Which of the following(s) is(are) correct about the equivalence point in titration of acids with strong base,NaOH?I. The source of proton is due to self dissociation of water at equivalence point for strong acid-basetitrationsII. The pH is calculated based on reaction of A with H20 at the equivalence point for weak acid and strongbase titrationII. pH>7 at equivalence point when weak acid is titrated with strong baseLütfen birini seçin:a.Il and IIIb.I and IIIC.1, Il and IIWindows'u EtkinleştirWindows'u etkinleştirmek için Ayarlara gidin.d.I and II13:2916.05.202110DELL

To find the following the true statements: I. The source of proton is due to self dissociation of…

Which of the following(s) is(are) correct about the equivalence point in titration of acids with strong base, NaOH? 1. The source of proton is due to self dissociation of water at equivalence point for strong acid-base titrations II. The pH is calculated based on reaction of A with H2O at the equivalence point for weak acid and strong base titration II. pH >7 at equivalence point when weak acid is titrated with strong base Lütfen birini seçin: a. Il and III b. I and II C. 1, Il and II Windows'u Etkinleştir Windows u etkinleştirmek için Ayarlata idi

Which of the following(s) is(are) correct about the equivalence point in titration of acids with strong base, NaOH? 1. The source of proton is due to self dissociation of water at equivalence point for strong acid-base titrations II. The pH is calculated based on reaction of A with H2O at the equivalence point for weak acid and strong base titration II. pH >7 at equivalence point when weak acid is titrated with strong base Lütfen birini seçin: a. Il and III b. I and II C. 1, Il and II Windows'u Etkinleştir Windows u etkinleştirmek için Ayarlata idi

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

Similar questions

When titrating a weak acid with a strong base, what is the approx. pH expected for the equivalence point (at 25oC.)? Why is this expected to be a different pH than the equivalence point pH for a strong acid with a strong base titration?
In an acid-base titration, a base or acid is gradually added to the other until they have completely neutralized each other. Since acids and bases are usually colorless (as are the water and salt produced in the neutralization reaction), pH is measured to monitor the reaction. Suppose that the equivalence point is reached after approximately 393 mL of a NaOH solution has been added (enough to react with all the acetic acid present) but that replicates are equally likely to indicate from 373 to 417 mL (exclusive), measured to the nearest mL. Assume that two technicians each conduct titrations independently. What is the probability that the average volume at equivalence from the technicians is 416 mL or 417? Select one: O a. 0.79069767 b. 0.00000000 c. 0.00054083 d. 1.00000000 e. 0.00049383 f. 0.02941176 O g. 0.04651163 O O
Why is a buffer composed of Hc2H3O2 and NaC2H3O2 more effective at maintaining the Ph of a solution at a pH of 4.75 than a buffer composed of HCN and NaCN? Thanks sooo much, I'm so confused.
For each scenario below, select the color of the solution using the indicator thymol blue during the titration. When you first add indicator to your Na₂CO3 solution, the solution is basic (pH ~10), and the color is [Select] At the equivalence point for the titration, the moles of added HCI are equal to the moles of Na₂CO3. One drop (or less!) past this is called the endpoint. The added HCI begins to titrate the thymol blue indicator itself. At the endpoint, the indicator color is [Select] When you weren't paying attention and added too much HCI (~12 mL extra), the color is [Select] When you really weren't paying attention and reached the second equivalence point of Na₂CO3, the color is [Select ]
2)Make a rough plot of pH versus milliliters of acid added for the titration of 50.0 mL of 1.0 M NaOH with 1.0 M HCl. Indicate the pH at the following points and tell how many milliliters of acid are required to reach the equivalence point. a)Before the titration starts b)At the equivalence point c)After an additional 10.0 mL of HCL is added after the equivalence point (i.e. equivalence point volume + 10.0 mL)
A 25.0 sample of a saturated Ca(OH) 2 solution is titrated with 0.029 HCI and the equivalence point is reached after 372 of dispersed. Based on this data what is the concentration (M) of the hydroxide lon?
How many milliliters of a 0.250 M acetic acid solution must be added to 50.0 mL of a 0.750 M NaOH solution to produce a buffer solution withpH = 4.500 ?
For each scenario below, select the color of the solution using the indicator thymol blue during the titration. When you first add indicator to your Na2CO3 solution, the solution is basic (pH ~10), and the color is [Select] At the equivalence point for the titration, the moles of added HCI are equal to the moles of Na2CO3. One drop (or less!) past this is called the endpoint. The added HCI begins to titrate the thymol blue indicator itself. At the endpoint, the indicator color is [Select] When you weren't paying attention and added too much HCI (~12 mL extra), the color is [Select] When you really weren't paying attention and reached the second equivalence point of Na2CO3, the color is ✓ [Select] blue yellow red orange green Question 9
A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.027 M HCI, and the equivalence point is reached after 38.1 mL of titrant are dispensed. Based on this data, what is the concentration (M) of the hydroxide ion? Type answer: 0.041
Strong acid-strong base titration 6) A 100.0 mL sample of 0.18 M HCIO4 is titrated with 0.27 M LIOH. Determine the pH of the solution a) before the addition of any b) after the addition of 30.0 mL of LİOH. c) after the addition of 50.0 mL of LIOH. d) after the addition of 66.67 mL of LiOH (this is the equivalence point). e) after the addition of 75.0 mL of LIOH. LIOH.
A buffer solution is made by mixing 55.0 mL of 0.115 M HCOOH and 45.0 mL of 0.160 M HCOONA. K, of HCOOH = 1.8 x 10-4. a) The buffer range of this buffer is as low as pH and as high as pH b) The pH of this buffer is c) The maximum volume in milliliters of 0.210 M KOH that can be neutralized by this buffer is mL. d) The pH of the solution, after 20.0 mL of 0.200 M HI is added to the original buffer is
explain why the pH for equivalence point when titrating a weak acid with a strong base would not be 7. use the neutralization between acetic acid, (CH3COOH) and sodium hydroxide (NaOH) to help you explain