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GRADE 11 CHEMISTRY SOLUTIONS AND SOLUBILITY NOTES

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SCH3U1 Grade 11 Chemistry Unit 3 Solutions and Solubility Unit Test Study Notes
Effect of Temperature on Solubility
- every unique pure substance has its own unique solubility based on the types of bond
present
- units used to describe/measure solubility is: mass of solute/100mL of solvent
Solubility of Solid
- trend: solubility of solids increase as temperature increases
- energy is required to break apart bonds of solids when dissolved in water
- as temperature increases, there is more energy to break these bonds
SATP/STP: standard ambient temperature and pressure
S = soluble
SS = slightly soluble
I = insoluble
Solubility of Gases
- trend: solubility of gases decrease as temperature increases
- with more energy, the gas particles escape the solution
Solubility of Liquids
- trend: solubility of liquids is not affected by the temperature
- solute: liquid with less amount
- solvent: liquid with greater amount
Water
- universal solvent
- small size, highly polar nature, and the capacity to form hydrogen bonds makes water very
successful at dissolving solutes
- water has a permanent dipole
- the negative end is attracted to the positive end, causing a special type of attraction called
hydrogen bonding
Hydrogen Bonding
- any substance containing hydrogen and oxygen/fluorine/nitrogen
- doesn’t create an actual bond, uses strong intermolecular forces to create a force of
attraction
- hydrogen bonded compounds are likely to dissolve in water
Properties
- water is held together by covalent bonds which re stronger than hydrogen bonds
- however, the hydrogen bond is stronger than regular dipole-dipole attractions
- this results in higher boiling points because more energy is required to break apart these
bonds
- hydrogen bonds also result in higher surface tension
Volume/Volume Concentration (V/V) %
- volume of solute(mL)/volume of solution(mL) X 100%
Mass/Volume Concentration (m/V) %
- mass of solute(g)/mass of solution(mL) X 100%
Mass/Mass concentration (m/m) %
- mass of solute(g)/mass of solution(g) X 100%
Very Low Concentrations
- parts per million (ppm) = mass of solute/mass of solution X 106
- parts per billion (ppb) = mass of solute/mass of solution X 109
Molarity
- molar [ ]
- moles of solute/1L of solution
Dilutions
- reducing concentration of a solute by adding additional solution to the mixture
- standard/stock solution: one where the [ ] is known
- c1V1 = c2V2
- c1 is the initial [ ]
- c2 is the final [ ]
- V1 is the initial volume
- V2 is the final volume
Double Displacement Reactions
- 2 possible outcomes
- Compounds remain as ions and no reaction occurs (NR)
- New compounds created that consist of 2 of the following: solid precipitate, gas, or water
Net Ionic Equations
- an ionic compound dissociates in water and is broken up into its constituent ions
- the above occurs before a double displacement reaction happens
- net ionic equation only contains the new product and the constituents that produce this
compound
- spectator ions are any ions not involved in the creation of the new product
Acids
- sour taste
- no texture
- conducts electricity in an aqueous solution
- pH less than 7
- turns litmus paper red
- phenolphthalein is colourless
H2(g)- Acid + Metal
CO2(g) + H2O(l)- Acid + Carbonate
Bases
- bitter taste
- slippery texture
- conducts electricity in an aqueous solution
- pH greater than 7
- turns litmus paper blue
- turns phenolphthalein pink
Arrhenius Theory
- an acid is any substance that will ionize in water to produce H ions
- a base is a substance that will dissociate in water to produce OH ions
- H ions cannot exist alone, and thus exist attached to H2O, creating hydronium: H3O
- Only valid for reactions in water
Bronsted-Lowry Theory
- acids are substances that have an H ion removed
- conjugate base is paired with the acid, and becomes the new base
- bases are substances that have an H ion added
- conjugate acid is paired with the base and becomes the new acid
Strong Acids
- will completely dissociate
Weak Acids
- will only have some of the solution dissociated
- indicated in a chemical equation by a double arrow
Monoprotic Acid
- can only give up 1 H ion
Diprotic Acid
- can give up 2 H ions (H2SO4, H2CO3)
Triprotic Acid
- can give up 3 H ions (H3PO4)
pH and pOH
- pH = -log[H or H3O]
- [H or H3O] = 10-pH
- pOH = -log[OH]
- [OH] = 10-pOH
- pH + pOH = 14
Neutralization
Salt + Water- Acid + Base
- Titrations are done to determine the number of moles when the number of moles of H and
OH are equal
- Equivalence point: the point when titration is complete (H = OH)
- End point: a sudden change occurs during a titration
