Chemical Equilibrium Concepts

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Questions and Answers

Which factor does NOT affect the position of equilibrium in a chemical reaction?

  • Pressure
  • Concentration of reactants
  • Color of the reactants (correct)
  • Temperature

Le Chatelier's Principle states that a change in pressure promotes a shift in equilibrium to favor the reactants.

False (B)

What is the formula for calculating molarity?

M = mol/L

According to Le Chatelier's Principle, a system at equilibrium will shift to counteract the effect of a change in __________.

<p>conditions</p> Signup and view all the answers

Match each action with its corresponding effect on equilibrium:

<p>Increasing concentration of products = Shift towards reactants Decreasing pressure = Shift towards more gas molecules Increasing temperature for an endothermic reaction = Shift towards products Adding a catalyst = No shift in equilibrium position</p> Signup and view all the answers

How can you speed up the process of dissolving a solid in a liquid?

<p>Increase the surface area of the solid (C)</p> Signup and view all the answers

A neutralization reaction always produces salts and water.

<p>True (A)</p> Signup and view all the answers

What does the term 'collision theory' refer to in the context of chemical reactions?

<p>It explains how reactants must collide with sufficient energy and proper orientation to react.</p> Signup and view all the answers

What is the molarity of SO2Cl2 in the flask?

<p>0.100 M (D)</p> Signup and view all the answers

Which direction will the reaction proceed to establish equilibrium?

<p>Forward direction (C)</p> Signup and view all the answers

A solution that contains the maximum amount of solute is described as unsaturated.

<p>False (B)</p> Signup and view all the answers

Define what a solute is.

<p>A solute is the substance that is dissolved in a solvent to form a solution.</p> Signup and view all the answers

The reaction quotient, Q, is calculated using concentrations expressed in _____ per liter.

<p>moles</p> Signup and view all the answers

Match the solution type with its definition:

<p>Saturated = Contains maximum solute at given temperature Unsaturated = Contains less solute than it could hold Supersaturated = Contains more solute than a saturated solution Electrolyte = Conducts electricity when dissolved in water</p> Signup and view all the answers

What oxygen-containing compound is involved in the equilibrium reaction?

<p>SO2 (D)</p> Signup and view all the answers

The solubility of solids increase with temperature.

<p>True (A)</p> Signup and view all the answers

Explain how agitation affects solubility.

<p>Agitation increases the contact and collision frequency between solute and solvent particles, thus enhancing dissolution.</p> Signup and view all the answers

Which of the following is a binary acid?

<p>HCl (D)</p> Signup and view all the answers

A substance that does not conduct electricity when dissolved in water is called a _____ solute.

<p>nonelectrolyte</p> Signup and view all the answers

At what temperature does a supersaturated solution of potassium nitrate occur?

<p>75°C (B)</p> Signup and view all the answers

Hydrobromic acid is represented by the formula HBr.

<p>True (A)</p> Signup and view all the answers

What is the molar concentration of aluminum sulfate if the sulfate ion concentration is 0.545 M?

<p>0.182 M</p> Signup and view all the answers

The reaction remains constant and does not change over time in a saturated solution.

<p>True (A)</p> Signup and view all the answers

The strong base potassium hydroxide is represented by the formula ______.

<p>KOH</p> Signup and view all the answers

Calculate the molarity of Cl2 in the flask.

<p>0.016 M</p> Signup and view all the answers

Match the acid to its correct formula:

<p>Nitric acid = HNO3 Sulfuric acid = H2SO4 Hydrochloric acid = HCl Phosphoric acid = H3PO4</p> Signup and view all the answers

When calculating molarity, you divide the number of _____ by the volume of the solution in liters.

<p>moles of solute</p> Signup and view all the answers

Which acid is formed when one H+ ion is added to the sulfate ion?

<p>H2SO4 (B)</p> Signup and view all the answers

All strong acids have strong conjugate bases.

<p>False (B)</p> Signup and view all the answers

Name the acid represented by the formula H2SO3.

<p>Sulfurous acid</p> Signup and view all the answers

The formula for acetic acid is ______.

