The fluoride ion is the conjugate base of the weak acid hydrofluoric acid.The value of K, for F, is 1.39x1011.Write the equation for the reaction that goes with this equilibrium constant.+

Answered: Image /qna-images/answer/a05cf69d-620e-49d4-b1b9-13eed16474bb.jpg

Answered: The fluoride ion is the conjugate base…

The fluoride ion is the conjugate base of the weak acid hydrofluoric acid. The value of K, for F", is 1.39×10-11. Write the equation for the reaction that goes with this equilibrium constant. +

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section12.2: The Equilibrium Constant

Problem 12.2PSP: When carbon dioxide dissolves in water it reacts to produce carbonic acid, H2CO3(aq), which can...

See similar textbooks

Related questions

Q: The hypochlorite ion, ClO-, acts as a weak base. When ClO- acts as a base, which atom, Cl or O, acts…

A: To know which is the proton acceptor we see the valancy of the Cl and the O. In O there is two…

Q: Determine the pH of each solution and classify it as acidic,basic, or neutral.(a) pOH = 8.5(b) pOH =…

A: We have four solution of pOH = 8.5, pOH = 4.2,pOH = 1,pOH = 7.0 . We have to calculate pH of each…

Q: C. Complete the table: Acidic, basic, neutral [H;O'] [OH] pH 1.0 x 106 3.00 2.8 x 105M Neutral D.…

Q: What is the equilibrium constant of the HSO4-ion, if [H3O+] = 0.027 M; [HSO−4] =0.29 M; and [SO2−4]…

A: The Complete and balanced chemical equation is given as,

Q: What will be the products when ammonia reacts with hydrofluoric acid? In the reaction, identify the…

A: Balanced chemical equation: NH3 + HF → NH4+ + F-…

Q: Write the formula of the conjugate acid of CH3CO2H

A: We have to tell the conjugate acid of CH3COOH

Q: Write the net ionic equation for the hydrolysis reaction that occurs when sodium carbonate, Na,CO3…

A: When sodium carbonate is made to react with water, it gives sodium bicarbonate and sodium…

Q: Determine the equilibrium constant for the following reaction, CH3COOH(aq) +F(aq) CH3COO (aq)+…

A: weak acid are those acid which does not dissociate completely to furnish H+ ion Given dissociation…

Q: Write a balanced equation for the acid–base reaction thatleads to the production of each of the…

A: Neutralization Reaction : It is a reaction in which acids react with Base to form salt & water.…

Q: Malonic acid, H,C,H,O,(aq), is a diprotic acid, so 2 moles of hydroxide ions are required per HIUIU…

Q: A 0.54 M solution of chloroacetic acid, CICH2 CO2H, has a pH of 1.57. Calculate K, for the acid. %3D

A: Given: The molarity of the solution of chloroacetic acid = 0.54 M The pH of the solution = 1.57 We…

Q: 5. Write the chemical formula of the conjugate base of boric acid.

A: Given: To determine the chemical formula of the conjugate base of boric acid.

Q: Write the formula of the conjugate acid of the Brønsted-Lowry base, H,PO,

A: Acids and bases are classified by help of different type of concepts or theories , like - Arrhenius…

Q: What are the conjugate base and conjugate acid for HSO4−? What is the term used to describe species…

A: The term conjugate acid can be defined as the compound which gets formed when and acid reacts with…

Q: Given the reaction: NH 4 + + C 3H 5O 2 ↔ NH 3 + HC 3H 5O 2, the Bronsted-Lowry base in the reverse…

A: Acid Base theories: Three theories exist: 1. The Lewis acid-base theory: The compounds which can…

Q: Calculate the pH of the following solutions: a. 2.0 M morphine hydrochloride, C,„H,„NO,•HCI (pK, =…

A: In order to solve this question, we will be using simple concepts of chemical and ionic equilibrium.…

Q: Determine the pH of each solution and classify it as acidic, basic, or neutral. (a) pOH = 8.5 (b)…

Q: Write the formula of the conjugate acid of the Brønsted-Lowry base, H₂PO₄⁻

Q: Oxalic acid, H2C2O4 , is a diprotic acid. Write a chemical equilibrium expression for each…

A: The chemical equilibrium expression for each ionization step has to be written.

