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Study Guide

Aqueous Solutions

Solutions are homogeneous mixtures of two or more substances
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The solute is dissolved in the solvent
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Mixture means that the solute and
the solvent retain their individual properties and that the solute and the solvent are only physically
combined
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Aqueous solutions are solutions in which the solvent is water
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Non-electrolytic solutions are solutions that cannot conduct electricity because the solutes do not
ions when dissolved in water
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Non-electrolyte is a solute that does not result to an electrolytic solution when dissolved in water
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Dissociation pertains to the separation of positive and negative ions in an
electrolyte
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No KNO3 is left undissociated
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Strong electrolytes
HCl
HNO3
HClO4
H2SO4
NaOH
Ba(OH)2
Ionic compounds

Weak electrolytes
CH2COOH
HF
HNO2
NH3
H2O

Non-electrolytes
(NH2)2CO
CH3OH
C2H5OH
C6H12O6
C12H22O11

Therefore, NaOH completely dissociates to form Na+ and OHNaOH → Na+(aq) + OH-(aq)
The (aq) subscript indicates that the ions are dissolved in water
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For weak electrolytes like HF, the process is reversible and eventually reaches and equilibrium state
in which the rate with which HF dissociate to H+ and F- ions is equal to the rate with which H+ and Fions recombine to form HF
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1

Reymon T
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The solubility guide below is a result of multiple experiments on solubility of substances since
there are no hard and fast rules for predicting the solubility
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2
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4
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Ammonium sulfate (NH4)2SO4
Lead iodide PbI2
Strontium nitrate Sr(NO3)2
Barium hydroxide Ba(OH)2
Sodium carbonate Na2CO3

Answers
1
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All compounds containing the ammonium ion is soluble
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2
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Compounds with iodide are soluble except when the cation is
Ag+, Hg2+, or Pb2+
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Strontium Nitrate is soluble
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There are no
exceptions
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Barium hydroxide is soluble
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5
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All compounds with alkali metal cations are soluble
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Write the balanced molecular equation for the reaction
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2
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2

Reymon T
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Write the net ionic equation by removing spectator ions
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Example 1
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Write the net ionic equation for the reaction
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Write the balanced molecular equation
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Check the equation for possible precipitate using the solubility guideline
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However,
compounds with silver are one of the exceptions which means that Ag2SO4 is a precipitate
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Write the ionic equation of the reaction
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Remove the spectator ions (ions that do not participate in the formation of the precipitate)
and write the net ionic equation
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2K+(aq) +SO4-2(aq) + 2Ag+(aq) + 2NO3-(aq)
Therefore, the net ionic equation is

→

Ag2SO4(s) + 2K+(aq) + 2NO3-(aq)

SO4-2(aq) + 2Ag+ → Ag2SO4(s)

Example 2
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Solution
Step 1
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Li2CO3 + CaCl2

→ 2LiCl + CaCO3

Step 2
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We can see from the solubility guideline that most carbonates are insoluble except compounds
with alkali metals and ammonium
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Mixing the solutions will form the precipitate CaCO3
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Write the ionic equation of the reaction
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Dela Cruz

→

CaCO3(s) + 2Li+(aq) + 2Cl-(aq)

Study Guide

Aqueous Solutions

Step 4
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2Li+(aq) +CO3-2(aq) + Ca 2+(aq) + 2Cl-(aq)

→

CaCO3(s) + 2Li+(aq) + 2Cl-(aq)

Example 3
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Solution
Step 1
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NaCl + KCH3COO → NaCH3COO + KCl
Step 2
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We can see that all of the reactants and products are soluble in water since all compounds
containing alkali metals (in this case potassium and sodium) are soluble compounds
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At this point, there is no need to write the ionic and net ionic equation for the reaction
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Dela Cruz



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