<p>CH3COOH or HC2H3O2</p> Signup and view all the answers

Which of the following is NOT classified as a strong acid?

<p>CH3COOH (D)</p> Signup and view all the answers

The chemical formula for hydroiodic acid is HI.

<p>True (A)</p> Signup and view all the answers

What is the oxidation state of sulfur in sulfuric acid (H2SO4)?

<p>6</p> Signup and view all the answers

Match the following acids with their common names:

<p>H3PO4 = Phosphoric acid HNO2 = Nitrous acid H2CO3 = Carbonic acid HCl = Hydrochloric acid</p> Signup and view all the answers

Which reaction is favored by an increase in temperature?

<p>Endothermic reaction (A)</p> Signup and view all the answers

The addition of a catalyst will change the position of the equilibrium.

<p>False (B)</p> Signup and view all the answers

What effect does an increase in pressure have on the concentration of reactants if the forward reaction is favored?

<p>The concentration of reactants will decrease.</p> Signup and view all the answers

In a heterogeneous equilibrium expression, _______ are not included.

<p>solids</p> Signup and view all the answers

Match the following equilibria symbols with their meanings:

<p>Kc = Equilibrium constant using molar concentrations Kp = Equilibrium constant using partial pressures Ksp = Solubility product Ka = Acid dissociation constant</p> Signup and view all the answers

What condition indicates the system is at equilibrium?

<p>Q = K (A)</p> Signup and view all the answers

A decrease in temperature favors the endothermic reaction.

<p>False (B)</p> Signup and view all the answers

What does the reaction quotient Q represent?

<p>The ratio of the concentrations or partial pressures of products over reactants at any state.</p> Signup and view all the answers

The expression for Kc in the reaction aA + bB ⇄ cC + dD is __________.

<p>Kc = [C]^c[D]^d / [A]^a[B]^b</p> Signup and view all the answers

Which of the following affects both forward and reverse reactions equally?

<p>Adding a catalyst (B)</p> Signup and view all the answers

Kc can be calculated for reactions only at equilibrium.

<p>False (B)</p> Signup and view all the answers

In the reaction N2(g) + 3H2(g) ⇄ 2NH3(g), what is the expression for Kc?

<p>Kc = [NH3]^2 / ([N2][H2]^3)</p> Signup and view all the answers

If Q < K, the reaction will proceed _______ to reach equilibrium.

<p>forward</p> Signup and view all the answers

Match the following reactions with their equilibrium expressions:

<p>H2(g) + I2(g) ⇄ 2HI(g) = Kc = [HI]^2 / ([H2][I2]) CaCO3(s) ⇄ CaO(s) + CO2(g) = Kp = [PCO2] PbI2(s) ⇄ Pb+2(aq) + 2I-(aq) = Ksp = [Pb+2][I-]^2 Fe(OH)3(s) ⇄ Fe+3(aq) + 3OH-(aq) = Ksp = [Fe+3][OH-]^3</p> Signup and view all the answers

What happens to equilibrium when the concentration of reactants is increased?

<p>The equilibrium shifts to the right. (C)</p> Signup and view all the answers

If the concentration of products is decreased, the equilibrium will shift to the left to produce more products.

<p>False (B)</p> Signup and view all the answers

What does Le Chatelier's principle state about equilibrium when a system is stressed?

<p>It will shift to counteract the stress.</p> Signup and view all the answers

An increase in _____ shifts the equilibrium towards the side with fewer moles in gaseous reactions.

<p>pressure</p> Signup and view all the answers

Match the changes in reaction conditions with their effects on equilibrium:

<p>Increasing temperature = Favors the endothermic reaction Decreasing temperature = Favors the exothermic reaction Increasing reactant concentration = Shifts equilibrium to the right Increasing product concentration = Shifts equilibrium to the left</p> Signup and view all the answers

The concentration of Cl− ions in a 0.035 M solution of CaCl2 is 0.070 M.

<p>True (A)</p> Signup and view all the answers

In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if SO3 concentration is decreased?

<p>Equilibrium shifts to produce more SO3. (C)</p> Signup and view all the answers

What is the concentration of K+ ions in a solution made from 7.5 g of K2S in 250 mL?

