Concept explainers
Interpretation:
The products of the given acid–base reactions are to be predicted and, in each case, the stronger acid, the stronger base, the weaker acid, and the weaker base are to be labeled.
Concept introduction:
Substitution reaction: A reaction in which one of the hydrogen atoms of a hydrocarbon, or a
Elimination reaction: A reaction in which two substituent groups are detached and a double bond is formed is called elimination reaction.
Addition reaction: It is the reaction in which unsaturated bonds are converted to saturated molecules by addition of molecules.
Sodium amide is a strong base that helps in the removal of terminal hydrogen of
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Organic Chemistry
- Calculate the equilibrium constant for the acid–base reaction between the reactants in each of the following pairs: (a) HCl + H2O (b) CH3COOH + H2O (c) CH3NH2 + H2O (d) CH3N+H3 + H2Oarrow_forward4, . Consider the following equilibrium: base + -H H-Base Which of the following base(s) would favour the product in this reaction? Он CH;O NH3 NH2 CH3CO2 (1) (II) (III) (IV) (V) (a) | (b) IV (c) I, IV and V (d) I and II (e) IIl and IVarrow_forward4. A student has prepared 0.05 M solution of CH3-C=CH and has added to it 0.05 M solution of potassium tert-butoxide (K" O-C(CH3)3). (i) Write the equation for the acid-base reaction that might occur. (ii) With curved arrows track the movements of electron pairs. (iii) Assign Base, Acid, Conjugate acid for the base, Conjugate base for the acid. (iv) Calculate the percentage of deprotonated methyl acetylene taking into account that pKa of the conjugate acid of potassium tert-butoxide equals 18 and pKa of methyl acetylene equals 24.arrow_forward
- For the Brønsted acid-base reaction shown below, determine the conjugate acid- base pairs. Then give the curved-arrow notation for the reaction in the left-to-right direction :0: :O: Нзс- H–Ö-H -> Нзс A D Fill in the blanks with the letters A,B,C, and D, representing the species in the reaction above. (It doesn't matter which pair you list first.) Pair 1: Pair 2: acid and its conjugate base acid and its conjugate basearrow_forwardIf the G for a reaction is 4.5 kcal/mol at 298 K, what is the Keq for this reaction? What is the change in entropy of this reaction if H = 3.2 kcal/mol?arrow_forward5. (a) The molecule shown below can react with a base, and lose one of the five protons to form an anionic intermediate. Draw this anionic intermediate, and explain why that proton is removed instead of one of the others. CI H Cl -H H H Cl (b) The same molecule can react with Ag", and lose one of the three chlorine atoms to form a cationic intermediate. Draw this cationic intermediate, and explain why that chlorine atom is removed, while neither of the other two are removed. CI H Cl -H H H H CIarrow_forward
- What 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_forward3.27 For each pair of structures below, identify the stronger acid, and explain your choice: H H N=H -N H H H (a) (c) H -" :0 H ΝΞΗ I H ΗΘΗ `N' H CONTA ΘΝ H (b) (d) H H H N H I Harrow_forwardPredict the products of the following acid-base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow: (a) O2-(aq) + H2O(l)<---> (b) CH3COOH(aq) + HS-(aq)<---> (c) NO2-(aq) + H2O(l)<--->arrow_forward
- (b) What will happen if acetic acid (HC2H3O2) is added to water? O An equilibrium will form between its molecular form, HC2H3O2, and the species formed by removal of water, C2H2O. O An equilibrium will form between its molecular form, HC2H3O2, and the species formed by addition of water, H3C2H3O3. O Acetic acid is a strong acid and will ionize completely. O An equilibrium will form between its molecular form, HC2H3O2, and the ionized form, H* and C2H3O2. O Acetic acid is a weak acid and will not ionize completely. Hint Attempts: 1 of 15 used Submit Save for Later TIng I aI system, SOme of UIS energy Can De transieIICU To une su t ST國 ост 15 MacBook Airarrow_forwardLiquid ammonia (anhydrous NH3(l)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton: 2NH3 NH4+ + NH2- K = 1×10-33 at -50°C Since ammonia is better proton acceptor than water, the ionization of acids is relatively enhanced in liquid ammonia. For example, acetic acid is a strong acid in liquid ammonia. a) Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C. b) Calculate [NH4+] (mol/L) in a 6.29×10-2 M solution of acetic acid in liquid ammonia at -50°C. c) Estimate [NH2-] (mol/L) in a 6.29×10-2 M solution of acetic acid in liquid ammonia at -50°C.arrow_forward(a) Ionic Solids do not dissolve in non-polar solvents. (TRUE OR FALSE) (b) H3AsO4 is a weak acid. (TRUE OR FALSE) (c) Once a chemical reaction has come to equilibrium, the reaction comes to a complete halt.(TRUE OR FALSE)arrow_forward
- Organic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning