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Chemistry 1 > Exam 4 > Flashcards

Exam 4 Flashcards

1
Q

Solute

A

a substance that’s present in a smaller amount

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2
Q

Solvent

A

present in greatest abundance

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3
Q

Aqueous solutions

A

solutions where water is the solvent

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4
Q

molarity

A

describes how much solute is dissolved per volume of solution

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5
Q

Equation for molarity

A

M= moles of solute/volume of solution L

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6
Q

Example: Calculate the molarity of a solution made by dissolving 23.4g of solution sulfate (Na2SO4) in enough water to form 125ml solution.

A

1.33 M Na2SO4 (reference notes for worked out problem)

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7
Q

True or False: The number of moles of solute remains the same in the concentrated and diluted forms of the solution

A

True

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8
Q

Dilution equation

A

(MB)(VB)=(MA)(VA) or (Mconc.)(Vconc.)= (Mdilute)(Vdilute)

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9
Q

Example: How many millimeters of 3.0 M H2SO4 are needed to make 450mL of 0.10 H2SO4?

A

V1=15mL

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10
Q

Example: How many grams of Cu are required to react with 1.5L of 0.10M AgNO3?

A

4.8g Cu

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11
Q

True or false: Ionic compounds don’t dissolve in water

A

False: Ionic compounds generally dissolve in water

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12
Q

What happens to ionic compounds in solutions?

A

ionic compounds don’t dissociate into ions in solution
(Example: NaCl (s)–> Na(aq) + Cl(aq)

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13
Q

True or False: Molecular compounds may dissolve in water

A

true

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14
Q

What happens to molecular compounds in solutions?

A

Molecular compounds don’t dissociate in solution
(Example: C12H22O11(l) –> C12H22O11(aq)

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15
Q

Are electrolytes strong or weak?

A

Electrolytes are both strong and weak

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16
Q

What are electrolytes?

A

compounds that break into ions when dissolved in water, and they conduct electricity

17
Q

What are nonelectrolytes?

A

compounds that don’t break into ions when dissolved in water, and don’t conduct electricity

18
Q

Compounds Containing the following Ions are generally soluble with NO exceptions

A

Li, Na, K, NH4, NO3, C2H3O2

19
Q

Compounds Containing the following Ions are generally soluble with exceptions

A

Cl, Br, I, SO4

20
Q

What are the exceptions for soluble ions: Cl, Br, and I

A

When these ions pair with Ag, Hg2, or Pb, the resulting compounds are insoluble

21
Q

What are the exceptions for soluble ions: SO4

A

When SO4 pairs with Sr, Ba, Pb, Ag, or Ca, the resulting compounds are insoluble

22
Q

Is NaCl soluble or insoluble?

A

Always soluble

23
Q

Is AgCl soluble or insoluble?

A

insoluble exception

24
Q

Compounds that are generally insoluble and their exceptions:

A

OH and S
Exceptions for both: Li, Na, K, NH4
Exception for S : Ca, Sr, Ba
Exception for OH: Ca, Sr, Ba however when OH is paired with these ions the result is slightly soluble

25
Q

Is Fe2S3 soluble or insoluble?

A

always insoluble

26
Q

Is CaS souble or insoluble?

A

soluble exception

27
Q

What happens when two water-soluble compounds are mixed?

A

it produces an insoluble product
(Example: Pb(NO3)2 (aq) + 2KI (aq) –> PbI2 (s) + 2KNO3 (aq)

28
Q

What do exchange/ double replacement reactions involve?

A

swapping ions in a solution (the cation from the first compound gets paired with the anion from the second compound) ( AX + BY –> AY + BX)

29
Q

Monoprotic acids

A

acids that ionize to form one H+ ion

30
Q

Diprotic acids

A

acids that ionize to form two H+ ions

31
Q

What are the 7 strong acids:
(all other acids are weak acids)

A
  1. hydroiodic (HI)
  2. hydrobromic (HBr)
  3. hydrochloric (HCl)
  4. Sulfuric (H2SO4)
  5. Nitric (HNO3)
  6. Chloric (HClO3)
  7. Perchloric (HClO4)
32
Q

Base

A

proton acceptors

33
Q

Strong bases:
(all other bases are weak bases)

A
  1. Alkali metals
  2. Strontium (Sr(OH)2)
  3. Calcium (Ca(OH)2
  4. Barium (Ba(OH)2)

Chemistry 1 (4 decks)

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