<p>0.09 M</p> Signup and view all the answers

In an exothermic reaction, increasing the temperature favors the forward reaction.

<p>False (B)</p> Signup and view all the answers

What type of reaction is favored when the temperature is decreased?

<p>Exothermic reaction</p> Signup and view all the answers

In the dissociation of Al2(SO4)3, the ratio of aluminum ions to sulfate ions is ___.

<p>2:3</p> Signup and view all the answers

Match the following ionic compounds to their respective ion concentrations:

<p>CaCl2 = 2 Cl− CuCl3 = 3 Cl− K2S = 2 K+ and 1 S2− Na3PO4 = 3 Na+ and 1 PO4^3−</p> Signup and view all the answers

If the concentration of a reactant decreases, the equilibrium will shift to produce more _____ of that reactant.

<p>reactants</p> Signup and view all the answers

When preparing a standard solution, what is the purpose of wetting the pipette?

<p>To remove any residues from the pipette (C)</p> Signup and view all the answers

What effect does adding heat to an endothermic reaction have on equilibrium?

<p>It shifts the equilibrium to the right. (B)</p> Signup and view all the answers

Match the following reactions to their conditions:

<p>N2(g) + 3H2(g) ⇌ 2NH3(g) ΔH=−92 = Exothermic reaction Increasing reactants in a reversible reaction = Shifts towards products Increasing products in a reversible reaction = Shifts towards reactants Pressure increases in gaseous reactions = Shifts to fewer moles</p> Signup and view all the answers

Students should discard the solution used to wet the pipette into the beaker provided or down the sink.

<p>True (A)</p> Signup and view all the answers

When pressure is increased in a gaseous reaction, the equilibrium shifts to the side with more moles.

<p>False (B)</p> Signup and view all the answers

What is the concentration of sulfate ions in a 0.500 M solution of sodium phosphate?

<p>0 M</p> Signup and view all the answers

The final step in preparing a diluted solution is to ___ the flask.

<p>invert</p> Signup and view all the answers

What happens to the yield of ammonia when the temperature is decreased in the reaction N2(g) + 3H2(g) ⇌ 2NH3(g)?

<p>The yield increases.</p> Signup and view all the answers

Match the process with its description:

<p>Dilution = Reducing concentration by adding more solvent Dissociation = Separation of soluble compounds into ions Stoichiometry = Calculating quantities in reactions Pipetting = Transferring precise volumes of liquid</p> Signup and view all the answers

In a reversible reaction, if more _____ are added, the equilibrium shifts toward the products.

<p>reactants</p> Signup and view all the answers

If the concentration of calcium ions is 0.035 M in CaCl2, what is the total concentration of chloride ions?

<p>0.070 M (D)</p> Signup and view all the answers

What best describes the outcome when the concentration of a product is increased?

<p>The equilibrium shifts to the left. (D)</p> Signup and view all the answers

If the water exceeds the marked volume during dilution, the dilution must be redone.

<p>True (A)</p> Signup and view all the answers

What ion concentrations must be calculated when determining ion compositions in a compound like sodium phosphate?

<p>Sodium ion and phosphate ion concentrations</p> Signup and view all the answers

When water is added to dissolve K2S, the resulting solution has concentrations of ___ for K+ and S2−.

<p>0.09 M for K+, 0.03 M for S2−</p> Signup and view all the answers

What is the correct way to express a molarity of 1.00 M?

<p>One point oh oh molar (B), 1.00 molar (C)</p> Signup and view all the answers

The molarity of a solution is calculated based on the volume of pure water used to prepare the solution.

<p>False (B)</p> Signup and view all the answers

What is Avogadro's Number?

<p>6.022 x 10^23</p> Signup and view all the answers

When calculating molarity, you must convert grams to __________ first.

<p>moles</p> Signup and view all the answers

What happens to the equilibrium when pressure is increased?

<p>It favors the side with fewer gas molecules. (B)</p> Signup and view all the answers

Match the compound to its molar mass:

<p>NaCl = 58.44 g/mol KMnO4 = 158.0 g/mol C6H12O6 = 180.0 g/mol H2SO4 = 98.08 g/mol</p> Signup and view all the answers

Which of the following is true when temperature decreases in an exothermic reaction?

