Answered: The value of Ka for benzoic acid ,…

The value of Ka for benzoic acid , CgH3COOH , is 6.30×10° . Write the equation for the reaction that goes with this equilibrium constan (Use H3O* instead of H*.)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 82AP

See similar textbooks

Related questions

Q: A solution of benzoic acid (HC7H5O2) is 14.2 percent ionized. Calculate the equilibrium…

A: Benzoic acid is a monoprotic weak acid. Benzoic acid HC7H5O2 dissociates into: HC7H5O2⇌H++C7H5O2…

Q: Methylamine is added to water to make a 0.050 M solution. What is the pHat equilibrium? The Kb for…

Q: 4. The acid dissociation constant Ka equals 1.26 x 102 for HSO4 and is 5.6 x 10-10 for NH4. Which…

A: Form the given information it is confirmed that HSO4- is a stronger acid than NH4+ since, its pKa…

Q: Write the equilibrium expression for a simple acid ionization. (HA (aq) -> H+ + A-

A: the equilibrium expression for a simple acid ionization. HA (aq) ----------> H+ + A- equilibrium…

Q: For 6 and 7, use the table of K, values compiled at 25 °C to answer the questions below: Acid HNO,…

A: Acid is substance which release hydrogen ions and base is substance which release hydroxyl ions when…

Q: At equilibrium, the value of [H+] in a 0.260M solution of an unknown acid is 0.00418M . Determine…

A: For acid HA, the acid dissociation constant Ka can be written as:

Q: The value of Ka for phenol (a weak acid) , C,H5OH , is 1.00×10-10 . Write the equation for the…

A: Phenol acts as a weak base that means the hydrogen attached to -OH group in phenol is removed as a…

Q: CoHsOH(ag) + H2O0 → CaHsO(aq) + H3O*@g K= 1.12 x 1010 (a) Phenol is a weak acid that partially…

A: Since you have asked a question with multiple parts, we are solving first three parts for you. For…

Q: The compound ammonia, NH3, is a weak base when dissolved in water. Write the K, expression for the…

A: The answer to the following question is given as:

Q: Write the equilibrium expression for water’s self-ionization. What are the [H+], pH and pOH for pure…

A: The equilibrium expression for self ionization of water is : or Equilibrium constant: pH…

Q: The compound dimethylamine, (CH3),NH, is a weak base when dissolved in water. Write the K expression…

A: The ionization of weak base can be given by, Where B is the weak base and HB+ is its conjugate…

Q: For the equilibrium, HSO4 + HPO4²SO4+H₂PO4 a conjugated Brönsted-Lowry acid-base pair is: HPO4…

A: Explanation :

Q: For 6 and 7, use the table of K, values compiled at 25 °C to answer the questions below: Acid HNO,…

A: This question is related to acid-base concept. Acids are species which can lose a proton while…

Q: The value of Ka for hypochlorous acid , HClO , is 3.50×10-8 . Write the equation for the reaction…

A: HClO(aq) + H2O(l) H3O+(aq) + ClO-(aq) Ka = [H3O+] [ClO-]/[HClO][H2O]

Q: FeCl3 + NH4SCN = Fe(SCN)+2 + 2Cl-1 + NH4Cl1) If I add FeCl3, would the equilibrium shift right or…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: In the laboratory, a general chemistry student measured the pH of a 0.474 M aqueous solution of…

Q: Write the Ka expression for the following reaction HF ->

A: Acid dissociation constant is expressed by Ka Greater is the value of Ka more is the acidity of the…

Q: 2 H, + ½ Cl, Na + H,0 = Na + 2 Cl, HCI K = 1.00x105 NaOH + ½ H, K = 1.00x10-2 K = 1.00x107 2 NaCI…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: The value of K, for benzoic acid , C¿H¿CcOOH , is 6.30x10-5. Write the equation for the reaction…

Q: Write the balanced chemical equation for the reaction of the weak acid HCN with water. Include the…

Q: The pH of a (1.7300x10^-1) molar solution of an aqueous weak acid (HA) is (1.99x10^0). The Ka for…

A: PHis defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: Given the chemical equation HCl + NaOH ----> H2O + NaCl How would the calculated concentration…

A: Molarity of a solution depends on volume. As the volume of the solution increases, molarity…

Q: Calculate the H,O" concentration in a solution of acetic acid if the concentration of molecular…

A: If we assume the concentration of H3O+ and CH3COO- ions is x then - CH3COOH H3O+ CH3COO- I…

Q: 6. Write the Ka expression for an aqueous solution of acetic acid , CH3COOH : Ka =

Q: If NH4OH at 30.0 °C is 1.20 % ionized is 0.250 M solution, what is its ionization constant and the %…

A: Ionisation constant is also known as equilibrium constant Which is equal to the ration of…

Q: You have 70 ml of 0.1 M HA, after adding 30.0 ml of 0.1 M NAOH, the pH is 5.0 what is the Ka of HA?…

A: We are given an Acid HA and a base NaOH. We have to find the ka of the acid. We are also given the…

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

Q: The kidneys function to help maintain blood pH. In one process they convert CO2 in the blood into…

Q: 7. The ka for acetic acid is 1.0 x 10.5. Is acetic acid a weak or a strong acid?

A: Strong acids completely dissociate in aqueous solution (Ka > 1, pKa < 1).

Q: The [H,O'] is 3.39 × 10“M for an unknown acid HA. Write the expression for K, for this acid based on…

Q: Write out the chemical reaction for the dissociation of acetic acid, CH3COOH, in water and…

A: Weak acids do not dissociate strongly in water.

