LE CHÂTELIER'S PRINCIPLE
Consider this reaction at equilibrium.
Predict the effect (shift right, shift left, or no effect) of these changes.
(a) addingNaOH to the reaction mixture
(b) addingHCl to the reaction mixture
(c) addingXe to the reaction mixture
(d) removingXe from the reaction mixture
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
INTRO CHEMISTRY PKG
- 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.arrow_forwardFor each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) NH4+(aq) + Br(aq) NH3(aq) + HBr(aq) (b) HPO42(aq) + CH3CO2(aq) PO43(aq) + CH3CO2H(aq) (c)[Fe(H2O)6]3+(aq) + HCO3(aq) [Fe(H2O)5(OH)]2+(aq) + H2CO3(aq)arrow_forwardThe pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107arrow_forward
- Describe any thermochemical (heat of reaction) evidence for the Arrhenius concept.arrow_forwardUse 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.arrow_forwardWrite a balanced molecular equation for the preparation of each of the following salts, using an acidbase neutralization reaction. a. LiNO3 (lithium nitrate) b. BaCl2 (barium chloride) c. K3PO4 (potassium phosphate) d. Na2SO4 (sodium sulfate)arrow_forward
- Identify the products formed in this Brønsted-Lowry reaction. HCO−3+NO−2↽−−⇀acid+basearrow_forwardHydrazoic 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.arrow_forwardCalculate the value of K eq given the following equilibrium conditions. CH 4 = 0.10M O 2 = 0.20M CO 2 = 1.5M H 2 O = 3.0Marrow_forward
- Boric acid, BOH is used as a mild antiseptic. What is the PH of a 0.025 aqueous solution of boric acid? What is the degree of ionisation of boric acid in this solution? The hydrogen ion arises principally from the reaction: B(OH)3(aq) + H2O(l) > B(OH)4- (aq) + H+ (aq) The equilibrium constant for the reaction is 5.9 x10-10arrow_forwardFor the following chemical reaction, identify the acid, the base, and the conjugate acid and conjugate base. H2O(l) + ClO1-(aq) ⇄ HClO(aq) + OH-(aq) Brønsted-Lowry acid = Brønsted-Lowry base= HClO(aq) is the conjugate of .OH-(aq) is the conjugate of .arrow_forwardConsider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2(aq) + H2O (l) <====> H3O+(aq) + NO2-(aq) In which direction will the equilibrium shift if NaOH is added? NaNO2 is added ? HCl is added? The acid solution is made more dilute ?arrow_forward
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningGeneral, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning