O ACIDS AND BASESCalculating the pH at equivalence of a titration0/3A chemist titrates 60.0 mL of a 0.5297M hypochlorous acid (HCIO) solution with0.6423M KOH Solution at 25 °c. Calculate the pH at equivalence. The pk ofhypochlorous acid is 7.50.Round your answer to 2 decimal places.Note for advanced students: you may assume the total volume of thesolution equals the initial volume plus the volume of кOH solution added.pH = 0X

Answered: Image /qna-images/answer/dd434c7c-4234-4d82-b526-085e805261e7.jpg

A chemist titrates 60.0 mL of a 0.5297M hypochlorous acid (íCIO) solution with 0.6423M KOH Solution at 25 °c. Calculate the pH at equivalence. The pk₁ of hypochlorous acid is 7.50. Round your answer to 2 decimal places.

A chemist titrates 60.0 mL of a 0.5297M hypochlorous acid (íCIO) solution with 0.6423M KOH Solution at 25 °c. Calculate the pH at equivalence. The pk₁ of hypochlorous acid is 7.50. Round your answer to 2 decimal places.

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 chemist titrates 170.0 mL of a 0.2489M nitrous acid (HNO₂) solution with 0.7980 M NaOH solution at…

A: Given,molarity of HNO2 = 0.2489 Mvolume of HNO2 = 170.0 mL = 0.1700 LTherefore, number of moles of…

Q: A student needs to make a buffer solution, so he prepares a 0.200 M solution of benzoic acid,…

Q: A chemist titrates 220.0 mL of a 0.6779M acetic acid (HCH3CO₂) solution with 0.3134M KOH solution at…

A: At equivalence point, all the acid are consumed by the added acid. Here the moles of acid reacted…

Q: What is the pH of a buffered system made by dissolving 17.42 g of KH2PO4 (MM 136.1 g/mol) and 20.41…

A: Given : Mass of KH2PO4 = 17.42 g Mass of K2HPO4 = 20.41 g And Ka of KH2PO4 = 6.2 X 10-8 Molar mass…

Q: A solution is prepared at 25 °C that is initially 0.26M in chloroacetic acid (HCH,CICO,), a weak…

Q: A chemist titrates 130.0 mL of a 0.7392M trimethylamine ((CH3)N) solution with 0.3687 M HNO3…

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

Q: A chemist titrates 190.0 mL of a 0.3406 M dimethylamine CH32NH solution with 0.2721M HBr solution…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Phenylacetic acid (C6H5CH2CO2H) is a weak monoprotic acid with Ka = 4.90 × 10−5. What is the pH that…

A: 2.56 g of phenylacetic acid is mixed with 1.59 g of potassium phenylacetate and the solution is…

Q: The base constant for ammonia, NH3, is Kb = 1.8 x 10-5. A solution was made up with ammonium…

Q: What is the pH of a buffer solution that is 0.15 M puridine, C6H5N and 0.08 M pyridinium bromide…

Q: A volume 100.0 mL of a 0.20 M acetic acid CH,COOH solution is titrated by a 0.10 M lithium hydroxide…

A: LiOH is a strong base it reacts with weak acid CH3 COOH to give a buffer solution before equivalence…

Q: Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.223 M…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: A chemist titrates 170.0 mL of a 0.6472M cyanic acid (HCNO) solution with 0.6584M KOH solution at 25…

A: Given Volume of HCNO taken = 170.0 mL Molarity of HCNO = 0.6472 M Moles of HCNO = Volume of HCNO…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: A chemist titrates 140.0 mL of a 0.4198M dimethylamine ((CH3)2NH) pK, of dimethylamine is 3.27.…

Q: An analytical chemist is titrating 117.9 mL of a 0.3200M solution of benzoic acid (HC H₂CO₂) with a…

Q: A 50.00 mL sample of the weak acid CH3COOH (aq) at an initial concentration of 0.1000 M is titrated…

A: From Henderson hesselbalch equation, pH = pKa + log…

Q: A chemist titrates 190.0 mL of a 0.3602M lidocaine (C₁4H₂1 NONH) solution with 0.2711 M HCl solution…

A: Answer:- This question involves the titration of weak base against the strong acid. At equivalence…

Q: An analytical chemist is titrating 122.2 mL of a 0.1800M solution of dimethylamine ((CH3)₂NH) with a…

Q: A chemist titrates 230.0 mL of a 0.1110 M pyridine (C5H;N) solution with 0.7963 M HNO, solution at…

Q: A chemist titrates 190.0 mL of a 0.5697 M carbonic acid (H, CO,) solution with 0.1442 M KOH solution…

A: At the equivalence point mole of acid = mole of the base. The reaction involved is as follows:

Q: A chemist titrates 250.0 mL of a 0.8118 M pyridine (C,H,N) solution with 0.3729M HBr solution at 25…

A: Given, [C5H5N] = 0.8118 M Volume of C5H5N in mL = 250.0 mL [HBr] = 0.3729 M pKb of C5H5N = 8.77…

Q: A chemist titrates 170.0 mL of a 0.6249M benzoic acid (HC6H₂CO₂) solution with 0.1372M NaOH solution…

A: Given data 170 ml of benzoic acid 0.6249 M NaOH = 0.1372 M pka = 4.20

Q: An analytical chemist is titrating 152.2 mL of a 0.2200M solution of propionic acid (HC₂H₂CO₂) with…

A: The balanced equation for the reaction is HC2H5CO2 (aq) + KOH (aq) -----> KC2H5CO2 (aq) + H2O (l)

Q: A chemist titrates 250.0 mL of a 0.8331 M butanoic acid (HC,H,CO,) solution with 0.5749 M NaOH…

A: Molarity dilution equation: Given data: Concentration of butanoic acid=0.8331M. Volume of butanoic…

Q: Calculate the pH of the following two buffer solutions. Be sure your answer has the correct number…

A: According to Henderson–Hasselbalch equation pH = pKa + log {[salt] ÷ [acid]}

Q: A chemist titrates 130.0 mL of a 0.7300M butanoic acid (HC3H₂CO₂) solution with 0.6738 M NaOH…

Q: You are asked to prepare a pH = 3.00 buffer solution starting from 1.00 L of a 1.00 M solution of…

A: Given:pH of solution = 3.00Volume of HF solution = 1.00 LConcentration of HF = 1.00 MKa of HF =…

Q: A chemist titrates 70.0 mL of a 0.6885 M pyridine (CHN) solution with 0.5067M HBr solution at 25 °C.…

A: Solution :

Q: A solution is prepared at 25 °C that is initially 0.089 M in propanoic acid (HC₂H-CO₂), a weak acid…

A: Concentration of propanoic acid = [HC2H5CO2] = 0.089 M Concentration of potassium propanoate =…

Q: An analytical chemist is titrating 101.2 mL of a 0.4900M solution of dimethylamine ((CH3)2NH) with a…

A: To calculate the pH after the addition of the acid, we'll follow these steps:Determine the moles of…

Q: A chemist titrates 60.0 mL of a 0.4543 M aniline (C,H;NH,) solution with 0.7673M HNO, solution at 25…

Q: Consider a 50.0 mL sample of a solution composed of 0.25 M HNO2 and 0.25 M KNO2. Find the pH of the…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base. It…

Q: A chemist titrates 220.0 mL of a 0.0579M propionic acid (HC₂H₂CO₂) solution with 0.1972M KOH…

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

Q: An analytical chemist is titrating 150.4 mL of a 0.5000M solution of benzoic acid (HC H-CO₂) with a…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: When 22.6 mL of 0.229 M hydrochloric acid (HCI) and 22.6 mL of 0.229 M ammonia (NH3) are combined,…

Q: A chemist titrates 50.0 mL of a 0.4173M nitrous acid (HNO₂) solution with 0.2299 M KOH solution at…

Q: A chemist titrates 180.0 mL of a 0.4192 M cyanic acid (HCNO) solution with 0.5880M NAOH solution at…

A: Given Information- Volume of HCNO = 180.0 mL Molarity of HCNO = 0.4192 M Molarity of NaOH =…

Q: A chemist titrates 240.0 mL of a 0.4685M acetic acid (HCH3CO₂) solution with 0.3845 M NaOH solution…

A: The objective of the question is to calculate the at the equivalence point.

