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Flashcards in this deck (63)

  • What is a titration?

    An experimental technique to determine the concentration of an unknown solution by combining it with a solution of known concentration.

    chemistry titration

  • What is a titrant?

    The solution of known concentration used in titrations, often placed in a burette.

    chemistry titration

  • What is an analyte?

    The substance being analyzed in a titration.

    chemistry titration

  • What is the equivalence point?

    The point in titration where the titrant completely reacts with the analyte.

    chemistry titration

  • What is a redox titration?

    A titration method that involves oxidation-reduction reactions to determine the concentration of an unknown solution.

    chemistry redox

  • When can redox titrations not require an indicator?

    Some redox titrations use solutions like KMnO₄, where color changes indicate the equivalence point.

    chemistry redox

  • What indicates the equivalence point in a titration using KMnO₄?

    The appearance of a faint pink color in a colorless analyte.

    chemistry redox

  • What is the theoretical yield?

    The maximum amount of product expected from a reaction under perfect conditions.

    chemistry stoichiometry

  • What is the actual yield?

    The amount of product actually obtained from a reaction.

    chemistry stoichiometry

  • How is percent yield calculated?

    Percent Yield = (Actual Yield / Theoretical Yield) * 100.

    chemistry stoichiometry

  • In a neutralization reaction, when an acid and a base are mixed, they undergo a reaction. For example, with baking soda and vinegar.

    chemistry reactions

  • The type of chemical reactions include: Acid-base, redox and others.

    chemistry reactions

  • What is an acid according to the Arrhenius concept?

    An acid is something that gives up a proton.

    chemistry acids

  • What characterizes a base in the Arrhenius concept?

    A base is something that forms hydroxide when added to water.

    chemistry bases

  • What is a Bronsted-Lowry acid?

    A Bronsted-Lowry acid is a proton donor.

    chemistry bronsted-lowry

  • What does a Bronsted-Lowry base do?

    A Bronsted-Lowry base is a proton acceptor.

    chemistry bronsted-lowry

  • In a Bronsted-Lowry acid-base reaction, a transfer of one or more protons occurs.

    chemistry bronsted-lowry

  • What are the typical products of a Bronsted-Lowry acid-base reaction?

    The products are often water and an ionic compound (salt).

    chemistry bronsted-lowry

  • What do oxidation-reduction (redox) reactions involve?

    They involve the transfer of one or more electrons.

    chemistry redox

  • What is an example of a redox reaction?

    The rusting of iron is an example.

    chemistry redox

  • In redox reactions, what happens to the substance that loses electrons?

    It is oxidized.

    chemistry redox

  • In redox reactions, what happens to the substance that gains electrons?

    It is reduced.

    chemistry redox

  • The acronym LEO stands for Loss of Electrons: Oxidized.

    chemistry redox

  • The acronym GER stands for Gain of Electrons: Reduced.

    chemistry redox

  • What are oxidation numbers used for?

    They identify the oxidized and reduced species in a redox reaction.

    chemistry oxidation_numbers

  • What is the oxidation number of atoms by themselves?

    Atoms by themselves have oxidation numbers of zero.

    chemistry oxidation_numbers

  • What is the common oxidation number of oxygen in compounds?

    Oxygen most often has an oxidation number of -2.

    chemistry oxidation_numbers

  • What is the oxidation number of hydrogen when bonded to a nonmetal?

    Hydrogen is +1 when bonded to a nonmetal.

    chemistry oxidation_numbers

  • What is the oxidation number of fluorine?

    Fluorine always has an oxidation number of -1.

    chemistry oxidation_numbers

  • When something gains more electrons, it becomes negative and is reduced in number.

    chemistry redox

  • When something loses electrons, it becomes positive and its number increases.

    chemistry redox

  • What is the electron-transfer process in redox reactions?

    Electrons are transferred from the oxidized to the reduced species.

    chemistry redox

  • To track electron transfer in a redox reaction, oxidation numbers are assigned to each atom.

    chemistry oxidation_numbers

  • The oxidation number of oxygen in H2O2 is -1.

    chemistry oxidation_numbers

  • What is the oxidation number of hydrogen when bonded to a metal?

    Hydrogen is -1 when bonded to a metal.

    chemistry oxidation_numbers

  • In neutral compounds, the sum of all oxidation numbers is zero.

    chemistry oxidation

  • For a polyatomic ion, the sum of all oxidation numbers equals the charge.

    chemistry oxidation

  • What are oxidizing agents?

    Substances that contain elements that accept electrons (becoming more negative).

    chemistry oxidation

  • What are reducing agents?

    Substances that contain elements that donate electrons (becoming more positive).

    chemistry oxidation

  • Oxidizing and reducing agents are ALWAYS reactants, NEVER products!

    chemistry oxidation

  • In aqueous acid-base reactions, water can behave like an acid and donate a proton.

    chemistry acid-base

  • What is a monoprotic acid?

    H₂SO₄

    CH₃COOH

    H₃PO₄

    HCl
    chemistry acids

  • What is a diprotic acid?

    H₃PO₄

    H₂SO₄

    HCl

    CH₃COOH

    chemistry acids

  • What characterizes a triprotic acid?

    CH₃COOH

    H₃PO₄

    H₂SO₄

    HCl

    chemistry acids

  • What does a one-direction arrow in reactions indicate?

    It indicates 100% completion and must involve a strong acid or base.

    chemistry reactions

  • What does a double arrow in reactions indicate?