<p>The exothermic reaction is favored. (C)</p> Signup and view all the answers

Which of the following statements about molarity is true?

<p>Molarity is defined as moles of solute per liter of solution. (C)</p> Signup and view all the answers

A catalyst has a significant effect on the position of equilibrium in a chemical reaction.

<p>False (B)</p> Signup and view all the answers

What happens to the yield of NH3 when pressure is decreased in the reaction of N2 and H2?

<p>The yield of NH3 decreases.</p> Signup and view all the answers

A solution of 0.500 mol/L and 0.500 M represents the same concentration.

<p>True (A)</p> Signup and view all the answers

In the reaction A + B ⇋ C + D, if ΔH = -75 kJ, then the reaction is _____.

<p>exothermic</p> Signup and view all the answers

If you dissolve 80.0 grams of glucose in enough water to make 1.00 L of solution, what is its molarity?

<p>0.444 M</p> Signup and view all the answers

Match the following reactions with their respective changes in pressure:

<p>N2(g) + 3H2(g) ⇌ 2NH3(g) = Equilibrium shifts right with increased pressure 2SO2(g) + O2(g) ⇌ 2SO3(g) = Equilibrium shifts right with increased pressure A + B ⇋ C + D (endothermic) = Equilibrium shifts left with decreased pressure C + D ⇋ A + B (exothermic) = Equilibrium shifts right with decreased pressure</p> Signup and view all the answers

Molarity is abbreviated as __________.

<p>M</p> Signup and view all the answers

Match the following terms with their definitions:

<p>Molar Mass = Mass of one mole of a substance in grams Molarity = Moles of solute per liter of solution Dilution = Process of reducing concentration by adding more solvent Concentration = Amount of solute in a given volume of solution</p> Signup and view all the answers

When analyzing the equilibrium state in a rate-time graph, what does it indicate?

<p>The system is at equilibrium. (D)</p> Signup and view all the answers

How does an increase in temperature affect an endothermic reaction?

<p>It favors the forward reaction. (B)</p> Signup and view all the answers

The molarity of a solution can remain the same regardless of the solute's identity.

<p>True (A)</p> Signup and view all the answers

Increasing the concentration of reactants will always result in an increased rate of the forward reaction.

<p>True (A)</p> Signup and view all the answers

What volume of solution will result when 15.0 g of H2SO4 is dissolved to make a 0.200 M solution?

<p>0.375 L</p> Signup and view all the answers

What color change is observed when the temperature is decreased in the reaction involving NO2 and N2O4?

<p>The color becomes paler.</p> Signup and view all the answers

To perform a dilution calculation, the total volume created is based on the final __________ of the solution.

<p>volume</p> Signup and view all the answers

A sharp increase in reaction rate occurs with a change in _____.

<p>concentration</p> Signup and view all the answers

What is impacted by a decrease in pressure during a reaction?

<p>The equilibrium will shift to the side with more gas molecules. (B)</p> Signup and view all the answers

What is Keq and when can it be calculated?

<p>Keq is the equilibrium constant and can only be calculated when the system is at equilibrium.</p> Signup and view all the answers

Match the gases with their respective changes in equilibrium due to pressure changes:

<p>N2 + 3H2 ⇌ 2NH3 = Shift right with increased pressure 2SO2 + O2 ⇌ 2SO3 = Shift right with increased pressure 2NO2 ⇋ N2O4 = Shift left with increased pressure A + B ⇋ C + D = Depends on the number of gas molecules</p> Signup and view all the answers

Flashcards

Chemical Equilibrium

A state in a reversible reaction where the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products.

Le Chatelier's Principle

A principle that states that if a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress.

Equilibrium Constant (K)

The ratio of products to reactants at equilibrium, expressed as a constant value (K).

How does changing reactant concentration affect equilibrium?

Adding more reactants shifts the equilibrium towards the products. Removing reactants shifts the equilibrium towards the reactants.

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How does changing pressure affect equilibrium?

