Answered: The pH of a 0.92M solution of…

The pH of a 0.92M solution of hypobromous acid (HBRO) is measured to be 4.34. Calculate the acid dissociation constant K, of hypobromous acid. Round your answer to 2 significant digits.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 16CR

See similar textbooks

Related questions

Q: Calculate the pH of the following acid or base: 1. 3.6x10 M HNO,

A: pH stands for hydrogen potential in a solution. Low pH (less than 7.0) - Acidic pH pH = 7.0 -…

Q: Illustrate using an equation, the meaning of the terms: conjugate acid and conjugate base. Give…

A: The question is based on the concept of conjugate acid & base .

Q: Calculate the pH of each solution given the following. [H3O+]=9×10−6M Express your answer using…

Q: 20. Which of the following mathematical equations corresponds to the acid dissociation constant (K)?

Q: Arrange in terms of increasing acidic and explain these using partial charges and inductive effects

Q: What is the pH of a 0.0556 M NH, (aq) solution at room temperature? The base ionization constant of…

Q: USE A REAL LIFE SITUATION TO INTRUDUCE AND EXPLAIN THE TOPIC: ACID AND BASES WHILE INCLUDING THE PH…

A: Acid are those substances which are sour in taste. It's pH is less than 7. Example:- tartaric acid…

Q: In most solutions containing a strong or weak acid, the autoionization of water can be neglected…

A: Acid is a compound that donates proton and base is a compound that accepts proton. The strength of…

Q: What is the pH of a 0.0350 M NaOH solution? Use correct number of significant figures. Explain why…

A: The required relationships are given below. pH + pOH = 14 pOH = -log [OH-]

Q: Calculate the concentration to the correct number of HO JAOH) significant figures for solutions with…

Q: Fill in blanks(): If the pH of a solution increases by 3, the acidity of the solution ( ) by a…

Q: Calculate the concentration of all solute species in each of the following solutions of acids or…

A: Given that 0.0092 M HCIO 0.0784 M C6H5NH2, a weak base

Q: Can you show me an example of how to calculate an answer similar with a pH of 9.5?

A: We know that when pH is in between 0-7 then the solution is acidic and when it is in between 7-14…

Q: Use this data to rank the following solutions in order of increasing pH. In other words, select a…

A: For salt of weak acid and strong base. pH = 7+{pKa + log[Salt]}/2 And pH>7 For…

Q: Summarize the important difference between strongacids and weak acids in terms of the battle of the…

A: ANSWER IS DISCUSSED BELOW :

Q: If ammonia (NH3) acted as a strong base, what would be the pH of a 0.1 00 M solution of ammonia?…

Q: What is the conjugate base of HCO3 ? Express your answer as a chemical formula. > View Available…

Q: Calculate the pH of the following given the molar hydrogen ion concentration. A. Carrots,…

A: Used Formula- pH=-log[H^+] [H^+]=9.4×10^-6M

Q: Determine the relation between the pH values of the two solutions. Select the correct choice below…

A: pH = -log [H+]

Q: Acid and bases. Solving for OH, pOH, H+, pH

A: pH is given by the negative logarithm of hydrogen ion concentration. pOH is given by the negative…

Q: The acid dissociation constant K, of boric acid (H,BO3) is 5.8 × 10 Calculate the pH of a 2.5M…

A: Give, the dissociation constant (Ka) of boric acid = 5.8×10-10 We have to calculate the pH of a 2.5…

Q: (i) Define pH in words. The strong acid HCla has a pH value of 1, use the following equation HCL ->…

A: We have to define pH and find the concentration of H+ ion

Q: Use information on the table below to determine which of the following bases would have the weakest…

A: Lowest Ka value indicates lowering the acid strength.

Q: Calculate the pH of a 6.9 × 10 -5 °M aqueous solution of hydrochloric acid (HCI). Round your answer…

Q: The pH of a solution is (6.5x10^0). What is the [OH-]? Report your answer to 2 sig figs. Note: Your…

A: Given, pH of the solution = 6.5 × 100 = 6.5 Concentration of the OH- ion = [OH-] = ? The formula…

Q: Construct the expression for Ka for the weak acid, CH-COOH. CH.COOH(aq) + H₂O(l) = H₂O (aq) + CH.COO…

A: Ka is the ratio of the equilibrium concentrations of product over equilibrium concentrations of…

Q: Explain what the pH scale measures, and state acidic, neutral, and basic pH values

A: pH of a solution measures acidic or basic or neutral nature of solution or concentration of…

Q: Fill in the missing chemical formulae in the tables below. acid conjugate base H,0 HI HSO,

A: Check the conjugate base for given acid. Conjugate base is formed by donating proton from acid. Now…

Q: Would an aqueous solution of 0.25M sodium formate be acidic, basic or neutral? Write the equation…

A: Given, An aqueous solution of 0.25M sodium formate is:

Q: Complete the table below. Round each of your entries to 2 significant digits. You may assume the…

A: According to Bronsted-Lowry theory, an acid is a proton donor and a base is a proton acceptor. The…

Q: Give at least five (5) theories of acids and bases. Give at least one (1) example for each theory to…

A: There are different theories which can be used to define acid and base

Q: triprotic

A: For triprotic acid, Ka1 > Ka2 > Ka3 More H+ ion comes from first dissociation and second…

Q: Define and give examples of conjugate acids and bases.

