid (HCH,CO,) with a…

A: The reaction of benzoic acid with sodium hydroxide will produce an acidic buffer solution. In the…

Q: A 21.4 mL sample of 0.260 M dimethylamine, (CH3)2NH, is titrated with 0.232 M hydrochloric acid.…

A: Given,Molarity of dimethyl amine ( (CH3)2NH ) = 0.260 MVolume of (CH3)2NH = 21.4 mLMolarity of…

Q: A buffer solution contains 0.77 mol of hydrosulfuric acid (H2S) and 0.43 mol of sodium hydrogen…

A: Here the reaction is, H2S(aq) + H2O(l) ⇌HS- (aq) + H3O+(aq) Here, Ka= 9.5×10-8 From Henderson…

Q: A 21.0 mL sample of 0.308 M methylamine, CH3NH2, is titrated with 0.245 M hydrobromic acid. At the…

A: The question is based on the concept of titrations. we have been given a weak base and a strong…

Q: A 29.5 mL sample of 0.258 M ethylamine, C2H5NH2, is titrated with 0.340 M hydrochloric acid. After…

A: Given- Volume of ethylamine=29.5mL Concentration of ethylamine =0.258M Volume of hydrochloric acid=…

Q: A 26.9 mL sample of 0.375 M diethylamine, (C2H5)2NH, is titrated with 0.258 M Hydrochloric acid.…

A: Given : Concentration of (C2H5)2NH = 0.375 M Volume of (C2H5)2NH solution = 26.9 mL = 0.0269 L…

Q: How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the…

A: a) Moles of base = Molarity * Volume (L) = 0.1M * 0.025 L = 0.0025 mol At equivalence point- Moles…

Q: Calculate pH for a weak base/strong acid titration. Determine the pH during the titration of 35.9 mL…

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

Q: Describe the pH changes that occur during the titration of a weak base by a strong acid. What is…

A: A reaction between a base and an acid to give water and salt as products is known as the…

Q: 12.0 g of sodium acetate is added to 125 mL of a 0.83 M acetic acid solution. What is the pH of this…

A: pH of buffer solution is calculated by using Henderson Hassel balch equation

Q: Consider the titration of 25.00mL of 0.200M Methylene (CH3NH2). The titrant is 0.120M HCL.…

A: The detailed solution is given below.Explanation:Step 1:Step 2: Step 3: Step 4:

Q: A 24.7 mL sample of 0.343 M dimethylamine, (CH3)2NH, is titrated with 0.219 M hydrobromic acid.…

A: we have to calculate the pH of the solution

Q: Calculate the molar solubility of Ni(OH)2 when buffered at pH 14.0

A: The solubility product of salt is a constant at a given temperature irrespective of the source from…

Q: A 28.9 mL sample of 0.290 M triethylamine, (C₂H5)3N, is titrated with 0.347 M perchloric acid. At…

Q: Calculate the minimum pH needed to precipitate Mn(OH)2 so completely that the concentration of Mn2+…

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

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

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 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

A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
Sulfanilic acid (NH2C6H4SO3H) is used in manufacturing dyes. It ionizes in water according to the equilibrium equation NH2C6H4SO3H(aq)+H2O(l)NH2C6H4SO3(aq)+H3O+(aq)Ka=5.9104 A buffer is prepared by dissolving 0.20 mol of sulfanilicacid and 0.13 mol of sodium sulfanilate (NaNH2C6H4SO3) in water and diluting to 1.00 L. Compute the pH of the solution. Suppose 0.040 mol of HCl is added to the buffer.Calculate the pH of the solution that results.
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
When a diprotic acid. H2A. is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If die pH at 50.0 mL NaOH added is 4.0 and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka and Ka. for the diprotic acid. d.