Chapter 4 and 5

Concentration

how much of dissolved in a solution

Molarity

Moles of solute / liters of solyte

what does like dissolve like mean?

"Like dissolves like" is a rule of thumb in chemistry: substances with similar polarity tend to dissolve in each other. Polar solvents dissolve polar (and ionic) solutes, and nonpolar solvents dissolve nonpolar solutes.

What is the universal solvent

Water

water reacts with a lot of molecules

what is an electrolyte and what does it need

An electrolyte is a substance that produces an electrically conducting solution when dissolved in a polar solvent like water. It conducts electricity because it breaks apart (dissociates) into positively and negatively charged ions that can move freely through the solution.

• it needs charge and movement

  • Charged but not mobile (solid salt): no current.

  • Mobile but not charged (sugar water): no current.

  • Charged and mobile (salt water, molten salt): current flows.

  • This is why dissolving matters so much. Water does two jobs at once: it pulls ionic compounds apart into charged ions, and it gives those ions a liquid to move through.

what does it mean by a compound dissociating

Dissociation is when an ionic compound separates into its individual ions as it dissolves. The ions were already there in the solid crystal; dissolving just pulls them apart so they move independently in the solution.

What are strong electrolytes

Strong acids, strong bases and soluble salts

what are weak electrolytes

weak acids, weak bases and insoluable salts

what is a nonelectrolyte

does not dissociate in a solution

what are the two parts of an ionic compound

cation - positive

anion - negative

precipitation reaction

two soluable ionic compounds react to form an insoluble product known as a precipitate and another product

what is a double displacement

A double displacement reaction (also called a double replacement or metathesis reaction) is a reaction where two ionic compounds swap partners.

what is dillution

Dilution is the process of lowering a solution's concentration by adding more solvent (usually water). The amount of solute stays the same, but it spreads out through a larger volume, so each unit of volume contains less of it.

Soluble salts vs insoluble salts

Soluble salts dissolve in water in significant amounts, breaking apart into free ions. Insoluble salts dissolve so little that almost all of the solid stays intact, often settling out as a precipitate.

what is a salt

First, what is a salt?

• A salt is an ionic compound made of a cation (other than H⁺) and an anion (other than OH⁻ or O²⁻).

• Salts are often formed when an acid reacts with a base: HCl + NaOH → NaCl + H₂O.

• "Salt" does not only mean table salt. CuSO₄, KNO₃, CaCO₃, and AgCl are all salts.

What is an arrhenius acid and base

• arrhenius acid

  • a substance that produces H+ ions when dissolved in water

  • a strong affinity of water molecules

• arrhenius base

  • produces OH- ions when dissolved in water

how is strength of an acid/base relate to dissasociation

the stringer an acid/base the more it dissociates

what is a neutralization reaction

A neutralization reaction is a reaction between an acid and a base that produces a salt and (usually) water.

Strengths vs molarity

Strength and molarity describe two different things. Strength is about how completely an acid or base breaks into ions. Molarity is about how much of it is dissolved in a given volume. They are independent: a solution can be strong and dilute, or weak and concentrated.

two types of acids in a solution

• binary acid

  • hydrogen and a nonmetal

  • hydro - ic acid

• oxyacid

  • has hydrogen and an oxyanion (polyatomic anion with oxygens)

  • ate - ic acid

  • ite - ous acid

what are the strong acids

HCL, HBr, HI, HNO3, HCLO4, and H2SO4

So i brought no clean clothes

Strong bases

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Ba(OH)2, and Sr(OH)2

Little Nancy Kicked Ruby's Cat. Can Sally Bake?

Bronsted lowry acid

species that gives up a H+ to another substacne

a proton donor

Bonsted lowry base

a species that accepts H+ from another substance

Molecular equation

the normal equation we write

Total ionic equation

• shows how all ionic compounds dissociate into compoonet ions

• make sure charges are balanced

• dont seperate weak acids and bases

• dont seperate insoluable compounds

net ionic equation

• main reaction or charge in the overall requation when we remove the spectator ions

• no balancing

Acid base titrations

• technique used by sicentists to find out the necessary amount of acid/base required to neutralize an acid/base solution

• concentration of one solution used to find concentration of other solutions

What is the equivalence point and end point, and what’s the difference between them

• The equivalence point is the moment in a titration when the added titrant has exactly reacted with all of the analyte, in the correct mole ratio from the balanced equation.

• The endpoint is the moment you actually see a signal, usually an indicator changing color, and stop adding titrant. The equivalence point is the theoretical target; the endpoint is your experimental estimate of it.

oxidation numbers

charge of an atom would have if the electrons were transferred completely; not shared

oxidation state is assigned to each individual atom

oxidation numbers rules

• Free elements are 0 (Na, O₂, Cl₂, P₄)

• Monatomic ions equal their charge (Na⁺ = +1, O²⁻ = −2)

• The sum equals 0 in a neutral compound, or the ion's charge in a polyatomic ion

• Group 1 metals are +1, Group 2 metals are +2

• Fluorine is always −1

• Hydrogen is +1 with nonmetals, −1 with metals (NaH)

• Oxygen is −2, except −1 in peroxides (H₂O₂) and positive with fluorine (OF₂)

• Cl, Br, and I are −1, except when bonded to oxygen or a more electronegative halogen

• Solve for any remaining atom using the sum rule

• If rules conflict, the higher rule on this list wins

• An increase is oxidation; a decrease is reduction

Redox reactions

• transfer of electrons from one reactant to another

• loss of eletrons is oxidation, gain of electrons is reduction

• LEO the lion goes GER

reducing agent

if it loses elections and gets a more positive charge

oxidizing agent

if it gains electrons and gets a less positive charge

formula for presure

force/unit area

what is atmospheric pressure

result of gas molecules exerting pressure on their surroundings

what is barometer

device used to measure atmospheric pressure

what is a manometer

• pressure measuring device used to determine pressures close to atmospheric presser

• An open tube manometer there is mercury in the tube between the gas and atmn

manometer problems must be in mmHg

what does the gas laws depend on

• pressure

• volume

• number of moles

• temperature

what is an ideal gas and when is a gas most like an ideal gas

• theoretical gas made of tiny particles that move randomly and do not attract or push away from each other

• doesn’t exist

• most like ideal gas when low external pressure and high temperature

what does temperature have to be for the gas laws

kelvin

what units for ideal gas law

ATm

liters

moles

ideal gas constant

kelvin

STP

temp is 273

pressure is 1 atm

in this condutions 1 mol of gas is equal to 22.1414 L

partial gas pressure

pressure exerted by a gas whem more than one gas is in a container

Pa = Xa * Ptotal

Mole fraction

Xa = moles of A/Total moles

Daltons law of partial pressures

collecting gas over water

when collecting gas over water you must subtract the vapor pressure of water

effusion

the abikuty of molecules to flow from a container through a hole to the outside world or into another ocntainer'

the heavier the gas the slower the effuson rate

Kinestic molecular theory of gases

• describve behavior on an atomic level

• gases consist of particles

• constant libear motion

• average kinetic eneergy deepdns on temperature