- Equivalence is theoretical and determined by calculations
- End is experimental and determined by indicators
RE
SCH3U1 Grade 11 Chemistry Unit 3 Solutions and Solubility Unit Test Study Notes
Effect of Temperature on Solubility
- every unique pure substance has its own unique solubility based on the types of bond
present
- units used to describe/measure solubility is: mass of solute/100mL of solvent
Solubility of Solid
- trend: solubility of solids increase as temperature increases
- energy is required to break apart bonds of solids when dissolved in water
- as temperature increases, there is more energy to break these bonds
SATP/STP: standard ambient temperature and pressure
S = soluble
SS = slightly soluble
I = insoluble
Solubility of Gases
- trend: solubility of gases decrease as temperature increases
- with more energy, the gas particles escape the solution
Solubility of Liquids
- trend: solubility of liquids is not affected by the temperature
- solute: liquid with less amount
- solvent: liquid with greater amount
Water
- universal solvent
- small size, highly polar nature, and the capacity to form hydrogen bonds makes water very
successful at dissolving solutes
- water has a permanent dipole
- the negative end is attracted to the positive end, causing a special type of attraction called
hydrogen bonding
Hydrogen Bonding
- any substance containing hydrogen and oxygen/fluorine/nitrogen
- doesn’t create an actual bond, uses strong intermolecular forces to create a force of
attraction
- hydrogen bonded compounds are likely to dissolve in water
Properties
- water is held together by covalent bonds which re stronger than hydrogen bonds
- however, the hydrogen bond is stronger than regular dipole-dipole attractions
- this results in higher boiling points because more energy is required to break apart these
bonds
- hydrogen bonds also result in higher surface tension
Volume/Volume Concentration (V/V) %
- volume of solute(mL)/volume of solution(mL) X 100%
Mass/Volume Concentration (m/V) %
- mass of solute(g)/mass of solution(mL) X 100%
Mass/Mass concentration (m/m) %
- mass of solute(g)/mass of solution(g) X 100%
Very Low Concentrations
- parts per million (ppm) = mass of solute/mass of solution X 106
- parts per billion (ppb) = mass of solute/mass of solution X 109
Molarity
- molar [ ]
- moles of solute/1L of solution
Dilutions
- reducing concentration of a solute by adding additional solution to the mixture
- standard/stock solution: one where the [ ] is known
- c1V1 = c2V2
- c1 is the initial [ ]
- c2 is the final [ ]
- V1 is the initial volume
- V2 is the final volume
Double Displacement Reactions
- 2 possible outcomes
- Compounds remain as ions and no reaction occurs (NR)
- New compounds created that consist of 2 of the following: solid precipitate, gas, or water
Net Ionic Equations
- an ionic compound dissociates in water and is broken up into its constituent ions
- the above occurs before a double displacement reaction happens
- net ionic equation only contains the new product and the constituents that produce this
compound
- spectator ions are any ions not involved in the creation of the new product
Acids
- sour taste
- no texture
- conducts electricity in an aqueous solution
- pH less than 7
- turns litmus paper red
- phenolphthalein is colourless
H2(g)- Acid + Metal
CO2(g) + H2O(l)- Acid + Carbonate
Bases
- bitter taste
- slippery texture
- conducts electricity in an aqueous solution
- pH greater than 7
- turns litmus paper blue
- turns phenolphthalein pink
Arrhenius Theory
- an acid is any substance that will ionize in water to produce H ions
- a base is a substance that will dissociate in water to produce OH ions
- H ions cannot exist alone, and thus exist attached to H2O, creating hydronium: H3O
- Only valid for reactions in water
Bronsted-Lowry Theory
- acids are substances that have an H ion removed
- conjugate base is paired with the acid, and becomes the new base
- bases are substances that have an H ion added
- conjugate acid is paired with the base and becomes the new acid
Strong Acids
- will completely dissociate
Weak Acids
- will only have some of the solution dissociated
- indicated in a chemical equation by a double arrow
Monoprotic Acid
- can only give up 1 H ion
Diprotic Acid
- can give up 2 H ions (H2SO4, H2CO3)
Triprotic Acid
- can give up 3 H ions (H3PO4)
pH and pOH
- pH = -log[H or H3O]
- [H or H3O] = 10-pH
- pOH = -log[OH]
- [OH] = 10-pOH
- pH + pOH = 14
Neutralization
Salt + Water- Acid + Base
- Titrations are done to determine the number of moles when the number of moles of H and
OH are equal
- Equivalence point: the point when titration is complete (H = OH)
- End point: a sudden change occurs during a titration
- Equivalence is theoretical and determined by calculations
- End is experimental and determined by indicators
