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Flashcards in Solutions And Neutralizations Deck (27)
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1

Aqueous solution

A solution where water is the solvent

2

Dissociation equation

Formulas/ reactions showing the separation of ionic salt in water by dissolving

3

Precipitate

Solid that “falls” out of solution

4

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

5

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.

6

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

7

Naming bases:

Cation+hydroxide

8

What makes a substance a strong acid or base?

Is dissociates completely

Ex: HCl—->H+(aq)+Cl-(aq)

9

Titration:

Laboratory technique used when performing a neutralization. Also used to determine the concentration of an unknown.

10

Do covalent substances dissolve?

Yes but don’t dissociate

11

Oxidation

The combining of oxygen with other elements (loss of electrons)

12

Reduction

The remaining of oxygen from a compound (gain of electrons)

13

[]

Molarity: concentration unit measured in Mol/L

14

Where are oxidation sign?

In front of number

15

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

16

Surface tension

The inward force or pull which leads to minimize the surface area of a liquid

17

Solvation

Occurs when a solute dissolves

18

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

19

Reducing agent

A substance in a redox reaction that donates electrons; in the reaction, reducing agent is oxidized.

20

Oxidizing agent:

A substance in a redox reaction that accepts electrons, in the reaction, the oxidizing agent is reduced.

21

Sacrificial metal

Metal allowed to corrode in order to save another from corroding.

Transfers electrons to metal that has lost them

22

Salts

Ionic compounds consisting of an atom from an acid and a cation from a base.

23

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.

24

End point

The point in titration at which the indicator changes colour

25

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.

26

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

27

Standardization

The process of determining the exact concentration of a solution