A solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium hypochlorite in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCI to this buffer solution causes the pH to drop slightly. The pH does not present in the buffer solution. The Ka of hypochlorous acid is 1.36 decrease drastically because the HCI reacts with the ×10-³. Select one: Oa. hypochlorous acid Ob. H30¹ Oc H2O Od. hypochlorite ion

A solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium hypochlorite in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCI to this buffer solution causes the pH to drop slightly. The pH does not present in the buffer solution. The Ka of hypochlorous acid is 1.36 decrease drastically because the HCI reacts with the ×10-³. Select one: Oa. hypochlorous acid Ob. H30¹ Oc H2O Od. hypochlorite ion

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 22.6 mL sample of 0.221 M ethylamine, C₂H5NH2, is titrated with 0.207 M hydrobromic acid. After…

Q: (a) Calculate the pH of a buffer solution containing 0.40 mole of KF and 0.50 mol of HF in 1.50…

A: pH of buffer solution is calculated using Henderson–Hasselbalch equation, amount of strong acid HCl…

Q: An analytical chemist is titrating 189.5 mL of a 0.6500M solution of ammonia (NH,) with a 0.8000M…

Q: Buffer solution is made by taking 0.404 moles of acid (Pka=5.83) & 0.468 moles of sodium acetate and…

Q: An analytical chemist is titrating 86.6 mL of a 0.4900M solution of dimethylamine ((CH,) NH) with a…

A: Step 1:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: An analytical chemist is titrating 216.4 mL of a 0.4800 M solution of cyanic acid (HCNO) with a…

A: Given: Volume of HCNO = 216.4 mL Concentration of HCNO = 0.480 M Volume of NaOH = 363.3 mL…

Q: Calculate pH for a strong acid/strong base titration. Determine the pH during the titration of 23.2…

Q: what volume of acetic acid 0.1 M and what volume of sodium acetate 0.1 M should be added together to…

A: Let the volume of acetic acid be x and the volume of sodium acetate solution be y. The pKa value of…

Q: The pH of this solution is equ HCN. The pK, value of HCN will d is added. The cyanide ion…

A: As concentration of HCN is double the concentration of NaCN. Now, if we add strong base in the…

Q: A 1.50 L buffer solution is 0.250M in HF and 0.250 M in NaF. Calculate the pH of the solution after…

Q: An analytical chemist is titrating 247.0 mL of a 0.6700M solution of propionic acid (HC,H,CO,) with…

Q: How many moles of sodium hydroxide would have to be added to 225 mL of a 0.316 M acetic acid…

Q: An analytical chemist is titrating 191.3 mL of a 0.8900M solution of hydrazoic acid (HN,) with a…

Q: 2. Giving reasons, explain which of the following can form hydrogen bonds with water? (a) CH3OCH3…

A: Hydrogen bonding- It is a attractive force between hydrogen atom covalently bonded to…

Q: Why does buffer capacity increase as the concentration of buffer increases?

A: The solutions which have a nearly constant value of pH or they resist any change in pH value are…

Q: An analytical chemist is titrating 163.7 mL of a 0.6200M solution of hydrazoic acid (HN,) with a…

A: Given that, Volume of 0.6200 M HN3 acid = 163.7 mL = 0.1637 L Moles of HN3 acid = 0.62 M×0.1637 L =…

Q: An analytical chemist is titrating 56.7 mL of a 0.4900M solution of formic acid (H,CO,) with a…

Q: What is the pH of a buffer solution with equal parts acetic acid and sodium acetate?

Q: I prepare a buffer solution by mixing 30.0mL of 0.10M HOAc and 40.0mL of 0.10m NaOAc. I divide this…

Q: How many moles of potassium hydroxide would have to be added to 150 mL of a 0.469 M hypochlorous…

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

Q: 1.0 mol NaH2PO4 and 1.0 mol Na2HPO4 are added to sufficient water to give a 1L buffer solution.…

Q: An analytical chemist is titrating 59.1 mL of a 0.6700 M solution of ammonia (NH,) with a 0.4500 M…

A: Given : Concentration of NH3 = 0.6700 M Volume of NH3 solution = 59.1 mL = 0.0591 L…

Q: Buffers resist pH by neutralizing any acid or base that is added to them. Consider the HC2H3O2 and…

