Aqueous solution
A solution where water is the solvent
Dissociation equation
Formulas/ reactions showing the separation of ionic salt in water by dissolving
Precipitate
Solid that “falls” out of solution
Spectator ions
Ions that remain in solution after the precipitate reaction has occurred.
In reeks reactions they may be soluble but do not change in oxidation
Neutralization reactions
Special type of double displacement reaction that involves a strong acid and a strong base to produce a salt and water in liquid form.
Naming acids steps:
Binary?
Oxyacid?
Binary: -hydro prefix, root of nonmetal element, is ending and acid
Oxyacid:-“ate” ions make “ic” acids
-“ite” ions make “ous” acids
Naming bases:
Cation+hydroxide
What makes a substance a strong acid or base?
Is dissociates completely
Ex: HCl—->H+(aq)+Cl-(aq)
Titration:
Laboratory technique used when performing a neutralization. Also used to determine the concentration of an unknown.
Do covalent substances dissolve?
Yes but don’t dissociate
Oxidation
The combining of oxygen with other elements (loss of electrons)
Reduction
The remaining of oxygen from a compound (gain of electrons)
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Molarity: concentration unit measured in Mol/L
Where are oxidation sign?
In front of number
Rules of oxidation numbers
Any elemental atom (Fe) or multiple of self (N2) is 0
An ions oxidation number is its charge
Hydrogen’s in +1 except in metal hydrides then it’s -1
Oxygens is -2
Surface tension
The inward force or pull which leads to minimize the surface area of a liquid
Solvation
Occurs when a solute dissolves
Electrolyte
Compounds that conduct an electrical current in an aqueous solution or molten state.
A strong electrolyte has a large fraction of solute that exist as ions
Reducing agent
A substance in a redox reaction that donates electrons; in the reaction, reducing agent is oxidized.
Oxidizing agent:
A substance in a redox reaction that accepts electrons, in the reaction, the oxidizing agent is reduced.
Sacrificial metal
Metal allowed to corrode in order to save another from corroding.
Transfers electrons to metal that has lost them
Salts
Ionic compounds consisting of an atom from an acid and a cation from a base.
Equivalence Point
The point in a titration where the number of moles of hydrogen ions is equal to the number of moles of hydroxide ions.
End point
The point in titration at which the indicator changes colour
What must happen in order to dissolve
The polar nature of water must be strong enough to overcome the attraction between ions in a compound.
Water is polar and attracted to other parts of molecules, causing them to separate.
Dipolar
Polar molecules attract one another, leads to a dipolar interaction between the positive region of water and the negative region of another. Weak compared to IMF
Standardization
The process of determining the exact concentration of a solution