Concept explainers
(a)
To determine:
Write chemical equations and equilibrium expressions for the reactions for acetic acid with water.
(a)
Explanation of Solution
Rate of equilibrium expression
In this equilibrium, water is pure liquid and its concentration is constant which is called acid dissociation constant
So, final concentration of product
(b)
To determine:
Write chemical equations and equilibrium expressions for the reactions for ethanoic acid and water.
(b)
Explanation of Solution
The given expression is expressed below.
Rate of constant
In this equilibrium water is pure liquid and its concentration is constant so,
(c)
To determine:
Write chemical equation and equilibrium expressions for the reactions of hydrogen fluoride acid and water.
(c)
Explanation of Solution
Equilibrium rate constant
Here, water is a pure is a pure liquid and its concentration is constant.
Arranging the equation, you get
(d)
To determine:
Write chemical equations and equilibrium expressions for the reactions for hydrogen fluoride acid and water.
(d)
Explanation of Solution
Rate constant of equilibrium reaction
Here water is pure liquid and its concentration is constant
Then, it is called dissociation constant.
Arranging the equation you get
(e)
To determine:
Write chemical equation and equilibrium expressions for the reactions of carbonic acid and water.
Explanation of Solution
Rate of equilibrium constant
In this equilibrium water is pure liquid and its concentration is constant
So, dissociation constant
Arranging the equation, you get.
Hence, all the parts have been described.
Want to see more full solutions like this?
Chapter 12 Solutions
Chemistry for Engineering Students
- 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 ionarrow_forwardAcrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?arrow_forwardGiven the following solutions: (1) 0.025 M NaOH (2) 0. 025 M NH3, Kb (NH3)= 1.75 x 10-10 (3) 0.025 M NH4Cl i) Is the solution acidic, basic, and neutral? Write the equations involved when each of the solutes are dissolved in aqueous solutions to justify your answer. ii) Write the equilibrium expression if any, use appropriate symbol for the equilibrium constant. iii) Calculate the pH of each. Show your calculation. You may use shortcuts.arrow_forward
- Question 15.24arrow_forwardThe solubility (denoted as s) of CaSO4 in pure water at 40o C is 1.09 grams per liter. What is the value of the solubility product of CaSO4?arrow_forward(7) Calculate the pH of each of the following solutions: (a) 0.1000M Propanoic acid( HC H O,,K=1.3x105) (b) 0.1000M sodium propanoate (Na C HỎ) (c) 0.1000M HC₂H₂O, and 0.1000M Nа С¸¸0₂ 3 5 52 (d) After 0.020 mol of HCl is added to 1.00 L solution of (a) and (b) above. (e) After 0.020 mol of NaOH is added to 1.00 L solution of (a) and (b) above.arrow_forward
- Write the ionic equation for the dissolution and the solubility product expression for each of the following slightly soluble ionic compounds:(a) AgI, silver iodide, a solid with antiseptic properties(b) CaCO3, calcium carbonate, the active ingredient in many over-the-counter chewable antacids(c) Mg(OH)2, magnesium hydroxide, the active ingredient in Milk of Magnesia(d) Mg(NH4)PO4, magnesium ammonium phosphate, an essentially insoluble substance used in tests for magnesium(e) Ca5(PO4)3OH, the mineral apatite, a source of phosphate for fertilizersarrow_forwardYou are asked to prepare a pH = 3.00 buffer solution startingfrom 1.25 L of a 1.00 M solution of hydrofluoric acid(HF) and any amount you need of sodium fluoride (NaF).(a) What is the pH of the hydrofluoric acid solution priorto adding sodium fluoride? (b) How many grams of sodiumfluoride should be added to prepare the buffer solution?Neglect the small volume change that occurs when the sodiumfluoride is added.arrow_forward8. Our bodies are able to preserve a near constant pH due to the presence of hydrogen carbonate anion (HCO,). K values for the diprotic acid carbonic acid (H,CO;) are Kaj = 4.5 x 10?, K2 = 4.7 x 10-". a) Hydrogen carbonate anion is an amphoteric species. Define amphoteric. b) In the space below, write out chemical equations to describe the behavior of this species as both a Bronsted acid and a Bronsted base, and use the equilibrium constants given above to decipher whether a solution of HCO;¯ will be acidic, basic, or neutral. Support your answer with pertinent calculations.arrow_forward
- A buffer is prepared by adding 5.0 g of ammonia, NH3, and 20.0 g of ammonium chloride, NH4Cl, to enough water to form 2.50 L of solution. (a) What is the pH of the buffer? (b) Write the complete ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. (c) Write the complete ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer.arrow_forwardChemical Equilibriaarrow_forwardACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called Xcitingpartic acid (HXp). She prepared a solution of the weak acid by diluting 2.7 ml of 0.20 M HXp with 19.3 mlL of water. Upon measuring the conductivity of the solution and a blank, she obtained 205.0 µS/cm and 2.0 uS/cm, respectively. She also measured the pH of the solution and got a pH of 3.49. Help her find the following: 1. Concentration of the weak acid (HXp) after dilution 2. Corrected conductivity 3. Molar conductivity of the solution 4. Equilibrium concentration of H30, and Xp 5. a 6. Equilibrium concentration of the weak acid (HXp) 7. K, 8. Aoarrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning