General Chemistry: Gas Laws, Chemical Equilibrium, Solubility, and Acid-Base Chemistry

Comprehensive review flashcards covering Gas Laws, Dalton's Law of Partial Pressures, Chemical Equilibrium (Keq, Kc, Kp, Q), Le Châtelier's Principle, Solubility Product (Ksp), Common Ion Effect, and Acid-Base Chemistry from CHEM 10171 lecture notes.

According to the lecture notes, what physical interaction gives rise to gas pressure?

Gas pressure arises from the collision of gas particles on a surface.

What are the standard atmospheric pressure equivalents of $1.00\,\text{atm}$ in $\text{mmHg}$, $\text{Torr}$, $\text{kPa}$, $\text{psi}$, and $\text{bar}$?

$1.00\,\text{atm} = 760\,\text{mmHg} = 760\,\text{Torr} = 101.325\,\text{kPa} = 101{,}325\,\text{Pa} = 14.7\,\text{psi} = 29.92\,\text{in Hg} = 1.013\,\text{bar}$.

What four characteristics define the behavior of ideal gases in the lecture notes?

1. Gas particles have negligible volume.
2. Gas particles are equally sized.
3. There are no intermolecular forces.
4. Gas particles move randomly.

What is the Ideal Gas Law equation, and what numerical value and units are specified for the gas constant $R$?

The equation is $PV = nRT$, where $R = 0.0821\,\frac{\text{L}\cdot\text{atm}}{\text{mol}\cdot\text{K}}$.

What specific variable proportionalities were established by Charles, Avogadro, and Boyle?

Charles established that volume is proportional to temperature ($V \propto T$); Avogadro established that volume is proportional to moles ($V \propto n$); and Boyle established that volume is inversely proportional to pressure ($V \propto \frac{1}{P}$).

Which scientist, shown below, is considered the father of modern chemistry, a pioneer of the scientific method, and author of The Skeptical Chymist?

Robert Boyle.

What principle governs a mixture of gases according to Dalton's Law of Partial Pressures?

Each gas exerts its own pressure independent of other gases, such that $P_{\text{Total}} = P_A + P_B + P_C + \dots$ and $n_{\text{Total}} = n_A + n_B + n_C + \dots$.

How is the mole ratio or mole fraction ($X_i$) of a component gas in a mixture calculated and related to partial pressure?

$X_i = \frac{n_i}{n_{\text{Total}}} = \frac{P_i}{P_{\text{Total}}}$, which allows calculating individual partial pressure via $P_i = X_i P_{\text{Total}}$.

What are the standard temperature and pressure (STP) parameters, and what volume does one mole of an ideal gas occupy at STP?

STP is defined as $1\,\text{atm}$ ($760\,\text{mmHg}$) and $273\,\text{K}$ ($0^\circ\text{C}$), at which one mole of an ideal gas occupies $22.4\,\text{L}$.

What do a single-sided straight arrow, two parallel opposite-direction arrows, and curved arrows signify in chemical equations?

A single-sided straight arrow signifies a reaction arrow ($\rightarrow$), two parallel arrows in opposite directions signify a reversible reaction arrow ($\rightleftharpoons$), a half-arrow curved signifies moving $1$ electron, and a full-arrow curved signifies moving $2$ electrons.

How is dynamic equilibrium defined in a reversible chemical reaction?

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction; concentrations of all species stabilize, but both forward and reverse reactions continue to take place.

What chemical equation represents the Haber-Bosch process for industrial nitrogen fixation?

$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ in the presence of an iron ($\text{Fe}$) catalyst.

Which chemist, pictured below, helped develop the industrial synthesis of ammonia and is historically referred to as the 'Father of Chemical Warfare'?

Fritz Haber.

Which industrial chemist, shown below, partnered with Fritz Haber to scale up ammonia production and won a Nobel Prize for his contributions?

Carl Bosch.

For the general gaseous reaction $aA(g) + bB(g) \rightleftharpoons cC(g) + dD(g)$, how are $K_c$ and $K_p$ expressed?

$K_c = \frac{[C]^c [D]^d}{[A]^a [B]^b}$ (using molar concentrations, $\text{M}$), and $K_p = \frac{(P_C)^c (P_D)^d}{(P_A)^a (P_B)^b}$ (using partial pressures in $\text{atm}$).

Which types of substances are excluded when writing equilibrium constant ($K$) expressions?

Pure solids ($s$), pure liquids ($l$), and spectator ions are omitted from $K$ expressions.

What does the magnitude of the equilibrium constant indicate when $K > 1$, $K < 1$, and $K = 1$?

If $K > 1$, products are favored at equilibrium (forward reaction is favored); if $K < 1$, reactants are favored at equilibrium (reverse reaction is favored); if $K = 1$, neither direction is favored.

How does comparing the reaction quotient ($Q$) to the equilibrium constant ($K$) indicate reaction progression?

If $Q < K$, the reaction proceeds in the forward direction (shifts toward products); if $Q > K$, the reaction proceeds in the reverse direction (shifts toward reactants); if $Q = K$, the reaction is at equilibrium.

What is Le Châtelier's Principle?

When a chemical system at equilibrium is disturbed, the reaction will shift in the direction that minimizes the disturbance.

According to Le Châtelier's Principle, how does changing pressure or adding an inert gas affect a gaseous reaction system?

Increasing pressure shifts the reaction toward the side with the lower number of moles of gas; decreasing pressure shifts it toward the side with the higher number of moles of gas; if both sides have equal moles of gas, changing pressure has no effect; adding an inert gas (noble gas) has no effect.