Q: Write an ionic equation to represent the hydrolysis of the pyridinium ion, and calculate the pH of…

A: given concentration of C5H5NH+Cl- = 0.0482 M Kb for prydine = 1.7× 10-9 Ka = Kw /Ka Kw =…

Q: The value of K, for hypochlorous acid , HCIO , is 3.50x10-8. Write the equation for the reaction…

A: Equilibrium reaction of HClO, HClO(aq) + H2O(l) -------> ClO-(aq) + H3O+(aq)

Q: Boric acid dissolves in water according to the equation B(OH)3(aq) + H₂O → B(OH)2 (aq) + H+ (aq)…

Q: 4. HCO 3 +H O2 Acid: Base: CA: CB:

A: Acid is a substance that is able of donating a H+ ion. Base can abstract the proton from an acid.…

Q: What is the equilibrium constant for the following acid-base reactions? a) fluoride ion and acetic…

A: part a :-

Q: Nitric acid reacts with ammonia to yield ammonium nitrate. Write the reaction and identify the acid,…

A: Given here, Nitric acid reacts with ammonia to yield ammonium nitrate and we are asked to write the…

Q: Write the formula of the conjugate acid of the Bronsted-Lowry base, HONH2

A: Conjugate acids are formed when a proton is added to the Bronsted-Lowry base Hence the molecule or…

Q: Write the Ka (acid ionization equilibrium constant) expression for the ionization of HC3H5O2 in…

A: Let us consider a general reaction for the ionization of an acid HA in water. HA (aq) ↔ H+(aq) +…

Q: Predict the products of the following acid-base reaction. Identify and label the conjugate acid /…

A: Complete the given reaction and identify acid-base pairs ----

Q: Write a balanced equation for the proton transfer reaction between hydrofluoric acid (HF) and…

A: An acid and a base that differs by a single proton are conjugate to one another and form a conjugate…

Q: Calculate the pH of a sample of 1.5 M CH3COOH.

A: Given :- molar concentration of acetic acid = 1.5 M To calculate :- pH

Q: Assuming 0.1 M concentrations, arrange the following acid solutions in order of increasing pH.…

A: Concentration of each given acid = 0.1 M (c) We know that -> [H+] = √(Ka ×c)

Q: 8. The compound Mg(OH)2 is classified as an Arrhenius base because, when dissolved in water, there…

A: According to the Arrhenius theory, the substance that gives hydrogen ion H+ in the aqueous solution…

Q: Write the formula of the conjugate acid of the Brønsted-Lowry base caffeine, CSH10N4O2

A: Given that, Bronsted -Lowry base = C8H10N4O2 Conjugate acid = ?

Q: Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when…

A: When a salt is dissolved in water, it will changed into their related acids and bases. Also the…

Q: Write the equation for reaction of hydrofluoric acid and its conjugate base, fluoride ion with…

Q: Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when…

Q: Write the equilibrium for the autoionization of sulfuric acids (H 2 SO 4 ) and write the expression…

A: Equilibrium expression for autoionisation of sulphuric acid

Q: Fill in the left side of this equilibrium constant equation for the reaction of dimethylamine ((CH,)…

A: The weak base given is (CH3)2NH Since weak base reacts with water to produce conjugate acid and…

Q: When hydrogen chloride reacts with ammonia ammonia chloride is formed. write the equation for this…

Q: The acetate ion is the conjugate base of the weak acid acetic acid. The value of K, for CH3C00", is…

A: Here Kb is given for acetate ion so reaction start with acetate ion

Q: What is the pH of a substance with a hydrogen ion concentration of 1.0 x 10-8 M?

