Answered: The pH of a 0.94M solution of…

The pH of a 0.94M solution of hydrofluoric acid (HF) is measured to be 1.60. Calculate the acid dissociation constant K, of hydrofluoric acid. Round your answer to 2 significant a K = 0 %3D x10

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 59QRT

See similar textbooks

Related questions

Q: The acid dissociation constant K of hydrocyanic acid (HCN) is 6.2 x 10-¹0. Calculate the pH of a…

A: We need to find the pH of HCN from the given data. Ka of HCN is given as 6.2 × 10-10 and…

Q: The acid dissociation constant K of alloxanic acid (HCH₂N₂O5) is 2.24 × 10¯7. a Calculate the pH of…

A: Information of question

Q: Acid Ка Base Kb hypochlorous acid, HCIO 4.0 x 10°8 methylamine, CH3NH2 5.0 x 104 hydrofluoric acid,…

A: pH of different solution can be calculated using respective formulas.

Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 x 10 -10 Calculate the pH of a…

A: Given: Concentration of HCN = 3.6 M Ka = 6.2×10-10

Q: The acid dissociation constant K, of alloxanic acid (HC,H,N,0,) is 2.24 x 10 '. Calculate the pH of…

A: Answer

Q: The pH of a 0.17 M solution of propanoic acid (HC3H;O2 is measured to be 2.81. Calculate the acid…

A: The dissociation reaction is given by HC3H5O2 ----> H+ + C3H5O2- hence we can say that the H+…

Q: Part D In the simulation, open the Custom mode. The beaker will be filled to the 0.50 L mark with a…

A: The alkalinity or acidity of a solution is determined by the pH scale. It has a range from 0 to 14,…

Q: The acid dissociation constant Kof alloxanic acid (HCH³N₂O²) is 2.24 × 10 Calculate the pH of a 4.0M…

A: The concentration of = 4.0 MThe dissociation constant for acid = pH of the solution = ?

Q: The pH of a 0.052M solution of acrylic acid (HC,H,CO,) is measured to be 2.77. Calculate the acid…

A: GivenpH = 2.77pH = -logH+2.77 = -log H+H+ = 0.00169 M[H+] = 1.7 * 10-3 M

Q: The pH of a 1.4M solution of propanoic acid (HC,H,O,) is measured to be 2.36. Calculate the acid…

A: Given :- pH = 2.36 concentration of HC3H5O2 = 1.4 M To calculate :- Ka

Q: Calculate the pH of a 4.2M solution of hypobromous acid.

A: Ka is the ratio of product of concentration of products raised to their stoichiometric coefficient…

Q: The acid dissociation constant K, of acetic acid (HCH,Co,) is 1.8 × 10. Calculate the pH of a 0.48M…

A: Given : Concentration of acetic acid = 0.48 M Ka of acid = 1.8 x 10-5 To calculate : pH of…

Q: The pH of a 0.18M solution of 3-hydroxypropanoic acid (HC,H,O3) is measured to be 2.63. Calculate…

Q: -69 The acid dissociation constant K, of hypobromous acid (HBrO) is 2.3x 10. Calculate the pH of a…

A: Consider the dissociation of hypobromous acid is as follows: HBrO → H+…

Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 × 10 1". а -10 Calculate the pH…

A: In this question, we want to determine the pH of the Solution. You can see details Solution below.…

Q: Consider the following data on some weak acids and weak bases: acid base K. K, name formula name…

Q: Consider the following data on some weak acids and weak bases: acid base K. name formula name…

A: Salts are characterized into three subcategories depending upon their constituent acid-base pair.…

Q: The acid dissociation constant Ka of alloxanic acid HC4H3N2O5 is ×2.2410−7 . Calculate the pH…

A: Given acid is organic weak acid so it will dissociates partially into [Alloxanate] and [H3O+].…

Q: The acid dissociation constant K, of alloxanic acid (HC H₂N₂O) is 2.24 x 10 Calculate the pH of a…

A: Ka of alloxanic acid HC4H3N2O5 = 2.23×10-7Concentration of alloxanic acid = 3.9 MpH of the solution…

Q: The pH of a 0.46M solution of propanoic acid (HC,H,O,) is measured to be 2.60. Calculate the acid…

Q: The acid dissociation constant K, of carbonic acid (H,CO3) is 4.5 x 10. Calculate the pH of a 3.4M…

A: All details explained in Handwritten solution

Q: The pH of a 1.0 M solution of pentanoic acid (HC;H,O2) is measured to be 2.42. Calculate the acid…

A: Given information: Concentration of pentanoic acid = 1.0M pH of pentanoic acid = 2.42 The…

Q: The pH of a 1.2M solution of benzoic acid (HC,H,CO,) is measured to be 2.06. Calculate the acid…

A: Benzoic acid is a weak acid that dissociates very weakly to form a weakly acidic solution. The…

Q: The pH of a 0.78M solution of benzoic acid (HCH,CO₂) is measured to be 2.15. Calculate the acid…

A: pH of the solution = 2.15 Concentration of benzoic acid (C) = 0.78 MKa of benzoic acid = ?

Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 × 10 0. Calculate the pH of a…

A: The acid dissociation constant for the HCN is = 6.2×10-10 The concentration of HCN solution is = 4.9…

Q: The pH of a 1.0M solution of hydrofluoric acid (HF) is measured to be 1.58. Calculate the acid…

A: pH = -log[H3O+] The expression for dissociation constant of weak acid can be determined from ICE…

Q: The pH of a 1.2M solution of acetic acid (HCH₂CO₂) is measured to be 2.33. Calculate the acid…

Q: predicting the qualitative acid-base properties of salts Consid follow name acetic acid acid…

A: An acid is a species which donates Proton while a base accepts proton. an acid after donating…

Q: The pH of a 0.86M solution of hydrocyanic acid (HCN) is measured to be 4.64. Calculate the acid…

Q: On a shelf in the lab storeroom marked “Solutions of Acids”, a bottle has a torn label. All that can…

A: Acid dissociates in water to form hydrogen ion and it's conjugate base.

Q: The pH of a 0.84M solution of barbituric acid (HC4H₂N₂O3) is measured to be 2.04. Calculate the acid…

A: 1st) Calculate [ H+ ]: 2nd) Construct ICE table :3rd) Calculate Ka:

Q: The acid dissociation constant K, of hypobromous acid (HB1O) is 2.3 x 10. Calculate the pH of a 1.8…

Q: The acid dissociation constant K, of hypobromous acid (HB1O) is 2.3 × 10 Calculate the pH of a 2.0 M…

A: Given: [HBrO] = 2.0 M Ka = 2.3×10-9 The hypobromous acid, HBrO is a weak monoprotic acid,…

Q: The acid dissociation K of acetic acid (HCH3CO2) is 1.8 × 105. -4 Calculate the pH of a 4.1 × 10 M…

A: The objective of this question is to calculate the pH of an acetic acid solution given its molarity…

Q: The acid dissociation constant K of hydrocyanic acid (HCN) is 6.2 × 10 10 a Calculate the pH of a…

Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 × 10¬1º. Calculate the pH of a…

A: Given, initial concentration of HCN = 3.0 M Ka for HCN = 6.2 x 10-10 The hydrocyanic acid…

Q: The acid dissociation constant Ka of alloxanic acid HC4H3N2O5 is ×2.2410−7. Calculate the pH of a…

A: Alloxanic acid is organic weak acid and it dissociates partially into [Alloxanate] and [H3O+].

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

O ACIDS AND BASES
Calculating the Ka of a weak acid from pH
The pH of a 0.94M solution of hydrofluoric acid (HF) is measured to be 1.60.
Calculate the acid dissociation constant K, of hydrofluoric acid. Round your answer to 2 significant
a
K = 0
x10

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

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 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

Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.
. Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar properties (such as the sour taste for acids) of these solutions correspond to their indicated pH?
Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
Write a formula for the conjugate base formed when each of the following behaves as a Brnsted acid: a. HSO3 b. HPO42 c. HClO3 d. CH3NH3+ e. H2C2O4
Arsenic acid (H3AsO4) is a moderately weak triprotic acid. Write equations showing its stepwise dissociation. Which of the three anions formed in these reactions will be the strongest Brnsted base? Which will be the weakest Brnsted base? Explain your answers.
You are asked to determine whether an unknown white solid is acidic or basic. You also need to say whether the acid or base is weak or strong. You are given the molar mass of the solid and told that it is soluble in water. Describe an experiment that you can perform to obtain the desired characteristics of the white solid.
For solutions of the same concentration, as acid strength increases, indicate what happens to each of the following (increases, decreases, or doesnt change). a. [H+] b. pH c. [OH] d. pOH e. Ka
Each box represents an acid solution at equilibrium. Squares represent H+ ions, and circles represent the anion. Water molecules are not shown. Which figure represents a strong acid? Which figure is a weak acid?
Using an acetic acid/sodium acetate buffer solution, what ratio of conjugate base to acid will you need to maintain the pH at 5.00? Describe how you would prepare such a solution.
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.