### pH at Equivalence Point in Titration**Question:** What is the pH at the equivalence point when Jeremiah titrates NaOH with HClO₃?The reaction involved is:\[ \text{HClO}_3 + \text{NaOH} \rightarrow \text{NaClO}_3 + \text{H}_2\text{O} \]To find the pH at equivalence:\[ \text{pH} = \boxed{?} \]**Interactive Response:** Students can enter their calculated pH value in the provided text box and click "Enter" to submit their answer.---**Explanation:**When NaOH, a strong base, is titrated with HClO₃, a strong acid, the reaction goes to completion, producing sodium chlorate (NaClO₃) and water (H₂O). At the equivalence point, the amounts of acid and base are stoichiometrically equal, and the solution mainly contains the salt of the strong acid and base. The pH of the solution at this point is determined by the neutral nature of the salt, resulting in a pH close to 7.**Diagrams/Graphs:** There are no diagrams or graphs present in this example. The focus here is on the chemical equation and the calculation based on titration principles.

Here, we have to find the pH at the equivalence point when NaOH is titrated with HClO3.

Answered: What is the pH at the equivalence point…

What is the pH at the equivalence point when Jeremiah titrates the NaOH and HCIO3? HCIO3 + NaOH → NaCIO3 + H₂O pH = [?] pH at equivalence Enter

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

The volume required to reach the equivalence point of an acid– base titration depends on the volume and concentration of the acid or base to be titrated and on the concentration of the acid or base used to do the titration. It does not, however, depend on the whether or not the acid or base being titrated is strong or weak. Explain.
Answer Questions #27 through #31 about the titration curves below (labeled a and b) for two different bases. The titrant acid used in both cases was 0.100 M HCl and the volume of the base solutions in both cases was 75.0 mL mL. 14 14 12 12 - 10- 10 8- 6. 4. 2- 2- 20 40 60 80 100 20 40 60 80 100 Volume of acid added (mL) (a) (b) Volume of acid added (mL) 2014 Pearson Education Inc P Type here to search 11:17 AM (? 3/18/2021 -> ort sc 80 6. ece num ER/TY || на 0 04 2C Hd
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 ]
Determine the pH during the titration of 11.4 mL of 0.231 M nitric acid by 4.23x10-² barium hydroxide at the following points: (1) Before the addition of any barium hydroxide (2) After the addition of 15.6 mL of barium hydroxide (3) At the equivalence point (4) After adding 39.2 mL of barium hydroxide 4
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)
25.00 mL of 0.100 M HCl solution is titrated with a 0.100 M NaOH solution. What is the pH of the solution after the addition of the following strong base? (pH= - log[H3O+] = - log[H+]) a) initially (Before adding NaOH) b) Before the equivalence point (with the addition of 24.00 mL of 0.100 M NaOH) c) At the equivalence point (with the addition of 25.00 mL of 0.100 M NaOH) d) After the equivalence point (with the addition of 26.00 mL of 0.100 M NaOH)
Given the titration curve of a weak acid, at which region is the buffer capacity considered maximized? IV II pH II volume of OH- added Select one: O a. Region I, because there is no strong base added O b. Region II, because there is almost equal amounts of weak acid and conjugate base O c. Region III, because it is the equivalence point, where equal amount of base is added to the weak acid O d. Region IV, because the buffer can easily neutralize acid or base at this point
Consider the titration curve for a diprotic acid: 12 10 8 pH 6 4+ 2 + + 10 20 30 Volume of NaOH added (mL) Label the curve with the following items: first equivalence point, second equivalence point, first halfway point, halfway between first and second equivalence points. Determine K, and K, for this diprotic acid. al a2
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
O ACIDS AND BASES Calculating the pH of a weak base titrated with a strong acid with a 0.3000 M solution of HNO,. The p K, of An analytical chemist is titrating 160.2 mL of a 0.5000 M solution of dimethylamine ((CH₂)2NH) w dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 280.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places... PH-0 X
In the titration of a solution of weak monoprotic acid with a O.1450 M solution of NaOH, the pH half way to the equivalence point was 4.38. In the titration of a second solution of the same acid, exactly twice as much of a 0.1450 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
What is the pH of a buffer solution made by adding 0.41 g of NaC2H3O2 to 100. mL of 0.10 M HC2H302? Molar mass of NaC2H3O2 = 82.0 g/mol Ka of HC2H3O2 = 1.8x10-5 pH of buffer [?] pH of Buffer Enter