What is the difference between the endpoint of a titration and the equivalence point? The endpoint is dictated by the indicator. The equivalence point is when the amount in moles of base added is equal to the amount of moles in the acid sample. The endpoint is often observed after the equivalence point. The equivalence point is dictated by the indicator. The end point is when the amount in moles of base added is equal to the amount of moles in the acid sample. B. There is no difference between the endpoint and the equivalence point. Both are determined by the color change in a titration.

What is the difference between the endpoint of a titration and the equivalence point? The endpoint is dictated by the indicator. The equivalence point is when the amount in moles of base added is equal to the amount of moles in the acid sample. The endpoint is often observed after the equivalence point. The equivalence point is dictated by the indicator. The end point is when the amount in moles of base added is equal to the amount of moles in the acid sample. B. There is no difference between the endpoint and the equivalence point. Both are determined by the color change in a titration.

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...

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In an acid-base titration experiment, the equivalence point on the titration curve was at a pH of 6.0. Based on this information, which of the following is represents the titration experiment that was conducted? It was a titration conducted between a strong base and strong acid It was a titration conducted between a weak acid and a strong base. It was a titration conducted between a strong acid and a weak base
Determine the pH during the titration of 20.0 mL of 0.110 M perchloric acid by 7.69x10-2 M barium hydroxide at the following points: (1) Before the addition of any barium hydroxide (2) After the addition of 7.15 mL of barium hydroxide (3) At the equivalence point (4) After adding 18.3 mL of barium hydroxide
Methyl Orange and phenolpthalein are common chemical indicators often used in titrations. What is the role of a chemical indicator? A substance added to a reaction that provides the proper environment for the reaction to move forward. A substance consumed in a reaction that changes the rate of the reaction. A substance that gives a visible sign, usually a color change, when a specific reaction condition is reached. A chemical indicator is necessary for the neutralization reaction between a strong acid and strong base to go to completion.
Regarding titrations, which of the following is TRUE? A plot of pH vs. the [base]/[acid] ratio is known as a titration curve. The equivalence point is when the moles of base equals the moles of acid during any acid–base titration. Indicators do not respond to changes in pH. The pH is always 7 once the equivalence volume has been delivered. None of the answers are true.
A titration is performed with KOH and HCl. 0.0100 M HCl is used to titrate a 60.0 ml sample of a 0.0075M solution of KOH. What is the initial pH of the 60.0ml sample of KOH before any HCl is added? What is the pH after 20.0ml of the acid is added? What is the pH at the equivalence point? At the equivalence point, if all of the water is evaporated what mass of KCl is present?
Match each term with its definition or description. 0000000 The point in a titration when the added amount of standard reagent is equal to the amount of analyte being titrated. A volumetric analysis technique used to determine the unknown concentration of a solution by using the known concentration of another. A solution of unknown concentration. The standard reagent of known concentration that is added from a buret to the analyte solution. A common concentration unit - moles per liter. The point in a titration when a change in the analyte solution is observed, indicating equivalency. It is added to the analyte solution and aids in the observation of the completion of the reaction. molarity equivalence point Answer Bank end point titration titrant analyte indicator
An aqueous solution of an unknown solid salt was placed into five different test tubes. Into each test tube a couple of drops of different indicators were then added to each test tube and the color of the indicator in the solution was recorded as shown below. What is the approximate pH of the solution? Test pH Acid Base Color in Unknown Indicator tube Range Color Color Solution 3.0 - 1 Methyl orange 4.4 Red Yellow Yellow 3.0 - Congo Red Purple Red Red 5.0 Bromcresol 3.8 - Yellow Blue Blue Green 5.4 Bromthymol 6.0 - 7.6 4 Yellow Blue Yellow Blue 8.2 - Phenolphthalein Colorless Blue Colorless 10.0 4.3 O 8.4 O 5.2 6.7
Use the following two titration curves to answer each of the following statements. Select the choice that completes the statement correctly. 14 pH 7 0 Graph A 25 volume of titrant added (mL) In graph A, the end point occurs at a In graph B, the equivalence point occurs at a + 141 pH 7 0 Graph B 25 volume of titrant added (mL)
The amount of acid or base the buffer can neutralize before the pH begins to change to an appreciable degree Buffer Buffer capacity Buffer equation Henderson-Hasselbalch
A buffer contains equal amounts of a weak acid and conjugate base and has a pH of 5.25. How will the concentration of weak acid in the buffer change after the addition of a small amount of strong acid? the concentration of weak acid will not change the concentration of weak acid will increase the concentration of weak acid will decrease
MISSED THIS? Read Section 18.4 (Pages 803-817); Watch KCV 18.48 Consider the curve shown here for the titration of a weak monoprotic acid with a strong base. 14 12- 10- 8 6 4 2- 0 0 10 20 30 40 Volume of base added (mL) ▶ Part A ▸ Part B Part C At what volume of added base is the pH calculated by working an equilibrium problem based on the initial concentration and K₁ of the weak acid? Express your answer in milliliters as an integer. V= ΠΗΓΙΑΣΦ VAX by Submit Previous Answers Request Answer X Incorrect; Try Again ? mL
Suppose that a buffer contains equal amounts of a weak acid and its conjugate base. What happens to the relative amounts of the weak acid and conjugate base when a small amount of strong acid is added to the buffer? What happens when a small amount of strong base is added?