Increasing pressure favors the side of the reaction with fewer moles of gas. Decreasing pressure favors the side with more moles of gas.

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How does changing temperature affect equilibrium?

Increasing temperature favors the endothermic reaction. Decreasing temperature favors the exothermic reaction.

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Equilibrium Graph

A graphical representation of the concentrations of reactants and products over time, showing how equilibrium is reached.

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Exothermic Reaction

A reaction that releases heat (energy) to the surroundings. The enthalpy change (ΔH) is negative.

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What is a stress in an equilibrium system?

A stress on a system at equilibrium is a change in conditions that causes the system to shift to re-establish equilibrium.

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What's one stress on an equilibrium system?

The concentration of reactants or products changes.

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What's another stress on an equilibrium system?

The pressure changes, but only in reactions involving gases.

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What's one more stress on an equilibrium system?

The temperature changes, by adding or removing heat.

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What does Le Chatelier's Principle state?

Le Chatelier's Principle states that a system at equilibrium will shift to relieve stress.

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What happens to equilibrium when you increase reactant concentration?

If you increase the concentration of reactants, the equilibrium will shift to the right (towards products) to use up the extra reactants.

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What happens to equilibrium when you decrease reactant concentration?

If you decrease the concentration of reactants, the equilibrium will shift to the left (towards reactants) to replenish the reactants.

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What happens to equilibrium when you increase product concentration?

If you increase the concentration of products, the equilibrium will shift to the left (towards reactants) to use up the extra products.

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What happens to equilibrium when you decrease product concentration?

If you decrease the concentration of products, the equilibrium will shift to the right (towards products) to replenish the products.

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What happens to equilibrium when you increase temperature?

If you increase the temperature, the equilibrium will shift towards the endothermic reaction (the reaction that absorbs heat) to cool the system down.

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What happens to equilibrium when you decrease temperature?

If you decrease the temperature, the equilibrium will shift towards the exothermic reaction (the reaction that releases heat) to warm the system up.

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What happens to equilibrium when you increase pressure in a gaseous reaction?

If you increase the pressure in a gaseous reaction, the equilibrium will shift to the side of the reaction with fewer moles of gas to relieve the pressure.

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What happens to equilibrium when you decrease pressure in a gaseous reaction?

If you decrease the pressure in a gaseous reaction, the equilibrium will shift to the side of the reaction with more moles of gas to increase the pressure.

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What happens to the equilibrium constant after a stress is applied?

The equilibrium constant (Kc) remains the same even after a stress is applied, even though the concentrations of reactants and products change.

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Why is Le Chatelier's Principle important?

Le Chatelier's Principle is a valuable tool for understanding and predicting how changes in conditions affect chemical reactions at equilibrium.

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Solubility

The amount of solute that can dissolve in a given amount of solvent at a specific temperature.

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Unsaturated Solution

A solution that contains less solute than it can hold at a given temperature. It can still dissolve more solute.

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Saturated Solution

A solution that contains the maximum amount of solute that can dissolve at a given temperature. Any additional solute will not dissolve.

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Supersaturated Solution

A solution that contains more solute than it can hold at a given temperature. It's unstable and can precipitate out.

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Solvation

The process of dissolving solute particles in a solvent.

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Solute

Substance that dissolves in a solvent.

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Solvent

Substance that dissolves the solute. Usually the substance present in a larger amount.

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Electrolyte

A solution that conducts electricity because it contains dissolved ions.

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Nonelectrolyte

A solution that does not conduct electricity because it does not contain dissolved ions.

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Solution

A homogeneous mixture of two or more substances.

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Dissolution

The process of dissolving a solute in a solvent, resulting in a solution.

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Concentration

The amount of solute dissolved in a given amount of solvent.

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Molarity

A measure of the concentration of a solute in a solution, expressed as moles of solute per liter of solution.

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Kc

The equilibrium constant expressed in terms of molar concentrations.

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Kp

The equilibrium constant expressed in terms of partial pressures.

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Equilibrium Expression

The ratio of the products to the reactants, each raised to the power of their stoichiometric coefficients in the balanced chemical equation.

