- 15.4.1: Identify the stronger acid and the stronger base in the reaction de...
- 15.4.2: Write the acid-ionization constant expression for the weak acid H2SO3.
- 15.4.3: The hydrogen sulfite ion, HSO3 , is a weak acid in aqueous solution...
- 15.4.4: What is a buffer solution?
- 15.4.5: Give two examples of the practical uses of buffers.
- 15.4.6: Use Table 7 to determine which direction is favored in the followin...
- 15.4.7: A 0.105 M solution of HOCl has a pH of 4.19.What is the acid-ioniza...
- 15.4.8: A buffer solution, prepared from equal amounts of an acid and its c...
- 15.4.9: Calculate the Ka of nitrous acid, given that a 1.00 M solution of t...
- 15.4.10: Ammonia is a weak base. A 0.0123 M solution of ammonia has a hydrox...
- 15.4.11: What would be the value of the acidionization constant for an acid ...
- 15.4.12: What would be a good acid-base pair from which to prepare a buffer ...
- 15.4.13: If 99.0% of the weak acid HX stays un-ionized in 1.0 M aqueous solu...
- 15.4.14: Write all three Ka expressions for H3PO4. Which will have the small...
- 15.4.15: Calculate Keq for the following reaction: H2CO3(aq) + CO32(aq) 2HCO...
Solutions for Chapter 15.4: Equilibria of Weak Acids and Bases
Full solutions for Modern Chemistry: Student Edition 2006 | 1st Edition
A list of metals in order of decreasing ease of oxidation. (Section 4.4)
The wave function (?) of an electron in an atom. (7.5)
The slow oxidation of organic compounds that occurs in the presence of atmospheric oxygen.
bonding atomic radius
The radius of an atom as defined by the distances separating it from other atoms to which it is chemically bonded. (Section 7.3)
A nuclear reactor that produces more fissionable materials than it uses. (19.5)
The scientific discipline that studies the composition, properties, and transformations of matter. (Chapter 1: Introduction)
Substance capable of conducting electric current. (21.3)
When two waves interact with each other in a way that produces a wave with a larger amplitude.
Protein that does not exhibit normal biological activities. (25.3)
The arrangement of electrons in the orbitals of an atom or molecule (Section 6.8)
A model for the behavior of electrons in metals. (Section 12.4)
The equilibrium established between substances in two or more different phases, for example, between a gas and a solid or between a solid and a liquid. (Section 15.4)
limiting reactant (limiting reagent)
The reactant present in the smallest stoichiometric quantity in a mixture of reactants; the amount of product that can form is limited by the complete consumption of the limiting reactant. (Section 3.7)
A simple sugar, most commonly containing six carbon atoms. The joining together of monosaccharide units by condensation reactions results in formation of polysaccharides. (Section 24.8)
nucleophilic aromatic substitution
A substitution reaction in which an aromatic ring is attacked by a nucleophile, which replaces a leaving group.
Pi (p) bond
A covalent bond formed by the overlap of parallel 2p orbitals.
The energy that can be released if given an opportunity
A solvent that contains at least one hydrogen atom connected directly to an electronegative atom.
A reaction for which the ratio of products is determined solely by the distribution of energy among the products.
A compound containing an !SH (sulfhydryl) group bonded to an sp3 -hybridized carbon.