A: An acetate buffer is a type of buffer solution made from a weak acid, acetic acid (also known as…

Q: Calculate the pH of the following buffer solutions:

A: a)Moles of KH2PO4 =2.668g/136gmol-1 =0.019617 mol Moles of K2HPO4=2.095g/174.2gmol-1 =0.0120264 mol…

Q: A buffer solution contains 0.302 M NaHSO3 and 0.438 M K2SO3. If 0.0168 moles of hydrochloric acid…

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

Q: A 27.5 mL sample of 0.306 M ethylamine, C₂H5NH₂, is titrated with 0.205 M hydrochloric acid. After…

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

Q: Given a solution in a volume of 200 ml of HCN 0.3M. We titrate the acid with a 0.75 M KOH solution.…

A: Given, Volume of HCN = 200 mL = 0.2 L (1mL = 0.001 L) Molarity of HCN = 0.3 M = 0.3 mol/L Molarity…

Q: There are 250 ml of a Buffer solution, where the concentration is 0.225 M of acetate of sodium and…

A: Buffer solution is a mixture of weak acid and it's conjugate base or a weak base with its conjugate…

Q: Calculate the pH of the buffer system made up of 0.15 M NH3NH3/0.35 M NH4ClNH4Cl.

A: The Henderson hasselbalch equation for calculation of pH of a buffer is pH = pKa + log[base][acid]…

Q: If 0.50 mL of 0.087 M HCl is added to the solution in (a), how many moles of the acetic acid, sodium…

A: Here we are required to find the percent change in pH of the buffer when acid is added.

Q: An analytical chemist is titrating 231.8 mL of a 0.9900M solution of acetic acid (HCH,CO,) with a…

Q: An analytical chemist is titrating 111.3 mL of a 0.2800 M solution of ammonia (NH, with a 0.3500 M…

A: Titration of 111.3 mL of a 0.2800M solution of ammonia NH3 with a 0.3500M solution of HIO3 is…

Q: An analytical chemist is titrating 147.3 mL of a 0.3200M solution of ammonia (NH,) with a 0.8200M…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

A solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium hypochlorite in water sufficient to
yield 1.00 L of solution. The addition of 0.05 mol of HCI to this buffer solution causes the pH to drop slightly. The pH does not
present in the buffer solution. The Ka of hypochlorous acid is 1.36
decrease drastically because the HCI reacts with the
× 10-3.
Select one:
Oa. hypochlorous acid
Ob. H30¹
Ос H2O
Od. hypochlorite ion

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

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

An aqueous solution contains 0.25 M HF and 0.20 M NaF . The pKa for HF is 3.45. What is the pH of this solution?
There are 0.250 ml of a Buffer solution, where the concentration is 0.225 M of sodium acetate and 0.225 M of acetic acid. What will the change in pH be if 30 ml of a 0.1 M HCl solution are added?
For 550.0 mLmL of a buffer solution that is 0.135 MM in HC2H3O2 and 0.115 MM in NaC2H3O2, calculate the initial pH and the final pH after adding 0.020 molmol of HCl.
For an aqueous solution formed by mixing 4.50mL of 0.15M LIOH with 25.0mL of 0.100M C2H5CO2H (propanoic acid), a) determine whether this forms a buffer solution. b) determine the pH of this combined solution. c) state whether the addition of 6.75mL of 0.100M HCl to the solution will have a large or small effect on the pH of the solution. Explain your reasoning (using 1-2 sentences).
How does a buffer solution prevent larger change in pH? What does it mean when a solution has exceeded the buffer capacity?
A 1.50 L buffer solution consists of 0.280 M propanoic acid and 0.139 M sodium propanoate. Calculate the pH of the solution following the addition of 0.065 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The Ka of propanoic acid is 1.34×10^−5.
A 1.33 L buffer solution consists of 0.168 M butanoic acid and 0.272 M sodium butanoate. Calculate the pH of the solution following the addition of 0.075 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The ?a of butanoic acid is 1.52×10−5.
An analytical chemist is titrating 94.2 mL of a 0.4600M solution of dimethylamine ((CH,),NH) with a 0.2300M solution of HNO,. The p K, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 121.9 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 =||
Describe the role of buffers in maintaining the pH of a solution.