6. Which of the following is NOT an acid-base conjugate pair? a. HCN and CN- b. H2S and OH c. H2O and OH d. NH3 and NH4* > Answer and brief explanation: 7. Predict the products of the following acid-base reaction: HCI (ag) + NaOH (ag) → a. H30* (ag) + OH b. Na* (ag) + CI (ag) c. NaCl (ag) + H2O d. no reaction takes place Answer and brief explanation:

6. Which of the following is NOT an acid-base conjugate pair? a. HCN and CN- b. H2S and OH c. H2O and OH d. NH3 and NH4* > Answer and brief explanation: 7. Predict the products of the following acid-base reaction: HCI (ag) + NaOH (ag) → a. H30* (ag) + OH b. Na* (ag) + CI (ag) c. NaCl (ag) + H2O d. no reaction takes place Answer and brief explanation:

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter4: Acids And Bases

Section: Chapter Questions

Problem 4.10P: Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow...

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Ammonia, NH3, is a base and will readily accept a proton in accordance with the following reaction: NH3(aq) + H2O <-> NH4+ + OH- ∆G0NH3(ag) = -26.6 kJ/mol ∆G0H2O = -237.1 kJ/mol ∆G0NH4+ = -79.3 kJ/mol ∆G0OH- = -157.2 kJ/mol For NH3 dissolving in water and forming NH4- and OH-, at pH 9.0, [NH3] = 10-5 mol/L, [NH4-] = 10-5 mol/L. Is the reaction at equilibrium? If not, in which direction is the reaction going?
In the following reaction of tetrafluoroboric acid, HBF4, with acetate ion, C2H3O2-, the formation of tetrafluoroborate ion BF4-, and acetic acid, C2H4O2 is favored. HBF4 + C2H3O2- → BF4- + C2H4O2 Which is the weaker base, BF4- or acetate ion?
In calculating pH by ICE method of 0.015 M CH2FCOOH (Ka CH2FCOOH = 2.6 x10-3), the change in CH2FCOOH can not be neglected because. a. Acid Dissociation constant, Ka, has a negative exponent. b. pH is not within +/- pka unit of pka of CH2FCOOH c. initial CH2FCOOH concentration is less than 0.1 M d. dissociation of [CH2FCOOH] will be more than 5% of initial [CH2FCOOH] ----------- To protect corrosion of materials made of iron, the surface of the iron material is electroplated with another metal. Given below information, which metal will be best to “galvanize” the material ? O2 + H2O + 2e- -> 4OH-(aq) .... E0 = 0.401 v Fe2+(g) + 2e- - -> Fe ............ E0 =(-) 0.440 v Cu2+(g) + 2e- - -> Cu ...........E0 = 0.337 v Ni2+(g) + 2e- - -> Ni ............ E0 = (-)0.250 v Zn2+(g) + 2e- - -> Zn ............ E0 =(-) 0.763 v a. Zn b. Ni c. Cu d. Fe2+ ------------ Given : C (s) + H2O(g) <-> CO(g) + H2(g) Which of the following will shift equilibria to form…
If we used H2C4H4O5 as the weak diprotic acid, which of the four species, H2C4H4O5, HC4H4O51-, C4H4O52- or OH1-, will be present in the highest concentrations in a solution at the given pH’s below? If you think any of the above are equal, write the two species that are equal as an equivalence (i.e. H2C4H4O5 = HC4H4O51-). pH = 5 Answer:____________ pH = 8 Answer:____________ pH = 12 Answer:____________
Find the pKa of the acids (or conjugate acids of the given base) below. Then, draw the form that is predominant at pH = 3, 7, 12 for each of the compounds:
For the following reaction, draw the Lewis Dot structure for each reactant and product including any formal charges. Also identify the Lewis Acid and the Lewis Base for this reaction. CH3CH2CCH + NH2- -> CH3CH2CC- + NH3 On the product side of the equation, one of the C atoms has 1 unshared pair of electrons and is (-) charged.
NaHSO3 is a salt, which ionized completely to give HSO3- ion. the following equations show that this ion can act either as an acid or as a base. HSO3- + H2O(l) <=> H3O+ + SO3-2 K1 = ? HSO3- + H2O(l) <=> H2SO3 + OH- K2 = ? (a) Knowing that for H2SO3:Ka1=1.4x10-2, Ka2 = 6.5x10-8, find K1 and K2. (b)Predict which reaction of the two is more important based on their K values. (c) What is the pH of 0.10 M NaHSO3
Write the equations that represent the first and third ionization steps for phosphoric acid (H3PO4) in water. (Use H3O+ instead of H+.) first ionization step: + H2O(l) + third ionization step: + H2O(l) + --- The value of Ka for acetic acid is 1.80×10-5.What is the value of Kb, for its conjugate base, CH3COO-? --- The value of Ka for nitrous acid is 4.50×10-4.What is the value of Kb, for its conjugate base, NO2-?
In reaction D: CuO + H2SO4= CUSO4 + H2O Students will occasionally use HNO3 (aq) instead of H2SO4 (aq) in reaction D, assuming that both strong acids will accomplish the same purpose. Briefly describe the results of this error.
In the reaction NH2- + CH3OH → NH3 + CH3O-, Bronsted would consider NH2- to be the (acid or base?) CH3OH to be the (acid or base?) , NH3 to be the (conjugate acid or conjugate base?) , and CH3O- to be the (conjugate acid or conjugate base?)
For each of the following reactions, highlight or circle the substance on the left hand side which is behaving as an acid and the substance on the right hand side which is its conjugate base. H2O + HCl ➡ H3O+ + Cl- CH3CO2H + OH ➡ CH3CO2- + H2O H2SO4 + HNO3 ➡ HSO4- + H2NO3+ CH3CO2H + HNO3 ➡ CH3CO2H2+ + NO3- Justify each of your choices with concrete explanations.
1.Given : ?? = [?3?+][??−] = 1.0 × 10−14 at 25C . pKw= 14 Which of the following is true ? a.At 25 C, [?3?+] & [??−] would be large in a water solution. b.The pH of an aqueous solution can be determined if [OH-] is provided.c. At 25 C, the pH of water is =14 d.At 25 C, majority of H2O will be dissociated.2.Which of the following is true about the molecule/s and acid strength ? a.HOCl is weaker than HOBr because Cl is more electronegative than Br b.H2SO4 is a strong acid because it has 2 Hydrogens c.CH3CH2OH is a weaker acid than CH3COOH because the negative charge is more dispersed in the conjugate base of CH3COOH.d.HCl is a weaker than HI acid because Cl- ion is more stable than I- ion. 3. Which of the following is true regarding acids and bases? a.All Bronsted-Lowry bases are also considered as Arrhenius bases b.Bronsted-Lowry acids accept protons from Bronsted-Lowry basesc.Lewis bases donate electron pairs to Lewis acids