How does a change in temperature affect equilibrium in exothermic versus endothermic reactions?

For an exothermic reaction ($\text{Reactants} \rightleftharpoons \text{Products} + \text{heat}$), increasing temperature shifts the reaction toward reactants, and decreasing temperature shifts it toward products. For an endothermic reaction ($\text{heat} + \text{Reactants} \rightleftharpoons \text{Products}$), increasing temperature shifts the reaction toward products, and decreasing temperature shifts it toward reactants.

What is the definition of solubility, and what three factors determine it?

Solubility is the maximum amount of a solute that will dissolve in a given amount of solution at a given temperature. The three determining factors are:

1. Identities of solute and solvent
2. Temperature
3. Strength of interactions (solute-solute, solvent-solvent, solute-solvent).

What is the writing caveat regarding the solubility product constant ($K_{sp}$) for dissolving salts?

$K_{sp}$ is always written as the product of the dissolved ion concentrations raised to their stoichiometric coefficients (solid reactant omitted), even when discussing the reverse precipitation reaction.

What is molar solubility ($S$ or $s$)?

The concentration in moles per liter ($\text{mol}/\text{L}$ or $\text{M}$) of a salt that dissolves under specified conditions.

What is the common ion effect on salt solubility?

A sparingly soluble salt is less soluble in a solution containing its constituent (common) ions than in pure solvent, in accordance with Le Châtelier's Principle.

What chemical reaction illustrates how atmospheric carbon dioxide absorption in seawater leads to ocean acidification and impedes calcification?

$CO_2 + H_2O + CO_3^{2-} \rightarrow 2HCO_3^-$, which consumes carbonate ions essential for marine shell calcification.

How do Arrhenius acids and bases differ in aqueous solution?

An Arrhenius acid produces $H^+$ (hydrogen ion/proton, forming hydronium $H_3O^+$) in aqueous solution, whereas an Arrhenius base produces $OH^-$ (hydroxide ion) in aqueous solution.

How does the Brønsted-Lowry definition classify acids and bases?

A Brønsted-Lowry acid donates protons ($H^+$), and a Brønsted-Lowry base accepts protons ($H^+$).

What is a conjugate acid-base pair?

Two substances related to each other by the transfer of a single proton ($H^+$). When an acid loses a proton, it forms its conjugate base; when a base gains a proton, it forms its conjugate acid.

What is the distinction between amphoteric and amphiprotic species?

An amphoteric substance can act as either an acid or a base; an amphiprotic substance specifically has the ability to either donate or accept a proton ($H^+$). Water ($H_2O$) and hydrogen carbonate ($HCO_3^-$) are examples.

How does bond strength influence the relative acidity of binary halogen acids ($HF$, $HCl$, $HBr$, $HI$)?

Longer bonds are weaker bonds, making proton donation easier. Moving down the halogens, bond length increases ($HF < HCl < HBr < HI$), bond strength decreases, and acid strength increases ($HF$ is weak, whereas $HCl$, $HBr$, and $HI$ are strong acids).

How do the number of oxygen atoms and the inductive effect influence oxoacid strength?

1. For oxoacids with the same central atom, the molecule with more oxygens is more acidic ($H_2SO_4 > H_2SO_3$, $HClO_4 > HClO_3$, $HNO_3 > HNO_2$) due to greater electron withdrawal.
2. Highly electronegative terminal atoms pull electron density away from the $O\text{--}H$ bond (inductive effect), weakening the bond and increasing acidity ($HOCl > HOBr > HOI$).

Which six strong acids are explicitly listed in the notes to memorize for complete ionization?

Hydrochloric acid ($HCl$), hydrobromic acid ($HBr$), hydroiodic acid ($HI$), nitric acid ($HNO_3$), perchloric acid ($HClO_4$), and sulfuric acid ($H_2SO_4$).

What is the autoionization expression for water, and what is the value of $K_w$ at $25^\circ\text{C}$?

$H_2O(l) \rightleftharpoons H^+(aq) + OH^-(aq)$, with $K_w = [H^+][OH^-] = 1.0 \times 10^{-14}$. In pure water, $[H^+] = [OH^-] = 1.0 \times 10^{-7}\,\text{M}$.

How are $\text{pH}$ and $\text{pOH}$ defined mathematically, and what equation relates them at $25^\circ\text{C}$?

$\text{pH} = -\log[H_3O^+]$, $\text{pOH} = -\log[OH^-]$, and $\text{pH} + \text{pOH} = 14$.

What $\text{pH}$ criteria define acidic, neutral, and basic solutions at $25^\circ\text{C}$?

An acidic solution has $\text{pH} < 7$ ($[H^+] > 1.0 \times 10^{-7}\,\text{M}$); a neutral solution has $\text{pH} = 7$ ($[H^+] = 1.0 \times 10^{-7}\,\text{M}$); a basic solution has $\text{pH} > 7$ ($[H^+] < 1.0 \times 10^{-7}\,\text{M}$).

How do ionic bonds, covalent bonds, and polyatomic ionic compounds differ in their chemical bonding?

Ionic bonds form between metals and nonmetals through full electron transfer; covalent bonds form between nonmetals through electron sharing; polyatomic ionic compounds contain covalent bonds within the polyatomic ion and ionic bonds between the cation and anion (e.g., $KNO_3$ has ionic bonds between $K^+$ and $NO_3^-$, and covalent bonds between $N$ and $O$).