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Catalyst

A substance that speeds up the rate of a reaction without being consumed in the process. It lowers the activation energy.

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Concentration-Time Graph

The change in concentration of a substance over time.

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Mole-Time Graph

The change in the number of moles of a substance over time.

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Homogeneous Equilibrium

A reaction that involves only one phase (e.g., all gases or all liquids).

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Heterogeneous Equilibrium

A reaction that involves more than one phase (e.g., solids, liquids, and gases).

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Solubility Product Constant (Ksp)

The equilibrium constant for a solid dissolving in a solvent (e.g., a salt dissolving in water).

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Reaction Quotient (Q)

A measure of the relative amounts of reactants and products at any given time, not necessarily at equilibrium.

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Q < K

The point where the reaction proceeds forward to reach equilibrium because the concentration of the products is lower than that required for equilibrium.

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Molarity (M)

The concentration of a solution expressed as moles of solute per liter of solution (mol/L).

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Molality (m)

The number of moles of a substance per kilogram of solvent.

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Molar Mass

The mass of one mole of a substance.

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Converting grams to moles

The process of converting grams of a substance to moles.

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Converting moles to grams

The process of converting moles of a substance to grams.

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Molar Volume

The volume of solution containing one mole of solute.

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Standard Solution

A solution prepared by dissolving a known weight of solute in a specific volume of solvent.

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Stock Solution

The initial concentration of the solution before dilution.

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Volume of Stock Solution

The volume of concentrated solution taken to prepare a dilute solution.

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Final Concentration

The final concentration of the solution after dilution.

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Final Volume

The final volume of the solution after dilution.

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Dilution Equation

The relationship between the concentration and volume of the stock solution and the diluted solution.

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Ion Concentration

The concentration of a specific ion in a solution.

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Dissociation Factor

The number of ions that a particular compound dissociates into.

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Mole Ratio

The change in the number of moles of gaseous reactants and products in a balanced chemical equation.

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Pressure and Equilibrium (Increase)

An increase in pressure favors the reaction that reduces the number of gas molecules, shifting the equilibrium to the side with fewer moles.

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Pressure and Equilibrium (Decrease)

A decrease in pressure favors the reaction that increases the number of gas molecules, shifting the equilibrium to the side with more moles.

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Enthalpy Change (ΔH)

The enthalpy change of a reaction, indicating whether heat is released (exothermic) or absorbed (endothermic).

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Temperature and Equilibrium (Increase)

An increase in temperature favors the endothermic reaction, absorbing heat and shifting the equilibrium to the side that absorbs energy.

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Temperature and Equilibrium (Decrease)

A decrease in temperature favors the exothermic reaction, releasing heat and shifting the equilibrium to the side that releases energy.

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Catalyst and Equilibrium

A catalyst speeds up both the forward and reverse reactions equally, having no effect on the equilibrium position.

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Concentration Change and Equilibrium

A change in concentration of a substance will shift the equilibrium to relieve the stress by favoring the reaction that consumes the added substance.

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Pressure Change and Equilibrium

A change in pressure will affect the rates of both the forward and reverse reactions, with the effect being greater on the side with more gas molecules.

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What is concentration?

The concentration of a solution is the amount of solute dissolved in a given amount of solvent.

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What is Molarity?

Molarity is a unit of concentration that tells you how many moles of solute are dissolved in one liter of solution.

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How do you calculate Molarity?

To calculate molarity, divide the number of moles of solute by the volume of the solution in liters.

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What is a dissociation equation?

A dissociation equation shows how an ionic compound breaks apart into its individual ions when dissolved in water.

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How do you find the concentration of ions in solution?

When an ionic compound dissolves, the concentration of each ion is determined by the stoichiometric coefficients in the dissociation equation.

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What is a dilution?

A dilution is the process of decreasing the concentration of a solution by adding more solvent.

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What is the dilution equation?

The dilution equation states that the initial concentration times the initial volume is equal to the final concentration times the final volume.

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How do you perform a dilution?

To perform a dilution, you first measure out a specific volume of stock solution and transfer it to a volumetric flask.

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What is a volumetric flask?

A volumetric flask is a special flask designed to hold a precise volume of solution.