    It indicates a weak acid-base reaction that doesn't fully dissociate.

    chemistry reactions

  • What are electrolytes?

    Compounds that easily dissociate into ions and conduct electricity.

    chemistry electrolytes

  • What are nonelectrolytes?

    Compounds that do not dissociate into ions and hence don't conduct electricity.

    chemistry electrolytes

  • Net ionic equations with weak electrolytes should not include them as they cannot be represented as ions; they stay in their molecular form.

    chemistry equations

  • Weak electrolytes stay in their molecular form and do not easily dissociate into ions in reactions.

    chemistry equations

  • What can be done to measure other strong electrolytes?

    Mesifying can be performed using electrical conductivity.

    chemistry electrolytes

  • What observable characteristic defines weak and strong acids?

    Weak acids do not fully dissociate, while strong acids do.

    chemistry acids

  • What denotes strong acids and bases?

    One-direction arrows denote strong acids or bases in reactions.

    chemistry acids-bases

  • Identify the correct description of strong acids.

    Strong acids fully dissociate in solution.

    chemistry acids

  • Identify the correct description of weak acids.

    Weak acids partially dissociate in solution.

    chemistry acids

  • What is vapor pressure?

    It is the pressure exerted by vapor particles above a liquid.

    chemistry vapor_pressure

  • How does a nonvolatile solute affect vapor pressure?

    It lowers vapor pressure by blocking solvent molecules from reaching the surface.

    chemistry vapor_pressure

  • What occurs to the boiling point when a nonvolatile solute is added?

    The boiling point of the solvent is raised.

    chemistry boiling_point

  • What must vapor pressure reach for a liquid to boil?

    It must reach atmospheric pressure.

    chemistry boiling_point

  • What happens to boiling point when you add 20 grams of salt to 5 liters of water?

    It will boil at 100.04° C instead of 100° C.

    chemistry boiling_point

  • How does a nonvolatile solute affect the freezing point?

    It lowers the freezing point of the solvent.

    chemistry freezing_point

  • When a substance freezes, its molecules become very organized. Adding a solute prevents this organization, resulting in a lower freezing point required to force organization. Thus, the freezing point is lowered when a nonvolatile solute is added.

    chemistry freezing_point

  • What is the effect of adding a nonvolatile solute to a solvent?

    Lowers vapor pressure

    Lowers boiling point

    Lowers freezing point

    Raises boiling point

    Raises vapor pressure

    Does not affect freezing point

    chemistry solutions
Study Notes

Titrations

  • Titration: Experimental technique combining a known concentration solution (titrant) with an unknown concentration solution (analyte).
  • Analyte: Substance being analyzed.
  • Equivalence Point: The point at which the titrant completely reacts with the analyte.

Redox Titrations

  • Redox Reaction: Utilized for determining the concentration of unknown solutions.
  • Indicator: Some titrations do not require it; for example, using KMnO₄ with a colorless analyte shows a faint pink at the equivalence point.

Stoichiometric Mixture

  • Theoretical Yield: Expected amount of product in perfect conditions.
  • Actual Yield: Amount produced in practice.
  • Percent Yield: \( ext{Percent Yield} = rac{ ext{Actual Yield}}{ ext{Theoretical Yield}} imes 100 \)

Types of Chemical Reactions

Acid-base Reactions

  • Mixing an acid and a base results in a neutralization reaction.
Strong Acid Strong Base Weak Acid Weak Base
HCl NaOH HCOOH NH₃
HNO₃ KOH CH₃COOH (CH₃)₂NH
H₂SO₄ Ca(OH)₂ HF CH₃NH₂
HClO₄ LiOH NH₄OH
Ba(OH)₂ Memorize

Acid & Base Concepts

Arrhenius Concept

  • Acid: Gives up a proton.
  • Base: Forms hydroxide in water.

Bronsted-Lowry Concept

  • Acid: Proton donor.
  • Base: Proton acceptor.

Oxidation-Reduction (Redox) Reactions

  • Involve electron transfer.
  • Example: Rusting of iron forms iron oxide.
  • LEO (Loss of Electrons: Oxidized) GER (Gain of Electrons: Reduced).
  • Oxidation numbers help track electron transfers.

Oxidation Number Rules

  1. Atoms alone = 0.
  2. Charge equals oxidation number.
  3. Oxygen = -2 (except in H₂O₂: -1).
  4. Hydrogen = +1 (to nonmetals), -1 (to metals).
  5. Fluorine = -1.

Agents in Redox Reactions

  • Oxidizing Agent: Accepts electrons (gets more negative).
  • Reducing Agent: Donates electrons (gets more positive).

Acid Types

Monoprotic Acid

  • Example: HCl (strong acid).

Diprotic Acids

  • Example: H₂SO₄ → H⁺ + HSO₄⁻.

Triprotic Acid

  • Example: H₃PO₄ → H⁺ + H₂PO₄⁻.

Electrolytes

  • Electrolytes: Dissociate into ions and conduct electricity.
  • Nonelectrolytes: Do not dissociate and do not conduct electricity.

Vapor Pressure

  • Vapor pressure is the pressure of vapor above a liquid.
  • Nonvolatile Solute: Lowers vapor pressure by blocking solvent from the surface.

Boiling Point Elevation & Freezing Point Depression

  • Boiling point increases and freezing point decreases with added nonvolatile solutes due to intermolecular interactions.

Useful Visuals

Titrations and Redox Overview

Acids, Bases, and Electrolytes

Vapor Pressure and Phase Changes

Arrhenius and Bronsted-Lowry Concepts