A: CONJUGATE ACID and BASE PAIRS As we know that , According to Bronsted - Lowry concept , an acid…

Q: Classify the following as Brønsted acids, bases or both. Write the letter that corresponds to your…

A: According to Bronsted acid base theory, acid are the specie that donate H+ and base are specie that…

Q: What is the pH of a solution containing 0.453 mol L-1 HF and 0.267 mol L-1 F- ? Round your answer to…

A: Given, [HF] = 0.453 M [F-] = 0.267 M What is the pH of the solution = ?

Q: The pH of a 0.33 M solution of barbituric acid (HC,H;N,0;) is measured to be 2.25. Calculate the…

A: Since pH = -log[H+] where [H+] = concentration of H+ ions Hence 2.25 = -log[H+] => [H+] = 5.62 X…

Q: Indicate whether the chemical species HC6H5O72- acts as an acid or base when added to water.

A: Acid : when acid is added to water , it gives hydrogen ion (H+) in aqueous solution. Eg. : HCl…

Q: White vinegar is a 5.0% by mass solution of acetic acid in water. If the density of white vinegar is…

Q: The acid dissociation constant K, of hypobromous acid (HB1O0) is 2.3 × 10°. Calculate the pH of a…

A: Please find your solution below : pH is the measure of acidity or alkalinity of solution. It is…

Q: The pH of a 0.72 M solution of hydrofluoric acid (HF) is measured to be 1.66. Calculate the acid…

A: HF is a weak acid. Hence it will dissociate partially as per the reaction HF ------> H+ + F-

Q: A chemist dissolves 692. mg of pure hydroiodic acid in enough water to make up 60. mL of solution.…

Q: Calculating the pH of a weak acid solution The acid dissociation constant K, of hypobromous acid…

A: Given information: Acid dissociation constant for HBrO = 2.3×10-9 Concentration of hypobromous acid…

Q: What is the pH of a solution with OH- of 0.0001 M KOH at 25°C. Give the answer in 2 significant…

A: Question 2. Concentration of KOH = 0.0001 M To be calculated :- pH of solution Nature of…

Q: Calculate the concentration to the correct number of HO]AOH] significant figures for solutions with…

A: pH is the -log [H+] and pOH is the - log [OH-] From these two formula we can calculate the…

Q: The pH of a 0.33 M solution of hydrofluoric acid (HF) is measured to be 1.82. Calculate the acid…

A: The pH of 0.33 M solution of hydrofluoric acid (HF) is measured to be 1.82. The acid dissociation…

Q: In H₂O, HF is weak and the other hydrohalic acids areequally strong. In NH₃, however, all the…

A: Solution-When we say that an acid is a strong acid we mean that, that specific aciddissociates…

Q: Calculate the concentration to the correct number of HO JAOH] significant figures for solutions with…

Q: HCl (hydrochloric acid) NaOH (sodium hydroxide

Q: The pH of a 0.90M solution of hydrofluoric acid (HF) is measured to be 1.61. Calculate the acid…

A: pH = 1.61 HF = 0.9 M Acid dissociation constant = ? Create an ICE chart: HF…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

The pH of a 0.92M solution of hypobromous acid (HBRO) is measured to be 4.34.
Calculate the acid dissociation constant K, of hypobromous acid. Round your answer to 2 significant digits.
K
%3D
a
x10
Canti
2021 McGraw Hill LLC.

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 Given

VIEW

Step 2 Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 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

For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Calculate the concentration of all solute species in each of the following solutions of acids or bases. Assume that the ionization of water can be neglected, and show that the change in the initial concentrations can be neglected, Ionization constants can be found in Appendix H and Appendix I. (a) 0.0092 M HCIO, a weak acid. (b) 0.0784 M C6H5NH2, a weak base. (c) 0.0810 M HCN, a weak acid. (d) 0.11 M (CH3)3N, a weak base. (e) 0.120 M Fe(H2O)62+ a weak acid, Ka=1.6107
Which of the following conditions indicate a basic solution? pOH = 11.21 pH = 9.42 (OH’] > IH+| |OH] > 1.0 X IO’7M
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
The ideal pH of a swimming pool is 7.2. You measure the pH of your pool to be 6.5. What should you add, acid or base, to restore your pool to the ideal pH? acid base neither
. In each of the following chemical equations, identify the conjugate acid-base pairs. a. NH3(aq)+H2O(l)NH4+(aq)+OH(aq) b. PO43(aq)+H2O(1)HPO42(aq)+OH(aq) c. C2H3O2(aq)+H2O(l)HC2H3O2(aq)+OH(aq)
Mark each of the following statements True or False: a. The conjugate base of a strong acid is always a weak base. b. The conjugate acid of a strong base is always a weak acid. c. The stronger the acid, the weaker its conjugate base, and vice versa.
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. H3PO4 b. H3PO3 c. HBr d. HC2H3O2