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What is the next step after transferring the stock solution to the volumetric flask?

After the stock solution is transferred, you then carefully add distilled water to the flask until the volume reaches the mark.

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What is the final step of the dilution process?

The final step is to mix the solution thoroughly by inverting the flask multiple times.

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How does the color of the diluted solution differ from the stock solution?

The color of the diluted solution will be lighter than the stock solution, as the concentration is now lower.

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Why is distilled water used in dilution?

It is important to use distilled water for dilution to avoid introducing impurities or contaminants to the solution.

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What equipment is used for accurate volume measurement in dilution?

To ensure accurate volume measurement, a pipette is used to transfer the stock solution and a volumetric flask is used for preparing the diluted solution.

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Why is it important to wet the pipette?

Wetting the pipette with a small amount of the solution before transferring the stock solution helps to prevent contamination and ensures accurate volume measurements.

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Strong Acids

Acids that completely ionize in solution, producing a high concentration of H+ ions.

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Weak Acids

They ionize less than 100% in solution, producing a lower concentration of H+ ions.

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Strong Bases

Bases that completely ionize in solution, producing a high concentration of OH- ions.

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Weak Bases

They ionize less than 100% in solution, producing a lower concentration of OH- ions.

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Conjugate Base

The species formed when an acid loses a proton (H+).

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Conjugate Acid

The species formed when a base gains a proton (H+).

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Reversible Reaction

A chemical reaction that can proceed in both the forward and reverse directions.

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Stress in an Equilibrium System

A change in conditions that causes a system at equilibrium to shift to re-establish equilibrium.

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How does increasing reactant concentration affect equilibrium?

Adding more reactants shifts the equilibrium towards the products.

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How does increasing temperature affect equilibrium?

Increasing temperature favors the endothermic reaction.

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Study Notes

Equilibrium Concepts

  • Chemical equilibrium is a state where the forward and reverse reaction rates are equal, resulting in no net change in concentration.
  • Le Chatelier's Principle: A change in a system at equilibrium causes a shift to counteract the change. This includes changes in concentration, temperature, and pressure (for gaseous systems).

Equilibrium Stress Factors

  • Concentration Changes: Adding reactants shifts equilibrium to products (forward). Adding products shifts equilibrium to reactants (reverse). Decreasing reactant concentration shifts equilibrium in the direction that produces more reactant (reverse). Decreasing product concentration shifts the equilibrium in the direction that produces more product (forward).

  • Temperature Changes: Increased temperature favors the endothermic reaction (absorbs heat). Decreased temperature favors the exothermic reaction (releases heat).

  • Pressure Changes: Increased pressure favors the side with fewer gas moles. Decreased pressure favors the side with more gas moles.

Equilibrium Constant

  • Equilibrium constant (K) is calculated using the concentrations (or partial pressures) of products and reactants at equilibrium.
  • Formula: K = [Products]coefficient / [Reactants]coefficient (Kc for concentrations, Kp for partial pressures)
  • Solids and liquids are excluded from equilibrium constant expressions.

Reaction Quotient (Q)

  • Q is calculated the same way as K but can be calculated for any set of conditions, not just equilibrium.
  • If Q < K, the reaction will proceed forward to reach equilibrium.
  • If Q > K, the reaction will proceed in reverse to reach equilibrium.
  • If Q = K, the system is already at equilibrium.

Molarity Calculations

  • Molarity (M) is moles of solute per liter of solution.
  • Formula: M = moles of solute / liters of solution.
  • Convert grams of solute to moles using molar mass.

Dilution Calculations

  • Dilution involves adding solvent to a solution to decrease its concentration.
  • Formula: M1V1 = M2V2 (where M1 and V1 are the initial concentration and volume, and M2 and V2 are the final concentration and volume).

Acid Nomenclature

  • Binary Acids: Hydro-(root)-ic acid (e.g., HCl – hydrochloric acid).
  • Oxyacids: (root)-ic or -(root)-ous acid, based on the polyatomic ion. (e.g., HNO3 – nitric acid, H2SO4 – sulfuric acid, HNO2 – nitrous acid)

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