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Chem > 10 > Flashcards

10 Flashcards

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1
Q

Hydration

A
  • positive ends of water molecule are attracted to negatively charged anions
  • negative ends are attracted to positively charged cations
  • this happens when water has salt or something in it
  • it breaks up INDIVIDUAL cation and anions
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2
Q

Solubility

A
  • ability of a substance to dissolve into a solvent
  • differences in solubilities of IONIC compounds in water depends on relative attractions of the ions for each other (forces hold the solid together) and attractions of ions for water molecules
  • all NITRATES are soluble in water
  • water can dissolve NONIONIC substances
  • in general, polar and ionic substances are expected to be more soluble in water than nonpolar substances
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3
Q

Solute

A

-substance being dissolved

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4
Q

Solvent

A

-substance dissolving the solute (water)

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5
Q

Electrical conductivity

A

-ability to conduct an electric current

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6
Q

Electrolyte

A

-substance that when dissolved in water produces a solution that can conduct electricity

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7
Q

Svante Arrhenius

A
  • believed that the conductivity of solutions arose from the presence of ions (how many ions they created in aqueous solutions)
  • believed acids provide a hydrogen ion (positive, H+) and are sour
  • believed bases provide a hydrogen ion (negative, OH-)
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8
Q

Strong Electrolytes

A
  • there are three classes : soluble salts, strong acids, strong bases
  • salt (cations and anions) separate in water
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9
Q

Strong Acids

A
  • when they are in water, virtually every molecule ionizes
  • sulfuric acid, nitric acid, and hydrochloric acids are aqueous and should be written like HCl(aq)
  • since strong acids completely dissociate into its ions, 100 molecules of HCl dissolved in water will created 100 H+ ions and 100 Cl- ions
  • H2SO4 says that this acid can produce 2 H+ ions per molecule when dissolved in water, but only the first H+ ion is completely broken down. The second H+ ion can be pulled off under certain conditions. Therefore, H2SO4 contains mostly H+ and H2SO4- ions.
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10
Q

Strong Bases

A
  • soluble ionic compounds
  • have hydroxide ion (OH-)
  • when in water, OH- ions separate and move independently
  • bitter and slippery
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11
Q

List of Strong Acids

A
  • HCl, hydrochloric
  • H2SO4, sulfuric
  • HBr, hydrobromic
  • HI, hydroiodic
  • HNO3, nitric
  • HClO4, perchloric
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12
Q

Weak Electrolytes

A
  • acetic acids is a weak acid

- ammonia is a weak base

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13
Q

Acetic Acids:

A
  • formula for acids are often written with acidic hydrogen atoms or atoms (produce H+ ions) first and non acidic hydrogens later
  • double arrow means that the reaction can occur in either direction
  • it is a weak acid
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14
Q

Weak Acid

A

-any acid that dissociate (ionizes) only to a slight extent in an aqueous solution

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15
Q

Weak Base

A
  • ammonia is one
  • resulting solution is a weak electrolyte (few ions are formed)
  • OH- ions are also formed
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16
Q

Nonelectrolytes

A
  • substances that dissolve in water but do not produce any ions
  • ethanol is one (molecules do not break up into ions)
  • table sugar (sucrose)
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17
Q

Molarity

A
  • number mol solute/liters of solution

- measure of concentration

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18
Q

Solubility rules:

A
  • all nitrates are soluble (NO3-)
  • all alkali metals and ammonium salts are soluble (NH4+) (first column)
  • all chlorides, bromides, and iodides are soluble except : Pb2+, Ag+, Hg2+
  • all sulfates (SO42-) are soluble except Pb2+, Ag+, Hg22+, Ca2+, Sr 2+, Ba2+
  • everything else is not soluble unless mr. william tells us otherwise
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19
Q

Spectator ions

A

things that don’t react

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20
Q

List of Strong Bases:

A
  • LiOH
  • NaOH
  • KOH
  • Ca(OH)2
  • SR(OH)2
  • Ba(OH)2
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21
Q

Three types of reactions

A
  • double displacement/precipitation reaction

- acid base reaction / water forming

22
Q

Double displacement/precipitation reaction:

A
  • characterized by AX + BY –> AY + BX

- switching partners

23
Q

Acid base reaction / water forming

A
  • acid and base combining
  • characterized by AX + BY –> AY + BX, like double displacement
  • creates water
24
Q

net ionic equation

A

crossing out spectator ions

25
Q

formal equation

A

you show the switching

26
Q

complete ionic eqution

A

formal with adding together

27
Q

oxidation

A

loss of electrons

28
Q

reduction

A

gain of electrons

positive charge getting lost

29
Q

oxidation state

A

charge on the atom, works only for ionic not molecular

30
Q

rules of oxidation state

A
  1. everything by itself in natural occurring state has a O charge
  2. oxygen COMPOUNDS are always 2- EXCEPT in peroxide (H2O2) where it is 1-
  3. hydrogen is always 1+ unless you are told otherwise
  4. everything else can be deduced from what you know
31
Q

N

A

can be expressed as 10 to the X

ex:
- 100 is x = 2
- 10 is x = 1

32
Q

using Log

A 
LogN = x
ex:
-65 is x = ?
-Log65 = x
= 1.81
33
Q

[A]

A

concentration of “A’ in molarity
ex:
[H+] is the concentration of H+ in molarity

34
Q

to find the pH using log

A 
pH = -log[H+] 
ex:
1. find concentration of H+ 
2. the concentration of H+ is the same as HCl  which is 6
3. [H+] is 6
4. plug in
35
Q

what is pH typically between

A

0 (acidic) - 14 (basic)

36
Q

what is H30+

A
  • it is the same as H+
  • H+ is just a proton and very small
  • H+ then just latches onto H20, creating H30+
37
Q

in the classic titration lab..

A

we are just adding NaOH to get HCl nneutralized

-at a 1 to 1 ratio

38
Q

using molarity to find moles

A
  • n = mv
  • na = mava
  • nb= mbvb
  • since na and nb are equal: mava=mbvb
  • in the classic titration lab we are trying to find ma
39
Q

Dilution

A
  • adding water to achieve molarity desired for particular solution
  • moles of solute after dilution = moles of solute before dilution
40
Q

Precipitation Reaction / Double displacement

A
  • when two solutions are mixed, an insoluble substance sometime forms / a solid forms and separates from the solution
  • remember: when ionic compounds dissolve in water, the resulting solution contains the separated ions
41
Q

slightly soluble

A
  • tiny amount of solid that dissolve is not noticeable

- the solid appears to be insoluble to the naked eye

42
Q

Formula equation

A
  • shows reactants and products of reaction

- does not give correct picture of what actually occurs in the solution

43
Q

complete ionic equation

A
  • all substances that are strong electrolytes are represented as ions
  • reveals that only some of the ions participate in the reaction
  • spectator ions are written as separate ions
  • but solids are not written as separate ions
44
Q

net ionic equation

A

-only shows solution components directly involved in the reaction

45
Q

Solving Stoichiometry Problems for Reactions in Solutions

A
  • identify species present in the combined solution, and determine what reaction occurs
  • write balanced net ionic equation for reaction
  • calculate moles of reactants
  • determine which reactant is limiting
  • calculate moles of product or products
  • convert to grams or other units
46
Q

indicator

A
  • equivalence point or stoichiometric point is marked by this
  • it changes color at the equivalence point
47
Q

endpoint

A

-the point where the indicator actually changes color

48
Q

Requirements for a successful titration

A
  • the exact reaction between titrant and analyte must be known (and rapid)
  • the stoichiometric point must be marked accurately
  • volume of titrant required to reach stoichiometric point must be known accurately
49
Q

covalent bonds

A

-electrons are shared

50
Q

cations

A

positive

51
Q

anions

A

negative

52
Q

electrolytes

A

substances that conduct electricity when dissolved in whatever

Chem (14 decks)

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