Concept explainers
(a)
Interpretation:
Whether for the given reaction, the value of
Concept Introduction:
A substance which produces
A substance which produces hydroxide ion when dissolved in aqueous solution is known as a base. These are proton acceptor.
A
The value that defines the relationship between the amount of products and reactants at equilibrium is known as equilibrium constant.
(b)
Interpretation:
Whether the answer in part (a) is consistent with the energy diagram for the reaction should be determined.
Concept Introduction:
A substance which produces
A substance which produces hydroxide ion when dissolved in aqueous solution is known as a base. These are proton acceptor.
A chemical reaction which takes place between an acid and a base is known as acid-base reaction.
The value that defines the relationship between the amount of products and reactants at equilibrium is known as equilibrium constant.
(c)
Interpretation:
Among the following options, the option which describes best the mathematical relationship between
Concept Introduction:
A substance which produces
A substance which produces hydroxide ion when dissolved in aqueous solution is known as a base. These are proton acceptor.
A chemical reaction which takes place between an acid and a base is known as acid-base reaction.
The value that defines the relationship between the amount of products and reactants at equilibrium is known as equilibrium constant.
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Chapter 4 Solutions
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- For 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_forwardFor each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) H2S(aq) + CO32(aq) HS(aq) + HCO3(aq) (b) HCN(aq) + SO42(aq) CN(aq) + HSO4(aq) (c) SO42(aq) + CH3CO2H(aq) HSO4(aq) + CH3CO2(aq)arrow_forwardWhen propionic acid is reacted with sodium hydroxide, as shown below, what can be said about the reaction after equilibrium has been reached? HO, NaOH + H,0 + Na propionic acid sodium hydroxide sodium propionate NaOH = Na® OH %3D O the concentration of propionic acid and sodium propionate are approximately equal the concentration sodium propionate is much greater than the concentration of propionic acid the concentration of propionic acid is much greater than the concentration of sodium propionatearrow_forward
- For the following reaction, K< 1. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. C18H21O3N + C,H;OH=C,H;0" + C18H21O3NH* Clear All C18H2103NH* Stronger Bronsted-Lowry acid Weaker Bronsted-Lowry C,H;O¯ acid C18H21O3N Stronger Bronsted-Lowry base Weaker Bronsted-Lowry C,H;OH basearrow_forward1. The following equilibrium exists when ammonium is dissolved in water: NH4+ (aq) + H2O (l) « H3O+ (aq) + NH3 (aq) The Ka of NH4 is 5.6 x 10-10. Find the pH of a 3.00 M solution of NH4Cl. (hint: since NH4Cl completely ionizes, the concentration of the ammonium ion is 3.00 M) NH4Cl (s)àNH4+ (aq) + Cl- (aq)arrow_forwardWhich direction does the equilibrium below favor and what is the deciding factor? HO H+ cat. NH2 ZIarrow_forward
- Formic acid dissociates reversibly according to the following equation. [ /20] HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.arrow_forwardFor each acid-base reaction shown below, predict whether the equilibrium lies to the left or the right. EtzNH*CI + EtzN + Na* + Cl + PHCO'Na* PHCOH Me4N*OH + MeąN* + H2Oarrow_forwardWhat is the correct equilibrium constant expression for the following reaction? NH3(aq) + H₂O(1) ⇒NH4*(aq) + OH¯(aq) O O (A) Ke (B) Kc (c) Ke (D) Kc (E) Kc - = = = [NH3] [H₂O] [NH4]+[OH]- [NH4+][OH-] [NH3] [NH4+] [OH [NH3] [H₂O] [NH3] [NH₂+] [OH-] 4 [NH₁+OH [NH3]arrow_forward
- Imagine that 500 mL of a 0.100 M solution of HOAc(aq) is prepared. What will be the [OAc–] at equilibrium in this solution if the acid dissociation constant Ka(HOAc) = 1.79 x 10–5? a. 1.33 x 10–3 M b. 4.23 x 10–3 M c. 9.46 x 10–4 M d. 0.100 M e. not enough information to tellarrow_forwardConsider the following chemical equilibrium: HCOO¯¯ (aq) + H₂O(aq) = HCOOH(aq) + OH¯(aq). Which of the following graphs represents the perturbation on the system and the change of pH when HCI is added to the container? | pH time || III pH ↑ time Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. C Q a || = III = d IV pH IV pH time time K Open Χ Your answerarrow_forwardThe equilibrium concentrations for a solution of the acid HA are [HA]=2.16 M, [A−]=0.0173 M, and [H3O+]=4.32×10−3 M. What is the Ka for this acid? Report your answer in scientific notation. Your answer should have three significant figures.arrow_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 & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
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