Answered: Consider the titration of 20.00 mL of…

Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3 is 2.2 x 10–5. What is the pH 2.00 mL past the equivalence point volume?

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

Related questions

Q: A 6.00 mL sample of 0.50 M NH3 is titrated with 0.15 M HCI. What is the pH of the solution after…

Q: Calculate the pH at the equivalence point in titrating 0.045 M solutions of each of the following…

A: Concept based on the finding out the pH at the he equivalence point between the acid- base…

Q: A 100.00mL solution of 1.00 M in HC2H3O2 is titrated with 1.00 M NaOH. Find the pH after 100.00mL of…

Q: Consider the titration of 50.0 mL of 0.0462 M HNO3 with 0.100 M KOH. What is the pH of the solution…

A: pOH = -log[OH-]pH = 14 - pOH

Q: A 65 mL sample of 0.460 M acetic acid (CH3CO2H) is titrated with 0.325 M NaOH. Calculate the pH of…

Q: Consider the titration of 100.0 mL of 0.200 M acetic acid (K, = 1.8 × 10-5) by 0.100 M KOH.…

Q: Sketch the titration curve when 10.0 mL of a 0.20 M solution of the polyprotic weak acid H2CO3 is…

A: H2CO3 is a weak diprotic acid. When it is titrated with NaOH, we see two inflection points.

Q: A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after…

Q: A 100ml sample of 0.20M HF is titrated with 0.10M NaOH. Determine the pH of the solution after the…

Q: The p?apKa of hypochlorous acid is 7.5307.530. A 54.054.0 mL solution of 0.1190.119 M sodium…

Q: 100.7 mL of 0.51 M HNO3 titrated with 0.26 M NaOH. What is the pH at the halfway point?

A: The number of moles of nitric acid (strong acid) can be determined as follows: Number of moles of…

Q: Titration curve for the titration of 25mL of 0.1 M NH3 with 0.1 HCl. What is the pH before any acid…

A: The question is based on the concept of titrations. we are titrating a weak base with a strong…

Q: Calculate the pH in the titration of 25.0 mL of 0.100 M acetic acid by sodium hydroxide after the…

A: Given volume of acetic acid is 25.0mL and strength is 0.100 M. Given volume of NaOH is 30.0 mL and…

Q: An analytical chemist is titrating 121.0 mL of a 0.3000M solution of isopropylamine ((CH) CHNH, with…

Q: culate the grams of the sodium salt that must be added to 100 ml of formic acid solution 0.25M Ka =…

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

Q: Titration of 0.1615 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 21.84 mL…

A: Given, An unknown monoprotic acid (HA) Molarity of NaOH solution = 0.1231 M = 0.1231 mol/L Volume…

Q: Calculate the pH at the following points in the titration of 25.00 ml of 0.250 M HNO3 with 0.250 M…

A: The acids which completely dissociate in the solution releasing hydronium ions are called strong…

Q: Consider the titration of a 20.0-mL sample of 0.100 M HC2H3O3 (Ka=1.8×10−5) with 0.125 M NaOH.…

A: Given question is related to calculating the pH at equivalent point in acid-base titration reaction.…

Q: A solution is made by dissolving 0.1283 g of the acid form of the buffer TRIS (molecular mass =…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: 10.00mL of O.10M HCI were collected in an Erlenmeyer flask, and 100mL with distilled water. After…

A: HCl is an acid and NaOH is a base and both react to form salt and water. The H+ ions dissociated…

Q: A 25.0mL sample of 0.653 M HN3 (ka = 1.9 x10^-5) is titrated with 0.777 M KOH Calculate the pH at…

Q: 10.0 mL of 0.80 M HF is titrated with 0.30 M NaOH. What is the pH of the solution after 10.0 mL of…

Q: Suppose we have a formula for the titration function P(x). What calculation would we want to do to…

A: Weak acids dissociate partially in an aqueous solution to furnish the hydrogen ions. The extent to…

Q: Calculate the pH at the equivalence point for the titration of 30.0 mL of 1.00 M HCN with 0.800 M…

A: The question can be solved using pH equilibrium concept as HCN is a weak acid so at equivalence…

Q: Consider the titration of a 34.0 mL sample of 0.135 molL−1 C3H7COOH (Ka=1.3\times 10−5) with 0.140…

A: Given ,

Q: A 15.00 mL sample of 0.355 M H3PO4 (Ka,1 7.52 ´ 10–3 , Ka,2 6.23 ´ 10–8 , Ka,3 2.1 ´ 10–13) is…

Q: c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results are…

A: Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated…

Q: Consider the titration of 50.00mL of 0.100M CH3CO2H with 0.100M NaOH. Acetic acid has Ka = 1.8x10-5…

A: The volume of NaOH needs to be added to the given solution to make the pH=7 can be calculated by the…

Q: Construct a rough plot of pH versus volume of added base for the titration of 50 mL of 0.045 M HCN…

Q: A certain acetic acid solution has pH = 2.68. Calculate the volume of 0.0975 M KOH required to reach…

A: we have to calculate the volume of KOH needed at the equivalence point

Q: A sample of 50.0 mL of 2.0 M HNO, (pKa=3.398) is titrated with 1.0 M KOH. Determine the pH after the…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: a) What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA…

A: the solution is as follows:

Q: You are titrating a 700 mL sample of 0.15 M CCI3COOH (pKa = 0.66) with 0.2 M NaOH. What will the pH…

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

Q: 25.0 mL of 0.225 M HNO2 is titrated to its equivalence point with 1.00 M NaOH. What is the pH at…

A: Equivalence point is the point where the amount of titrant ( NaOH) added is enough to completely…

Q: Determine the pH at the equivalence point in the titration of 50.0 mL of 0.300 M CH₃COOH with 0.300…

Q: Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3…

Question

Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN₃) with 0.1250 M HCl. The K_a of HN₃ is 2.2 x 10^–5. What is the pH 2.00 mL past the equivalence point volume?

Expert Solution

Step 1

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

A titration of 3.36 g of an acid requires 43.72mL of 0.100M NaOH to reach the equivalence point. What is the molar mass of the acid?
Calculating the pH of a weak base titrated with a strong acid An analytical chemist is titrating 104.1 mL of a 0.1200M solution of propylamine (C,H,NH,) with a 0.2600M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 53.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume eguals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy | Accessibility APR 23 MacBook Air O00 000 F4
When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5 1) Calculate the pH at this point 2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?
A 25.0 mL sample of 0.86 M HCOOH is titrated with 0.20 M KOH. What is that pH of the solution at equivalence point ? Ka= 1.77 x 10^-14
You are given a 1.00 L buffer solution that is 0.250 M in HF and 0.250 M in LiF. Find the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4.
Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3 is 2.2 x 10–5. What is the pH at the equivalence point?
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 ratio of NaCN to HCN is needed to prepare a pH 10.00 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)
A 26.25 mL sample of 0.32 M CH3COOH is titrated with 0.24 M LIOH. What is the pH of the solution after 35.0 mL of LIOH has been added to the acid? Ką of CH3COOH = 1.8 × 10-5 None of these 2.84 11.16 5.09 8.91