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Solutions and Solubility (5/10)

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

#1
Front (Question)

Solution definition

Back (Answer)

A homogeneous mixture • mixture: two substances • Homogeneous: evenly distributed • Heterogeneous: not evenly distributed (like a salad)

#2
Front (Question)

Dissoultion

Back (Answer)

Minority component (solute) reacts with solvent (majority component)

#3
Front (Question)

Dissolving

Back (Answer)

Like dissolves like -polar amino acids dissolve most readily in polar solvents (like water)

#4
Front (Question)

Saturation

Back (Answer)

extent which solute is dissolved in solvent -adding more solute than what solvent can handle to dissolve will precipitate

#5
Front (Question)

Supersaturation

Back (Answer)

Solute concentration>solute solubility must heat and cool slowly to keep all dissolved. If not, crystallized

#6
Front (Question)

Electrolyte

Back (Answer)

Ions conduct electricity in a solution

#7
Front (Question)

higher temperature for solids

Back (Answer)

higher solubility in endothermic reactions

#8
Front (Question)

Higher temperature for gases

Back (Answer)

lowers solubility for gases

#9
Front (Question)

Solubility rules: alkali metals

Back (Answer)

All soluble in water

#10
Front (Question)

Solubility rules: Nitrates

Back (Answer)

All soluble in water

#11
Front (Question)

Solubility rules: Halides

Back (Answer)

soluble in water except when combined with silver, lead, or mercury

#12
Front (Question)

Solubility rules: Sulfates

Back (Answer)

Souble in water except when combined with calcium, silver, lead, etc

#13
Front (Question)

Solubility rules: Carbonate, phosphate, sulfide

Back (Answer)

Insoluble except when combined with sodium carbonate or ammonium phosphate

#14
Front (Question)

Solubility rules: Hydroxides and metal oxides

Back (Answer)

Insoluble except if combined with alkali metals

#15
Front (Question)

Molarity

Back (Answer)

moles of solute/Liters of solution

#16
Front (Question)

Molality

Back (Answer)

Moles of solute/Kg of solvent

#17
Front (Question)

High concentration of solute

Back (Answer)

Impacts volume Molarity does not equal molality

#18
Front (Question)

Colligative properties

Back (Answer)

Properties changing solely with the concentration of solute in solution

#19
Front (Question)

Normality

Back (Answer)

Equivalents of solute/ Liters of solution

#20
Front (Question)

Calculating normality

Back (Answer)

(molarity of acid) x (acidic protons per molecule) molarity of base) x (hydroxide ions per molecule

#21
Front (Question)

Solubility equilibria

Back (Answer)

balance between reactant and balanced species

#22
Front (Question)

Ksp expression

Back (Answer)

Product ions only high value = large concentration of dissolved ions (high solubility)

#23
Front (Question)

Insolubility

Back (Answer)

No compound is truly insoluble

#24
Front (Question)

Molar solubility

Back (Answer)

Ksp/[cation] = [anion] number of moles that need to dissolved for the solution to be saturated