A: Consider the given information is as follows: Concentration of hydrogen ion = 1.0×10-8 M pH = ?

Q: Fill in the left side of this equilibrium constant equation for the reaction of diethylmethylamine…

Q: The Kb of hydrazine is 9.1 x 10-7. If 3.12 x 10-3 mol of hydrazine is added to water to make up…

A: Hydrazine (N2H4) is a weak base Concentration of hydrazine is calculated as follows,

Q: Fill in the left side of this equilibrium constant equation for the reaction of ammonia (NH,), a…

A: From given Initially we are giving reaction of ammonia with water and Kb is calculated and the…

Q: The fluoride ion is the conjugate base of the weak acid hydrofluoric acid. The value of K, for F, is…

Q: Define the process of drawing the products of a Brønsted–Lowry acid–base reaction ?

A: Given: Bronsted-Lowry acid-base reaction

Q: 0.0500 M HF (Ka= 7.20 x 10–4) determine the quilibrium molar concentration of H3O+, equilibrium…

Q: A 0.05 molar acidic solution has an ionization constant of 2.50 x 10-5 , what is the concentration…

A: Leta consider Acid is a monoprotic Acid Ionisation constant = 2.50 × 10-5Concentration of Acid =…

Q: Determine the pH of a 0.068 M aqueous solution of sodium cyanide. The Ka for HCN is 4.9x 10^-10

Question

The fluoride ion is the conjugate base of the weak acid hydrofluoric acid.
The value of K, for F, is 1.39x1011.
Write the equation for the reaction that goes with this equilibrium constant.
+

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

Trending now

This is a popular solution!

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

Write the equilibrium constant expression for each of the following reactions in terms of concentrations. (a) CO2(g) + C(s) 2 CO(g) (b) [Cu(NH3)4)2+(aq) Cu2+(aq) + 4 NH3(aq) (c) CH3CO2H(aq) + H2O() CH3CO2(aq) + H3O+(aq)
Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion
The active ingredient of Pepto-Bismol is the compound bismuth subsalicylate, which undergoes the following dissociation when added to water: C7H5BiO4(s)+H2O(l)C7H4O32(aq)+Bi3+(aq)+OH(aq)K=? If the maximum amount of bismuth subsalicylate that reacts by this reaction is 3.2 1019 mol/L, calculate the equilibrium constant for the preceding reaction.
For an acid-base reaction, what is the reacting species (the ion or molecule that appears in the chemical equation) in the following bases? (a) barium hydroxide (b) trimethylamine (CH3)3N (c) aniline, C6H5NH2 (d) sodium hydroxide
When carbon dioxide dissolves in water it reacts to produce carbonic acid, H2CO3(aq), which can ionize in two steps. H2CO3(aq)HCO3(aq)+H+(aq)Kc1=4.2107HCO3(aq)CO32(aq)+H+(aq)Kc2=4.81011 Calculate the equilibrium constant for the reaction H2CO3(aq)CO32(aq)+2H+(aq)
You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.
The equilibrium expression for any weak acid can be written as HA (aq) + H20 (1) = A- (aq) + H;O+ (aq) 1. Write the K value expression based on the equation above (remember that pure liquids are not included in the K expression). This is given the special symbol Ka. 2. In this experiment, you will be using pH to find [H3O+]. The relationship is [H3O*] = 10-PH . For a pH of 7.4, find the [H3O+].
Write the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 HF (aq) + H20(1) H30+(aq) + F (aq) K =
Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HF (aq) + OH- (aq)F- (aq) + H2O (l) K =
Hydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5. Calculate the equilibrium concentrations of all substances if the initial concentration of HN3 is 0.0750 M. Determine the pH of the solution. Would a 0.0750 M solution of HBr have a higher or lower pH than the 0.0750 M HN3 solution? Explain why.
Write the equilibrium constant expression for this reaction: 2H (aq)+So (aq) → H,SO,(aq)