Concept explainers
(a)
Interpretation:
The stronger acid among
Concept introduction:
Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.
If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.
If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.
Electronegativity depends on the acidity of a species. The species having high electronegativity is a weak acid.
(b)
Interpretation:
The stronger acid among
Concept introduction:
Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.
If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.
If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.
Electronegativity depends on the acidity of a species. The species having high electronegativity is a weak acid.
(c)
Interpretation:
The stronger acid among
Concept introduction:
Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.
If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.
If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.
Electronegativity depends on the acidity of a species. The species having high electronegativity is a weak acid.
(d)
Interpretation:
The stronger acid among
Concept introduction:
Electronegativity: The chemical behavior of an atom where it attracts the shared electron pair to itself. Down the group, electronegativity decreases as the number of energy levels increases.
If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.
If an acid lose one proton, then the formed species is a conjugated base. Weak base forms stronger conjugated acid.
Electronegativity depends on the acidity of a species. The species having high electronegativity is a weak acid.
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Organic Chemistry
- Which is a stronger base? a. HS− or HO− b. CH3O− or CH3NH c. CH3OH or CH3O d. Cl− or Br− e. CH3COO− or CF3COO− f. CH3CHClCOO− or CH3CHBrCOO−arrow_forwardPredict the stronger acid in each pair: (a) HNO3 or HNO2;(b) H2S or H2O; (c) H2SO4 or H2SeO4; (d) CH3COOH or CCl3COOH.arrow_forwardWhat is the conjugate base of HSO4- is ???? a. SO4 2- b. H2SO4 c. H3O+ d. None correctarrow_forward
- 16.What is the conjugate acid of NH3? Select one:a. NH2+b. NH3c. NH4+d. NH3+arrow_forwardWhich is a stronger base?a. HS− or HO− b. CH3O− or CH3N-H c. CH3OH or CH3O− d. Cl− or Br−e. CH3COO− or CF3COO− f. CH3CHClCOO− or CH3CHBrCOO−arrow_forwardWhich is the stronger base? a. Br− or I− b. CH3O− or CH3S− c. CH3CH2O− or CH3COO− d. H2C CH or HC C− e. FCH2CH2COO− or BrCH2CH2COO− f. ClCH2CH2O− or Cl2CHCH2O−arrow_forward
- Why is H2SO4 a weaker acid than HClO4? I. S is less electronegative than Cl. II. H2SO4 has fewer terminal O atoms than HClO4. III. The S–H bond is less polar than the Cl–H bond. Select one: a.I only b.I and II only c.I, II, and III d.II onlyarrow_forwardPredict the stronger acid in each pair: (a) HCl or HF;(b) H3PO4 or H3AsO4; (c) HBrO3 or HBrO2; (d) H2C2O4 orHC2O4-; (e) benzoic acid (C6H5COOH) or phenol (C6H5OH).arrow_forwardArrange the compounds in Figure 36 from the strongest to the weakest acid.arrow_forward
- Explain why the C – Ha bond is much more acidic than the C – Hb bond in pentan-2-one.arrow_forwardcompared to HCO3-, H2co3 has a A Stronger conjugated base B Weaker conjugated base C Higher ka D Lower ka E Both b and carrow_forwardWhich solution has the highest concentration of H3O+: a 0.50 M solution of acetic acid (CH3CO2H), or a 0.50 M solution of formic acid (HCO2H)? Ka of acetic acid is 1.8×10−5 and Ka of formic acid is 1.8×10−4.arrow_forward
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