Notes in General-Chemistry

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Published	03/29/2024	In element notation, A is the {{c1::Mass number}}
Published	03/29/2024	In element notation, Z is the {{c1::atomic number}}
Published	03/29/2024	{{c1::Atomic weight}} is {{c2::the weighted average of the masses of an element's isotopes}}.
Published	03/29/2024	The {{c1::Rutherford Model::... Model}} states that an atom is mostly  {{c2::empty space}}, with {{c2::electrons::electrons/protons}} orbiting a …
Published	03/29/2024	According to the {{c1::Bohr Model::... Model}}, {{c2::electrons orbit the nucleus in orbits that have a set size and energy}}.
Published	03/29/2024	The {{c1::Heisenberg Uncertainty Principle::... Principle}} states that it is impossible to know the {{c2::momentum}} and {{c2::position}} o…
Published	03/29/2024	{{c1::Hund’s Rule}} states that {{c2::all orbitals must first have one electron before any orbital can obtain a second electron}}.
Published	03/29/2024	The {{c1::Pauli Exclusion Principle::... Principle}} states that {{c2::no two electrons can share the same four identical quantum numbers}}.
Published	03/29/2024	Avogadro’s Number = {{c1::6.022 × 1023 = 1 mol}}
Published	03/29/2024	Planck’s Constant (h) = {{c1::6.626 × 10-34 J•s}}
Published	03/29/2024	Speed of Light (c) = {{c1::3.0 × 108 m/s}}
Published	03/29/2024	Give the equation for energy of a photon:{{c1::}}
Published	03/29/2024	Paramagnetic materials are {{c1::pulled into}} an external magnetic field.
Published	03/29/2024	He atom is {{c1::diamagnetic::diamagnetic or paramagnetic}}
Published	03/29/2024	Li is {{c1::paramagnetic::diamagnetic or paramagnetic}}
Published	03/29/2024	Quantum number {{c1::n}} is the {{c2::principal quantum}} number and gives the electron {{c1::energy level or shell number}}
Published	03/29/2024	Quantum number {{c1::l}} is the {{c2::azimuthal quantum}} number and gives the {{c1::3D shape (subshell)}} of an orbital
Published	03/29/2024	Quantum number {{c1::ml}} is the {{c2::magnetic quantum}} number and gives the {{c1::orbital sub-type}}
Published	03/29/2024	Quantum number {{c1::ms}} is the {{c2::spin quantum}} number and gives the {{c1::electronic spin}} of the electron
Published	03/29/2024	The maximum number of electrons in {{c2::a single energy level}} in terms of {{c3::principal quantum}} number = {{c1::2n2}}
Published	03/29/2024	The maximum number of electrons in a single subshell in terms of the {{c2::azimuthal quantum}} number = {{c1::4l + 2}}
Published	03/29/2024	A/an {{c1::free radical}} is an atom or molecule with {{c2::an unpaired}} electron.
Published	03/29/2024	The Azimuthal quantum number for this orbital is {{c1::0 = s orbital}}
Published	03/29/2024	The Azimuthal quantum number for this orbital is {{c1::1 = p orbital}}
Published	03/29/2024	The Azimuthal quantum number for this orbital is {{c1::2 = d orbital}}
Published	03/29/2024	The Azimuthal quantum number for this orbital is {{c1::3 = f orbital}}
Published	03/29/2024	Give the principal and azimuthal quantum number labels for the periodic table.{{c1::}}
Published	03/29/2024	The {{c1::Aufbau Principle::... Principle}} states that {{c2::electrons will fill the lower energy levels before moving to higher energy orbitals}}.
Published	03/29/2024	The elements in the group labeled with ? are known as {{c1::alkali metals}}.
Published	03/29/2024	The elements in the group labeled with ? are known as {{c1::alkaline earth metals}}
Published	03/29/2024	The elements in the groups labeled with ? are known as {{c1::transition metals}}
Published	03/29/2024	The elements in the grey group labeled with ? are known as {{c1::post-transition metals}}
Published	03/29/2024	The elements in the group labeled with ? are known as {{c1::metalloids}}
Published	03/29/2024	The elements in the groups labeled with ? are known as {{c1::non-metals}}
Published	03/29/2024	The elements in the group labeled with ? are known as {{c1::halogens}}
Published	03/29/2024	The elements in the group labeled with ? are known as {{c1::noble gases}}.
Published	03/29/2024	The elements in the groups labeled with ? are known as {{c1::lanthanides}}
Published	03/29/2024	{{c1::Zeff}} is the {{c2::attractive positive}} charge of {{c2::nuclear protons}} acting on {{c2::valence electrons}}.
Published	03/29/2024	What is the periodic trend for effective nuclear charge?{{c1::}}
Published	03/29/2024	{{c1::Ionization energy}} is the amount of energy required to {{c2::remove an electron}}.
Published	03/29/2024	What is the periodic trend for ionization energy?{{c1::}}
Published	03/29/2024	{{c1::Electron affinity}} is {{c2::the amount of energy released when an electron is added to the atom}}.
Published	03/29/2024	What is the periodic trend for electron affinity?{{c1::}}
Published	03/29/2024	{{c1::Electronegativity}} is a measure of {{c2::how strongly atoms attract electrons in a bond}}.
Published	03/29/2024	What is the periodic trend for electronegativity?{{c1::}}
Published	03/29/2024	What is the periodic trend for atomic size?{{c1::}}
Published	03/29/2024	Give the approximate electronegativity values of H, C, N, O, and F {{c1::  HCNOFExact2.202.553.043.443.98≈2.02.53.03.54.0 }}
Published	03/29/2024	A/an {{c1::covalent}} bond is the {{c2::sharing}} of electrons between two elements.
Published	03/29/2024	{{c1::Coordinate covalent}} bonds are when {{c2::a single atom provides both bonding electrons}}.
Published	03/29/2024	{{c1::Ionic}} bonds are formed by {{c2::the complete transfer of valence electron(s) between atoms}}.
Published	03/29/2024	{{c1::Bond order}} refers to {{c2::the number of bonds between two atoms (single, double, or triple bond)}}.
Published	03/29/2024	The greater the number of bonds (bond order) the {{c1::higher::higher or lower}} the bond strength and the {{c1::shorter::longer or shorter}} the bond…
Published	03/29/2024	Non-polar bonds have a △EN that is {{c1::less than 0.5}}.
Published	03/29/2024	Polar bonds have a △EN that is between {{c1::0.5}} and {{c1::1.7}}.
Published	03/29/2024	{{c2::Cations}} are ions with a {{c1::positive}} charge.
Published	03/29/2024	{{c2::Anions}} are ions with a {{c1::negative}} charge
Published	03/29/2024	{{c1::Crystalline lattices}} are {{c2::large, organized arrays of ions.::what exactly?}}
Published	03/29/2024	{{c2::Hydrogen}} bonds are most often formed between hydrogen and the following elements: {{c1::O, N and F}}.
Published	03/29/2024	{{c2::Van der Waals Forces}} is a general term that includes {{c1::dipole-dipole}} forces and {{c1::London dispersion}} forces.
Published	03/29/2024	{{c1::Dipole-dipole}} forces are {{c2::attractive}} forces between {{c2::the positive end of one polar molecule}} and {{c2::the negative end…
Published	03/29/2024	{{c1::London dispersion}} forces are {{c2::temporary attractive}} forces created when {{c3::a temporary dipole induces a dipole in a neighboring molec…
Published	03/29/2024	Place in order of decreasing strength:hydrogen bonds, dipole-dipole forces, and London dispersion forces{{c1::hydrogen bonds > dipole-dipole > L…
Published	03/29/2024	{{c1::Sigma}} bonds are formed by {{c2::head-on overlapping}} between atomic orbitals.
Published	03/29/2024	{{c1::Pi}} bonds are formed by {{c2::lateral (side-by-side) overlap}} of atomic orbitals.
Published	03/29/2024	{{c1::Formal charge}} is the charge given to {{c2::an individual element within a molecule}}.
Published	03/29/2024	Give the formula for formal chargeFormal Charge = {{c1::valence electrons − dots − sticks}}.
Published	03/29/2024	O is the hydrogen bond {{c1::acceptor::acceptor or donor}}.N is the hydrogen bond {{c1::donor::acceptor or donor}}.
Published	03/29/2024	The bond angle of an {{c2::sp}} hybridized atom is {{c1::180°}}
Published	03/29/2024	The bond angle of an {{c2::sp2}} hybridized atom is {{c1::120°}}
Published	03/29/2024	The bond angle of an {{c2::sp3}} hybridized atom is {{c1::109.5°}}
Published	03/29/2024	Bond angles of an {{c2::sp3d}} hybridized atom are {{c1::90°}} and {{c1::120°}}
Published	03/29/2024	The bond angle of an {{c2::sp3d2}} hybridized atom is {{c1::90°}}
Published	03/29/2024	An H2O molecule has {{c2::bent}} geometry because {{c1::the lone pair of electrons repel each other and push the H atoms away}}
Published	03/29/2024	An {{c1::empirical}} formula is the {{c2::simplest whole-number}} ratio of atoms.
Published	03/29/2024	The {{c1::molecular}} formula shows {{c2::the exact number of atoms of each element}}.
Published	03/29/2024	{{c1::Reaction order}} is a number that relates the {{c2::rate of a chemical reaction}} to the {{c2::concentrations of the reacting sub…
Published	03/29/2024	For a {{c2::zeroth}} order reaction:Rate Law: {{c1::\(R=k\)}}Integrated Rate Law: {{c1::\([A] = [A]_0-kt\)}}
Published	03/29/2024	For a {{c2::first}} order reaction:Rate Law: {{c1:: \(R = k[A]\)}}Integrated Rate Law: {{c1:: \([A] = [A]_0 \times e^{-k…
Published	03/29/2024	For a {{c2::second}} order reaction:Rate Law: {{c1::\(R = k[A]^2\)}}Integrated Rate Law: {{c1::\(\frac{1}{[A]} = \frac{1}{[A]_0}+k…
Published	03/29/2024	The units for the rate constant of a {{c2::zeroth}} order reaction are{{c1::\(\frac{M}{s}\)}}
Published	03/29/2024	The units for the rate constant of a {{c2::first}} order reaction are{{c1::\(\frac{1}{s}\)}}
Published	03/29/2024	The units for the rate constant of a {{c2::second}} order reaction are{{c1::\(\frac{1}{M \cdot s}\)}}
Published	03/29/2024	{{c2::}}The order of this plotted reaction is {{c1::zeroth order}}.
Published	03/29/2024	{{c2::}}The order of this plotted reaction is {{c1::first order}}
Published	03/29/2024	{{c2::}}The order of this plotted reaction is {{c1::second order}}
Published	03/29/2024	In {{c1::decomposition}} reactions, {{c2::a single reactant breaks down::this happens}}.
Published	03/29/2024	{{c1::Combustion reactions}} are {{c2::exothermic}} reactions in which something reacts with {{c2::oxygen}}.
Published	03/29/2024	A/an {{c1::neutralization}} reaction is when {{c2::an acid and base}} react to form {{c2::water and salt}}
Published	03/30/2024	A/an {{c1::hydrolysis}} reaction uses water to break the bonds in a molecule.
Published	03/29/2024	Give the {{c2::Arrhenius}} equation:{{c1::\(k = A \times e^{\frac{-E_a}{RT}~}\)}}
Published	03/29/2024	If temperature goes {{c2::up::up or down}}, the rate constant goes {{c1::up::up or down}} and the reaction speed goes {{c1::up::up or down}} .
Published	03/29/2024	The {{c1::reaction quotient (Qc)}} is a measure of {{c2::the relative amounts of products and reactants present in a reaction at a given tim…
Published	03/29/2024	You exclude {{c2::pure solids and liquids}} in the {{c3::reaction quotient}} and {{c3::equilibrium constant}} because {{c1::their effective concentrat…
Published	03/29/2024	If Q {{c2::<}} Keq, then the reaction will move to the {{c1::right}}.
Published	03/29/2024	A reaction is at {{c2::equilibrium}} if Q = {{c1::Keq}}.
Published	03/29/2024	If Q {{c2::>}} Keq, then the reaction will move to the {{c1::left}}.
Published	03/29/2024	{{c2::Kinetic}} products are {{c1::higher::higher or lower}} in free energy compared to {{c2::thermodynamic}} products and kinetic…
Published	03/29/2024	Thermodynamic products are {{c1::lower::higher or lower}} in {{c2::free energy}} compared to kinetic products and they are {{c1::more::…
Published	03/29/2024	{{c2::Le Châtelier’s Principle}} states that if {{c1::a stress is applied to a system}}, then {{c1::system shifts to relieve that applied stress}…
Published	03/29/2024	{{c2::Standard temperature & pressure}} are {{c1::273}} K, {{c1::1}} atm.
Published	03/29/2024	{{c1::Fusion}} is the phase change from {{c2::solid}} to {{c2::liquid}}.
Published	03/29/2024	{{c1::Freezing}} is the phase change from {{c2::liquid}} to {{c2::solid}}.
Published	03/29/2024	{{c1::Vaporization}} is the phase change from {{c2::liquid}} to {{c2::gas}}.
Published	03/29/2024	{{c1::Sublimation}} is the phase change from {{c2::solid}} to {{c2::gas}}.
Published	03/29/2024	{{c1::Deposition}} is the phase change from {{c2::gas}} to {{c2::solid}}.
Published	03/29/2024	Label the phases in the phase diagram: {{c1::}}
Published	03/29/2024	The point in phase diagram where all 3 phases exist is known as the {{c1::triple point}}.
Published	03/29/2024	A/an {{c1::supercritical}} fluid is one in which {{c2::the density of gas = density of liquid}}.
Published	03/29/2024	{{c1::Gibbs Free Energy}} combines {{c2::enthalpy}} and {{c2::entropy}} into a single value and is used to determine {{c3::the spontane…
Published	03/29/2024	If a reaction has a {{c2::positive}} ∆H and {{c2::positive}} ∆S, then it will be {{c1::spontaneous::spontaneous or non-spontaneous}}&nb…
Published	03/29/2024	If a reaction has a {{c2::positive}} ∆H and {{c2::negative}} ∆S, then it will be {{c1::non-spontaneous::spontaneous or non-spontan…
Published	03/29/2024	If a reaction has a {{c2::negative}} ∆H and {{c2::positive}} ∆S, then it will be {{c1::spontaneous::spontaneous or non-spontaneous…
Published	03/29/2024	If a reaction has a {{c2::negative}} ∆H and {{c2::negative}} ∆S, then it will be {{c1::spontaneous::spontaneous or non-spontaneous…
Published	03/29/2024	{{c2::Room}} temperature is approximately {{c1::25°C aka 75°F}}
Published	03/29/2024	{{c2::Body}} temperature is approximately {{c1::37°C aka 98.6°F}}
Published	03/29/2024	{{c1::Enthalpy (H)}} is a measure of {{c2::the potential energy of a system}} found in {{c3::intermolecular attractions}} and {{c3::chemical…
Published	03/29/2024	Phase changes from {{c2::solid}} → {{c2::liquid}} → {{c2::gas}} are {{c1::endothermic::endothermic or exothermic}}.
Published	03/29/2024	Phase changes from {{c2::gas}} → {{c2::liquid}} → {{c2::solid}} are {{c1::exothermic::endothermic or exothermic}}
Published	03/29/2024	Give the formula for ∆H when using heat of formations{{c1::\(\Delta H^{\circ}_{rxn} = \Delta H^{\circ}_{products} - \Delta H^{\circ}_{reactants}\…
Published	03/29/2024	Give the formula for ∆H when using bond dissociation energies{{c1::\(\Delta H^{\circ}_{rxn} = \Delta H^{\circ}_{reactants} - \Delta H^{\circ}_{pr…
Published	03/29/2024	{{c1::Entropy}} is a measure of how much energy has spread out or how spread out energy has become.
Published	03/29/2024	Give the formula for the standard entropy of reaction{{c1::\(\Delta S^{\circ}_{rxn} = \Delta S^{\circ}_{f,products} - \Delta S^{\circ}_{f,reactants}\)…
Published	03/29/2024	Give the Gibbs Free Energy equation under standard conditions that uses the equilibrium constant Keq{{c1::\(\Delta G^{\circ}_{rxn} = -RTln(K_{eq})\)}}
Published	03/29/2024	Give the Gibbs Free Energy equations that use the reaction quotient Q{{c1::\(\Delta G_{rxn} = RTln(\frac{Q}{K_{eq}~})\)}}{{c1::\(\Delta G_{rxn} =…
Published	03/29/2024	If ∆G {{c2::<}} O, the reaction will be {{c1::spontaneous}}.
Published	03/29/2024	If ∆G {{c2::=}} O, the reaction will be {{c1::at equilibrium}}
Published	03/29/2024	If ∆G {{c2::>}} O, the reaction will be {{c1::non-spontaneous}}
Published	03/29/2024	Orbits that are {{c2::farther from::closer to or farther from}} the nucleus have {{c1::increased::increased or decreased}} energy.
Published	03/29/2024	If an electron moves to a {{c2::farther}} orbital, a photon is {{c1::absorbed}}.
Published	03/29/2024	If an electron moves to a {{c2::closer}} orbital, a photon is {{c1::emitted}}
Published	03/29/2024	{{c2::Ionic}} bonds have a △EN that is {{c1::greater than 1.7}}.
Published	03/29/2024	The orbital hybridization of an atom with {{c2::2}} electron groups is {{c1::sp}}.
Published	03/29/2024	The electronic geometry of an atom with {{c2::2}} electron groups is {{c1::linear}}.
Published	03/29/2024	The orbital hybridization of an atom with {{c2::3}} electron groups is {{c1::sp2}}.
Published	03/29/2024	The electronic geometry of an atom with {{c2::3}} electron groups is {{c1::trigonal planar}}
Published	03/29/2024	The orbital hybridization of an atom with {{c2::4}} electron groups is {{c1::sp3}}.
Published	03/29/2024	The electronic geometry of an atom with {{c2::4}} electron groups is {{c1::tetrahedral}}.
Published	03/29/2024	The orbital hybridization of an atom with {{c2::5}} electron groups is {{c1::sp3d}}.
Published	03/30/2024	The electronic geometry of an atom with {{c2::5}} electron groups is {{c1::trigonal bipyramidal}}.
Published	03/29/2024	The orbital hybridization of an atom with {{c2::6}} electron groups is {{c1::sp3d2}}.
Published	03/29/2024	The electronic geometry of an atom with {{c2::6}} electron groups is {{c1::octahedral}}.
Published	03/29/2024	{{c1::Equilibrium Constant (Keq)}} is the value of the {{c2::reaction quotient (Q)}} when a chemical reaction has reached equilibrium
Published	03/29/2024	Protons and electrons have {{c1::different::the same or different}} masses.
Published	03/29/2024	A/an {{c1::solution}} is a special type of {{c2::homogeneous}} mixture composed of {{c3::two or more substances}}.
Published	03/29/2024	A/an {{c1::solvent}} is a {{c3::liquid}} that {{c2::dissolves a solid, liquid or gaseous solute::does what?}}
Published	03/29/2024	{{c1::Solvation}} or {{c1::dissolution}} is the process of {{c2::dissolving a solute in solvent}}.
Published	03/29/2024	{{c1::Solubility}} is measured in terms of {{c2::the maximum amount of solute dissolved in a solvent at equilibrium}}.
Published	03/29/2024	{{c1::Molar solubility}} is the number of {{c2::moles}} of a substance that can be dissolved per {{c2::liter}} of solution before the soluti…
Published	03/29/2024	A/an {{c1::complex ion}} has a {{c2::metal ion}} at its center with a number of other molecules or ions surrounding it.
Published	03/29/2024	Polar molecules are {{c1::hydrophilic::hydro...}}.Nonpolar molecules are {{c1::hydrophobic::hydro...}}.
Published	03/29/2024	In a 1 molar solution, {{c2::normality}} can be thought of as the {{c1::number of protons a molecule of acid can release in solution}}.
Published	03/29/2024	{{c2::Na+}}, {{c2::K+}}, {{c2::NH4+}}, and {{c2::NO3-}} are {{c1::always::sometimes or always}} soluble.
Published	03/29/2024	{{c2::Cl-}}, {{c2::Br-}}, and {{c2::I-}} are {{c1::soluble}} except with {{c3::Pb2+}}, {{c3::Hg22+}}, and {{c3::Ag+}}
Published	03/29/2024	{{c2::SO42-}} is {{c1::soluble}} except with {{c3::Ca2+}}, {{c3::Sr2+}}, {{c3::Ba2+}}, {{c3::Pb2+}}, {{c3::Hg22+}}, and {{c3::Ag+}}
Published	03/29/2024	{{c2::S2-}} is {{c1::insoluble}} except with {{c3::Na+}}, {{c3::K+}}, {{c3::NH4+}}, {{c3::Mg2+}}, {{c3::Ca2+}}, {{c3::Sr2+}}, and {{c3::Ba2+}}
Published	03/29/2024	{{c2::O2-}} is {{c1::insoluble}} except with {{c3::Na+}}, {{c3::K+}}, {{c3::Sr2+}}, and {{c3::Ba2+}}
Published	03/29/2024	{{c2::OH-}} is {{c1::insoluble}} except with {{c3::Na+}}, {{c3::K+}}, {{c3::Ca2+}}, {{c3::Sr2+}}, and {{c3::Ba2+}}
Published	03/29/2024	{{c2::CrO42-}} is {{c1::insoluble}} except with {{c3::Na+}}, {{c3::K+}}, {{c3::NH4+}}, and {{c3::Mg2+}}
Published	03/29/2024	{{c2::PO43-}} and {{c2::CO32-}} are {{c1::insoluble}} except with {{c3::Na+}}, {{c3::K+}}, and {{c3::NH4+}}
Published	03/29/2024	{{c3::Ksp}} is the {{c1::equilibrium constant}} for a reaction that consists of {{c2::a solid dissolving in a solution}}.
Published	03/29/2024	Give the solubility product constant for the following chemical equation:BaSO4(s) ⇌ Ba2+(aq) + SO42-(aq)Ksp = {{c1::[Ba2+][SO42-]}}
Published	03/29/2024	{{c2::Qsp}} is the {{c1::reaction quotient}} for a reaction that consists of {{c3::a solid dissolving in a solution}}.
Published	03/29/2024	If Qsp is {{c1::less than::less than, greater than, or equal to}} Ksp then the solution is {{c2::unsaturated}} so {{c2::no precipitate}} will for…
Published	03/29/2024	If Qsp is {{c1::equal to::less than, greater than, or equal to}} Ksp then the solution is {{c2::saturated and at equilibrium}} so {{c2::no p…
Published	03/29/2024	If Qsp is {{c1::greater than::less than, greater than, or equal to}} Ksp then the solution is {{c2::supersaturated}} so {{c2::a precipitate}…
Published	03/29/2024	The {{c3::common ion effect}} causes {{c2::solubility}} to {{c1::decrease::increase or decrease}} when {{c2::adding like ions.::what happens?}}
Published	03/29/2024	A/an {{c1::chelate}} is a compound with a {{c2::central cation}} bonded to {{c2::the same ligand in multiple places}}
Published	03/29/2024	{{c1::Colligative properties}} are {{c2::physical}} properties of {{c2::solutions}} that depend on {{c3::the concentration of dissolved particles}}&nb…
Published	03/29/2024	{{c3::Raoult's law}} states that {{c2::the vapor pressure of a solution}} is equal to {{c1::the sum of the vapor pressures of each volatile component …
Published	03/29/2024	The presence of {{c2::nonvolatile solute particles}} in a liquid solvent results in a/an {{c1::reduction::increase or reduction}} of the vap…
Published	03/29/2024	{{c1::Osmolarity}} is the number of {{c2::individual particles in solution}}.
Published	03/29/2024	{{c2::An Arrhenius}} acid is a substance that {{c1::produces H+}}.
Published	03/29/2024	{{c2::An Arrhenius}} base is a substance that {{c1::produces OH-}}
Published	03/29/2024	{{c2::A Brønsted-Lowry}} acid is a substance that {{c1::donates H+}}
Published	03/29/2024	{{c2::A Brønsted-Lowry}} base is a substance that {{c1::accepts H+}}
Published	03/29/2024	{{c2::A Lewis}} acid is a substance that {{c1::accepts a pair of electrons}}
Published	03/29/2024	{{c2::A Lewis}} base is a substance that {{c1::donates a pair of electrons}}
Published	03/29/2024	A/an {{c1::amphoteric species::... species}} is a species that can {{c2::behave as an acid or a base::do this!}}
Published	03/29/2024	{{c1::Polyprotic acids}} are specific acids that are capable of {{c2::losing more than a single proton per molecule.::doing what?}}
Published	03/29/2024	The equilibrium constant for the autoionization of water, {{c2::Kw}}, is {{c1::10-14}} at 25º C.
Published	03/29/2024	pH + pOH = {{c1::14}}.
Published	03/29/2024	{{c2::[H+]}} = {{c1::10-pH}}.
Published	03/29/2024	{{c2::[OH-]}} = {{c1::10-pOH}}.
Published	03/29/2024	{{c2::Strong}} acids and bases dissociate {{c1::completely::partially or completely}}.
Published	03/29/2024	{{c2::Weak}} acids and bases do not completely {{c1::dissociate}}.
Published	03/29/2024	{{c1::Ka}} is the {{c2::equilibrium constant}} corresponding to {{c3::the dissociation of an acid, HA, into a proton and its …
Published	03/29/2024	{{c1::Kb}} is the {{c2::equilibrium constant}} corresponding to {{c3::the dissociation of a base, BOH, into a hydroxide ion and it…
Published	03/29/2024	{{c2::pKa}} = {{c1::-log(Ka)}}.
Published	03/29/2024	{{c2::pKb}} = {{c1::-log(Kb)}}
Published	03/29/2024	pKa + pKb = {{c1::pKw}} = {{c1::14::#}}
Published	03/29/2024	Strong acids and bases have {{c1::weak::strong or weak}} conjugates.
Published	03/29/2024	Weak acids and bases have {{c1::strong::strong or weak}} conjugates.
Published	03/29/2024	A neutralization reaction is when an acid and a base react to form {{c1::water}} and {{c1::a salt}}.
Published	03/29/2024	{{c2::An acidic buffer}} is a mixture of a {{c1::weak acid}} and {{c1::its conjugate salt}}.
Published	03/29/2024	{{c2::A basic buffer}} is a mixture of a {{c1::weak base}} and {{c1::its conjugate salt}}.
Published	03/29/2024	Buffering capacity is a measure of the ability of a buffer to {{c1::resist changes in pH}}.
Published	03/29/2024	When {{c2::[A-]}} = {{c2::[HA]}} at the half-equivalence point, log({{c2::1}}) = {{c1::0}}, so pH = {{c1::pKa}}.
Published	03/29/2024	The {{c1::half-equivalence point}}, also known as the {{c1::midpoint}}, is the point of the {{c2::buffering}} region, in which {{c2::half the analyte …
Published	03/29/2024	The {{c1::equivalence point}} is the point at which {{c2::equivalent amounts of acid and base have reacted.::what has happened?}}
Published	03/29/2024	In a titration, the {{c1::titrant}} (aka the {{c1::known solution}}) is added from a {{c2::burette}} to a certain quantity of the {{c1:…
Status	Last Update	Fields