Q: Write an equation for the ionizations of carbonic acid

A: Carbonic acid is a diprotic acid as it has two replaceable protons.

Q: The value of Ka for acetic acid, CH3COOH, is 1.80x10^-5 Write the equation for the reaction that…

A: The value of Ka for acetic acid, CH3COOH, is 1.80x10-5 Write the equation for the reaction that…

Q: For 6 and 7, use the table of K, values compiled at 25 °C to answer the questions below: cid HNO,…

A: Acid can be defined as the species that donate hydrogen ions in aqueous solution and base is a…

Q: Consider a hypothetical acid-base indicator, "HX", ionizes in water according to the equation HX(aq)…

A: HX(aq) <----> H+(aq) + X-(aq)

Q: At equilibrium, the value of [H+] in a 0.260M solution of an unknown acid is 0.00405M . Determine…

A: Given: Equilibrium concentration of H+ ion = 0.00405 M Initial concentration of acid = 0.260 M

Q: 4) For the following acids, write the reaction for the acid ionizing in water. Write the Ka…

Q: A 0.11 M solution of weak acid, HA, has a pH of 5.08. a. Write the dissociation reaction of the acid…

A: The dissociation reaction of acid in water is represented as

Q: 2. Write the equilibrium reaction (with water) of the following compounds and their corresponding…

A: Equilibrium can be defined as a state of reaction at which rate of forward reaction become equal to…

Q: acid, Ka = 7. The value of Ka for acetylsalicylic acid (aspirin) is 3.00x10-4. What is the value of…

Q: 35. In each reaction, identify the Brønsted-Lowry acid, the Brønsted- Lowry base, the conjugate…

Q: Hydrocyanic acid has a Ka value of 4.9 x 10-10. If the initial concentration of HCN is 0.432 M…

A: For a weak acid: [H+] = (Ka x C)1/2 Where, C = molar concentration of acid pH = -log[H+] pOH = 14 -…

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: The Keq for the reaction: A + B ↔ AB is 2.03 What is the Keq for AB ↔ A + B Keq = ?

A: The equilibrium constant, Keq for the reaction: A + B ⇌ AB is 2.03 The equilibrium constant, Keq…

Q: Q10. Blood pH is controlled by the carbon dioxide-bicarbonate buffer system. CO₂ (g) + H₂O (L) H*…

A: #Q.10: While running long distances, the metabolic activities of the body increase leading to…

Q: Problem attached

Q: 9. A base is added to water and a new equilibrium is established. The new equilibriu described by A.…

A: In the pure water pH and POH both are same

Q: Use the The value of K, for hypochlorous acid, HCIO.s 3.50×10 Write the equation for the reaction…

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

The value of K, for benzoic acid , C,H3COOH , is 6.30×105.
Write the equation for the reaction that goes with this equilibrium constant.
(Use H30* instead of H*.)
+

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 1 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

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.
Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the amount of ammonia at equilibrium be affected by 1. removing O2(g)? 2. adding N2(g)? 3. adding water? 4. expanding the container at constant pressure? 5. increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
Dissolving CaCO3 is an endothermic reaction. The following five graphs represent an experiment done on CaCO3. Match the experiment to the graph. (a) HCl is added. (b) The temperature is increased. (c) CaCl2 is added. (d) NaCl is added.
Use Le Chátelier's principle to explain what happens to the equilibrium H2O(l)H+(aq)+OH(aq) when a few drops of HCl are added to pure water.
Vinegar (chemical name : acetic acid, CH3COOH) is a weak acid. Consider the ionization of acetic acid in water. CH3COOH(aq) = H*(aq) + CH3COO (aq) Kc=6.80 ×10-4 If the initial concentration of acetic acid is 0.150 M. What is the concentration of hydrogen ions (H*) at equilibrium? O 0.0100 M O 0.0500 M O 0.100 M O 0.500 M
The value of K, for phenol (a weak acid), C,H3OH , is 1.00×1010. Write the equation for the reaction that goes with this equilibrium constant. (Use H30* instead of H".)
The value of K, for methylamine, CH3NH2, is 4.20×10-4. Write the equation for the reaction that goes with this equilibrium constant.
1&2. Write the expression for Kc (equilibrium constant) for the following reactions.
The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25 degrees celsius of 1.8 x 10-5. CH3COOH(aq) ⇋ CH3COO-(aq) + H+(aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H + for the reaction.
The value of Kh for methylamine, CH2NH,, is 4.20×10-4. Write the equation for the reaction that goes with this equilibrium constant. +
Be sure to answer all parts. Consider the formation of ammonia in two experiments. (a) To a 1.00-L container at 727°C, 1.30 mol of N₂ and 1.65 mol of H₂ are added. At equilibrium, 0.100 mol of NH3 is present. Calculate the equilibrium concentrations of N₂ and H₂ and find Ke for the reaction: [N₂ leq = [H₂ leq 2 NH3(g) = N₂(g) + 3 H₂(g) Kc = ㅈ = M Kc = (b) In a different 1.00-L container at the same temperature, equilibrium is established with -2 8.34 × 10² mol of NH3, 1.50 mol of N2, and 1.25 mol of H₂ present. Calculate Ke for the reaction: M 3 NH3(g) = N₂(g) + H₂(g) 2 2 C C < Prev *********** 18 of 20 MacBook Pro Search or type URL Next *********** ☆