Answered: Describe the pH changes that occur…

Describe the pH changes that occur during the titration of a weak base by a strong acid. What is meant by the term equivalence point?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 108QRT

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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Describe the pH changes that occur during the titration of a weak base by a strong acid. What is meant by the term equivalence point?

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You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.
Equimolar quantities of potassium fluoride and hydrofluoric acid are placed into solution. What happens to the buffer system if some hydrochloric acid is added to the solution? The hydrochloric acid reacts with the fluoride ions so the pH decreases only slightly. The hydrochloric acid reacts with the fluoride ions so the pH decreases significantly. ) The hydrochloric acid reacts with the hydrofluoric acid so the pH increases only slightly. The hydrochloric acid reacts with the hydrofluoric acid so the pH increases significantly.
You are studying a clear solution and you added the pH indicator methyl violet. The colour range of the indicator methyl violet in a clear solution when changing from acidic to basic is yellow (pH 0) to blue purple (pH 1) to violet (pH 2). You initial pH of the solution when tested with a pH meter is O.2. You are going to add 250 drops of 0.1 M HCI. Please select the most appropriate answers to the following two questions. What is the initial colour of the solution at pH 0.2? What is the colour of the solution and what will the pH be after the addition of the HCI? Select 2 correct answer(s) The colour of the solution after the addition of HCI will be clear and the pH will be less than 0.2. The colour of the solution after the addition of HCI will be violet and the pH will be higher than 0.2.
A series of carbonic acid or carbonate buffers regulate pH in blood within the human body. The kidneys and the lungs work together to help maintain a blood pH of 7.4 by affecting the components of the buffers in the blood. What conjugate acid/base pair is the main component in the buffer? Write out the chemical reaction that the conjugate pair undergoes in water. What is the ratio of the acid to the base? What is the ideal pH range for this buffer? Is the pH of blood within the ideal range of the buffer? If it is not, what is the physiological reason that the body would have for still using a carbonate buffer as opposed to another conjugate pair?
Select the statements that describe a method which can be used to make a buffer. Add appropriate quantities of weak acid and its conjugate base to water. Partially neutralize a strong base solution by addition of a strong acid. Partially neutralize a strong acid solution by addition of a strong base. Partially neutralize a weak base solution by addition of a strong acid. Partially neutralize a weak acid solution by addition of a strong base.
Consider the buffer system of carbonic acid (H₂CO₂) and its salt, KHCO₂, which provides the conjugate base, HCO,. H_COjlog) + HJO W 7 HyO" loạ) + HCOy loa) How does the buffer react when some base is added? The bicarbonate ion (HCO) of the buffer reacts with the base. OHCO and H₂CO, both react with the base. O The buffer does not react. O The carbonic acid (H₂CO₂) of the buffer reacts with the base Question 15 Indicate whether each of the following reactions is an example of reaction of an acid with a metal, reaction of an acid with a carbonate, or acid-base neutralization reaction using the dropdown on the right. Reaction A: ZnCO3(s) + 2HBr(aq) → ZnBr₂(aq) + CO₂(g) + H₂O(l) Reaction B: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) HCI(g) + NaHCO3(s)→ NaCl(aq) + CO₂(g) + H₂O(0) H₂SO4(aq) + Mg(OH)2(s)→ MgSO4(aq) + 2H₂O(1) 3LIOH(aq) + H₂PO₂(aq) → Li₂PO₂(aq) + 3H₂O(0) Cal(s) + H₂SO4(aq) → H₂(g) + CaSO₂(aq) Reaction C: Reaction D: Reaction E: Reaction E
Here is ph of the molarity of butyl chloride (C,H,CI) in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the table below. у 0.030- 0.0247 olo 0.020- Ar M 0.015- 0.010- 0.005- 500 1000 1500 2000 2500 3000 seconds created x10 Is C,H,Cl being created or destroyed by the chemical destroyed reaction? neither created nor destroyed If C,H,Cl is being created or destroyed, what is the rate at which it is being created or destroyed 1200 seconds after the reaction starts? Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
You have a 16 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 7.66. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 5.52. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 16 mL sample. Acetylcholine CH₂ acetycholine in original sample: CH,—C−O−CH,—CH,AN-CH, HO–CH,—CH,*N–CH, + CHy H₂O I CH3 CH3 Choline CH₂ CH,-GO + H Acetate nmol
7. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant of ammonia, NH3, is 1.815x10-5 A student worker is asked to prepare a buffer solution with NH3 and ammonium salt. However, after the student did a thorough search, no ammonium salt is found. After the student reported the result to the professor, the professor told the student the buffer can be prepared with ammonia and a strong acid. Can you help this student out? The pH of the buffer to be prepared is 10.08. The molarity of the ammonia in the buffer is 0.4717 M. The molarity of the ammonia solution found in the laboratory is 1.201 M, the strong acid solution is 0.9948 M HNO3. The volume of the buffer solution to be prepared is 500.0 mL. Please answer the following questions. A. B. What is the molarity of the ammonium ion in the buffer? Please provider your answer below. Check answer How many mL of 0.9948 M HNO3 solution is needed? Please provider your answer below. 0² 0₂ $…
1) Write the equilibrium constant expression for the dissociation of acetic acid 2) Vinegar sold commercially is typically 0.8−1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00 M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures? 3) What is the value of the equilibrium constant Keq for the dissociation according to the concentrations from number 2?
A 29.6 mL sample of 0.271 M dimethylamine, (CH3)2NH, is titrated with 0.237 M hydrobromic acid. After adding 12.9 mL of hydrobromic acid, the pH is Use the Tables link in the References for any equilibrium constants that are required.
You have a 18 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 8.35. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 6.03. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 18 mL sample.

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