Q: A chemist titrates 210.0 mL of a 0.1055M hypochlorous acid (HCIO) solution with 0.3543M KOH solution…

A: Reaction between HClO and KOH is shown below: HClO(aq)+KOH(aq)→KOCl(aq)+H2O(l) According to reaction…

Q: An analytical chemist is titrating 156.4 mL of a 0.2700 M solution of butanoic acid (HC3H7CO2) with…

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.

Question

O ACIDS AND BASES
Calculating the pH at equivalence of a titration
0/3
A chemist titrates 60.0 mL of a 0.5297M hypochlorous acid (HCIO) solution with
0.6423M KOH Solution at 25 °c. Calculate the pH at equivalence. The pk of
hypochlorous acid is 7.50.
Round your answer to 2 decimal places.
Note for advanced students: you may assume the total volume of the
solution equals the initial volume plus the volume of кOH solution added.
pH = 0
X

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Description of problem statement

VIEW

Step 2: Determine the volume of KOH for equivalence point

VIEW

Step 3: Determine the pH at equivalence point

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 5 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Determine the pH of the resulting solution by mixing 0.36 M of sodium formate (HCOONA) of 20.0 mL with 0.18 M of HCI of 40.0 mL. Kp (HCOO") = 5.65 x 10-11. Your answer should have 3 significant figures.
An analytical chemist is titrating 92.2mL of a 0.4800M solution of piperidine C5H10NH with a 0.4500M solution of HNO3 . The pKb of piperidine is 2.89 .Calculate the pH of the base solution after the chemist has added 21.3mL of the HNO3 solution to it.
Calculating the pH at equivalence of a titration 1/5 Izabella A chemist titrates 140.0 mL of a 0.5644M nitrous acid (HNO 2) solution with 0.4397M KOH solution at 25 °C. Calculate the pH at equivalence. The pKa of nitrous acid is 3.35. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = - 0 ☑ ? 000 日。
Calculating the pH of a buffer -4 and 0.13M in sodium nitrite α A solution is prepared at 25 °C that is initially 0.15M in nitrous acid (HNO2), a weak acid with K₁ = 4.5 × 10¯ (NaNO2). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = ? olo 18 Ar B⚫
A chemist titrates 160.0 mL of a 0.3272M nitrous acid (HNO₂) solution with 0.3027M KOH solution at 25 °C. Calculate the pH at equivalence. The pK₁ of nitrous acid is 3.35. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = X Ś
A chemist titrates 60.0 mL of a 0.2562M benzoic acid (HC6H5CO₂) solution with 0.0811M KOH solution at 25 °C. Calculate the pH at equivalence. The pK of benzoic acid is 4.20. a Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = X S
A chemist titrates 160.0 mL of a 0.4056M hypochlorous acid (HC1O) solution with 0.4300M NaOH solution at 25 °C. Calculate the pH at equivalence. The PK of hypochlorous acid is 7.50. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added. pH = 0 X S
Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.241 M CsOH. With 0.00151 moles of C₅H₅NH⁺ and 0.00289 moles of C₅H₅N in the beaker, what would be the pH of this solution after the reaction goes to completion and the system reaches equilibrium?
An analytical chemist is titrating 110.0mL of a 0.5600M solution of butanoic acid HC3H7CO2 with a 1.100M solution of KOH . The pKa of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 31.66mL of the KOH solution to it. Round your answer to 2 decimal places.
A chemist titrates 120.0 mL of a 0.3246M cyanic acid (HCNO) solution with 0.2427M NaOH solution at 25 °C. Calculate the pH at equivalence. The p Ka of cyanic acid is 3.46. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added. pH = [] X Ś
An analytical chemist is titrating 243.8 mL of a 0.7000 M solution of butanoic acid (HC3H,CO2) with a 0.3800 M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 278.5 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. PH ☐ olo Ar
A 0.500 L solution is composed of 0.200 M (CH3)2NH and 0.200 M (CH3)2NH₂Cl at 25 °C. What is the pH of the solution after 0.040 moles of HBr are added to the solution at the same temperature? You may assume no change in volume for the system. Enter your answer with two decimal places. At 25 °C: Kb for (CH3)₂NH = 5.9 x 10-4 Kb for KOH= 3.2 x 10¹