RE
SCH3U1 Grade 11 Chemistry Unit 3 Solutions and Solubility Unit Test Study Notes
Effect of Temperature on Solubility
- every unique pure substance has its own unique solubility based on the types of bond
present
- units used to describe/measure solubility is: mass of solute/100mL of solvent
Solubility of Solid
- trend: solubility of solids increase as temperature increases
- energy is required to break apart bonds of solids when dissolved in water
- as temperature increases, there is more energy to break these bonds
SATP/STP: standard ambient temperature and pressure
S = soluble
SS = slightly soluble
I = insoluble
Solubility of Gases
- trend: solubility of gases decrease as temperature increases
- with more energy, the gas particles escape the solution
Solubility of Liquids
- trend: solubility of liquids is not affected by the temperature
- solute: liquid with less amount
- solvent: liquid with greater amount
Water
- universal solvent
- small size, highly polar nature, and the capacity to form hydrogen bonds makes water very
successful at dissolving solutes
- water has a permanent dipole
- the negative end is attracted to the positive end, causing a special type of attraction called
hydrogen bonding
Hydrogen Bonding
- any substance containing hydrogen and oxygen/fluorine/nitrogen
- doesn’t create an actual bond, uses strong intermolecular forces to create a force of
attraction
- hydrogen bonded compounds are likely to dissolve in water
Properties
- water is held together by covalent bonds which re stronger than hydrogen bonds
- however, the hydrogen bond is stronger than regular dipole-dipole attractions
- this results in higher boiling points because more energy is required to break apart these
bonds
- hydrogen bonds also result in higher surface tension
Volume/Volume Concentration (V/V) %
- volume of solute(mL)/volume of solution(mL) X 100%
Mass/Volume Concentration (m/V) %
- mass of solute(g)/mass of solution(mL) X 100%
Mass/Mass concentration (m/m) %
- mass of solute(g)/mass of solution(g) X 100%
Very Low Concentrations
- parts per million (ppm) = mass of solute/mass of solution X 106
- parts per billion (ppb) = mass of solute/mass of solution X 109
Molarity
- molar [ ]
- moles of solute/1L of solution
Dilutions
- reducing concentration of a solute by adding additional solution to the mixture
- standard/stock solution: one where the [ ] is known
- c1V1 = c2V2
- c1 is the initial [ ]
- c2 is the final [ ]
- V1 is the initial volume
- V2 is the final volume
Double Displacement Reactions
- 2 possible outcomes
- Compounds remain as ions and no reaction occurs (NR)
- New compounds created that consist of 2 of the following: solid precipitate, gas, or water
Net Ionic Equations
- an ionic compound dissociates in water and is broken up into its constituent ions
- the above occurs before a double displacement reaction happens
- net ionic equation only contains the new product and the constituents that produce this
compound
- spectator ions are any ions not involved in the creation of the new product
Acids
- sour taste
- no texture
- conducts electricity in an aqueous solution
- pH less than 7
- turns litmus paper red
- phenolphthalein is colourless
H2(g)- Acid + Metal
CO2(g) + H2O(l)- Acid + Carbonate
Bases
- bitter taste
- slippery texture
- conducts electricity in an aqueous solution
- pH greater than 7
- turns litmus paper blue
- turns phenolphthalein pink
Arrhenius Theory
- an acid is any substance that will ionize in water to produce H ions
- a base is a substance that will dissociate in water to produce OH ions
- H ions cannot exist alone, and thus exist attached to H2O, creating hydronium: H3O
- Only valid for reactions in water
Bronsted-Lowry Theory
- acids are substances that have an H ion removed
- conjugate base is paired with the acid, and becomes the new base
- bases are substances that have an H ion added
- conjugate acid is paired with the base and becomes the new acid
Strong Acids
- will completely dissociate
Weak Acids
- will only have some of the solution dissociated
- indicated in a chemical equation by a double arrow
Monoprotic Acid
- can only give up 1 H ion
Diprotic Acid
- can give up 2 H ions (H2SO4, H2CO3)
Triprotic Acid
- can give up 3 H ions (H3PO4)
pH and pOH
- pH = -log[H or H3O]
- [H or H3O] = 10-pH
- pOH = -log[OH]
- [OH] = 10-pOH
- pH + pOH = 14
Neutralization
Salt + Water- Acid + Base
- Titrations are done to determine the number of moles when the number of moles of H and
OH are equal
- Equivalence point: the point when titration is complete (H = OH)
- End point: a sudden change occurs during a titration
- Equivalence is theoretical and determined by calculations
- End is experimental and determined by indicators
RE
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