Exam 2 Flashcards by Charlotte Tisch

Balanced Chemical Equation

Every atom on the reactant side ends up on the product side. Vice versa.

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Limiting Reagent

Reactant in the shortest supply limits the amount of product

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Excess Reagent

Reactant with excess amount after the reaction

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Percent Yield

Actual Yield/ Theoretical Yield * 100

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Solution

a homogenous mixture of two or more substances in which the ions or molecules intermingle freely

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Solvent

component of a solution present in the largest amount. It is the medium into which solutes are mixed or dissolved.

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Solute

Substance dissolved in the solvent.

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Concentration

Ratios between the solute, solvent, and solution.

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Dilute Solution

Has a small solute-solvent ratio

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Concentrated Solution

Has a large solute-solvent ratio

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Saturated Solution

Limit to how much solute can go into a solvent. When amount of solute added exceeds the limit, solution is saturated.

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Unsaturated Solution

Less solute present than required for saturation.

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Solubility and Temperature

Directly proportional. Increase temperature, increase solubility. Sometimes can dissolve MORE solute by heating the mixture. i.e. sugar water vs. simple syrup

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Supersaturated Solution

Solution that contains more solute than required for saturation at a given temperature. Usually unstable.

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Precipitation Reactions

Reactions that form precipitates

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Electrolyte

a compound that conducts electricity either in solution or in a molten state.

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Dissociation of Ionic Compound

Particles surrounded by solvent

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Nonelectrolytes

aqueous solutions of most molecular compounds that do not conduct electricity

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Hydrated

When a solute particle is surrounded by water

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Ionic Equation

All soluble strong electrolytes are written in dissociated form.

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Spectator Ions

Ions present in the reaction that do not participate.

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Net Ionic Equation

Ionic equation without spectator ions. Allow us to generalize/ predict future relations. Charges on each side MUST balance.

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Double Replacement Definition

a reaction of two salts in which the cations and the anions switch places.

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Types of Replacement (single or double) Rx

gas forming, precipitation, acid-base

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Gas forming rx

- Type of replacement | - One product is a gas

Precipitation Rx

- Type of replacement - use solubility rules - one product is a solid

Molarity

M | The number of moles of solute per liter of solution

Electrolyte

compound that conducts electricity in solution or molten state

Conductivity

get definition from Pam!

dissociated vs. dissolved

dissociate: break into ions dissolve: stay in lattice surrounded by H2O

Dissociate

break up into ions

Base

a substance that produces hydroxide in water

Ionization Reaction

reaction that forms ions from neutral reactants

Acid/Water Rx

Acid + H2O --> H3O+ + anion

Monoprotic Acid

Only 1 H+ per molecule of acid

Polyprotic Acid

Many H+ per molecule of acid

Base/Water Rx

Base + H2O --> BaseH+ + OH-

Binary Acids

binary compounds of hydrogen with nonmetals

Oxoacids

acids that contain H, O, and another element

Acid Salt

Salt of a partially neutralized polyprotic acid

Naming Oxoacids

ate --> -ic + acid | ite --> -ous + acid

Naming Binary Acids

'hydro' + nonmetal stem + '-ic' acid.

Naming Bases with O2-

(metal) oxide

Strong Acid Definition

acids that are strong electrolytes

Strong Acid List

``` HClO4- perchloric acid HCL- hydrochloric acid HBr- hydrobromic acid HI- hydroiodic acid HNO3 - nitric acid H2SO4 - sulfuric acid ```

Strong Base Definition

metal hydroxide that dissociates essentially 100% in water

Strong Bases in Group IIA

Ca(OH)2 - calcium hydroxide Sr(OH)2 - strontium hydroxide Ba(OH)2 - barium hydroxide Mg(OH)2 - magnesium hydroxide

weak electrolyte

substance that has low percent ionization or dissociation in water

weak acid

acid that has low % ionization in solutions, poor proton donor

weak base

base with low % ionization in solution, poor proton acceptor.

forward reaction

L -> R

reverse reaction

R -> L

dynamic equilibrium

- forward and reverse rx occurring at the same rate | - double arrows

chemical equilibrium

dynamic equilibrium of a chemical system

Coulomb's Law

F = k (q1q2)/(d^2)

ion charge to force

directly proportional

distance to force

inversely proportional

conjugate acid

a base that has gained a proton

conjugate base

an acid that has lost a proton

metal oxide

- strong bases | - deprotonate water to make 2OH-

metal hydroxide

metalOH

Molarity

moles of solute / liters of solution

weight percent

(mass solute/ mass solution) * 100

1 ppm

1 mg solute/kg of solution

1 ppb

1 ug (microgram) solute/kg of solution

When preparing solutions

add solid first, then liquid!

Molarity of hydrates

- use H2O in molar mass | - ignore after that

moles in stock =

moles final

moles =

Molarity * Volume (L)

M1V1 =

M2V2

Exam 2 Flashcards

(70 cards)