SCH3U1 Grade 11 Chemistry Unit 3 Solutions and Solubility
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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
