Solution Chemistry
Reactions
Gas Law
Bonding
Mixture of Topics
100

Number of moles of solute per liter of solution

molarity (M)

100

Acid +Base --> salt and this

water

100

1 atm = ____  mmHg

760


100

Three examples of hydrogen bonds

HO, HN,HF

100

face centered unit cell has this much atoms

4

200

Mathematical formula used for dilutions

M1V1=M2V2

200

Give one example of a strong acid and a strong base 

HCl or NaOH
200

T(K)=T(oC)+____

273.15

200
The weakest intermolecular force

LDF

200

Phase change from solid to gas

sublimation

300

Molarity of K+ Ion in 1M K3PO4 

3M

300

Reaction between strong acids and metals will always yield this gas

hydrogen gas (H2)

300
R constant in the ideal gas law (including unit)

0.08206 L.atm/mol.K

300

The strongest intermolecular forces

Ion-Ion Forces
300
In ideal gas law, distances between gas particles are considered this 

zero, negligible

400

Most chemical reactions can be classified into three categories: precipitation, acid-base, and this

Oxidation-Reduction Reactions (RedOx)
400

Oxidation of N2(g)

0

400

At STP, 1 mole of gas have a volume of this (include unit)

22.4 L

400

The point on the diagram where all three states meet is called this

triple point

400

The average kinetic energy of a gas particle is proportional to this only

temperature

500

This ion is always soluble in water

nitrate or chlorate

500

Oxidation of Mn in KMnO4

+7

500

PV=nRT can be rearranged to solve the density of gas

PV=dRT

500

at extremely high temperatures and pressures, this indicates the critical pressure and temperature

critical point

500

All else stays the same, as volume decreases, pressure will do this

increases

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