Podcast
Questions and Answers
What is the relationship between pH and acidity?
What is the relationship between pH and acidity?
- pH and acidity are directly proportional.
- Increased pH indicates lower acidity. (correct)
- Decreased pH indicates lower acidity.
- pH changes do not affect acidity.
What characterizes a weak acid in terms of pKa?
What characterizes a weak acid in terms of pKa?
- Weak acids do not have a pKa.
- Weak acids fully dissociate in solution.
- Weak acids have a low pH.
- Weak acids have high pKa values. (correct)
Which of the following is a characteristic of a polyprotic acid?
Which of the following is a characteristic of a polyprotic acid?
- It is always a strong acid.
- It cannot be used in buffers.
- It can donate only one proton.
- It has one pKa for each proton it can lose. (correct)
What is the effect of a buffer's maximum buffering capacity?
What is the effect of a buffer's maximum buffering capacity?
What is the typical dissociation behavior of a strong acid?
What is the typical dissociation behavior of a strong acid?
How does an increase of one unit in pH affect hydrogen ion concentration?
How does an increase of one unit in pH affect hydrogen ion concentration?
What is the formula for the dissociation constant of weak acids (Ka)?
What is the formula for the dissociation constant of weak acids (Ka)?
Which combination of acids demonstrates monoprotic characteristics?
Which combination of acids demonstrates monoprotic characteristics?
What happens to the pH when acetate salt (CH3COONa) is added to a solution?
What happens to the pH when acetate salt (CH3COONa) is added to a solution?
What is the molarity of a solution containing 300 g of NaCl in 700 mL of solution?
What is the molarity of a solution containing 300 g of NaCl in 700 mL of solution?
Which functional group is characterized by a nitrogen atom bonded to at least one hydrogen atom?
Which functional group is characterized by a nitrogen atom bonded to at least one hydrogen atom?
What is a correct statement about a buffer solution?
What is a correct statement about a buffer solution?
Which of the following statements accurately describes acids and bases?
Which of the following statements accurately describes acids and bases?
If the concentration of H+ ions in a solution increases, what is the effect on pH?
If the concentration of H+ ions in a solution increases, what is the effect on pH?
What type of bond is primarily responsible for the interactions in a buffer system?
What type of bond is primarily responsible for the interactions in a buffer system?
What is the correct interpretation of pH = -log[H+]?
What is the correct interpretation of pH = -log[H+]?
In a neutral solution, what is the relationship between [H+] and [OH-]?
In a neutral solution, what is the relationship between [H+] and [OH-]?
Which of the following is NOT a functional group found in organic chemistry?
Which of the following is NOT a functional group found in organic chemistry?
The increase in acidity of a solution corresponds to which change in pH?
The increase in acidity of a solution corresponds to which change in pH?
What does molarity quantify?
What does molarity quantify?
If the molarity of a solution is 2 M, how many moles are there in 1 liter of solution?
If the molarity of a solution is 2 M, how many moles are there in 1 liter of solution?
How is the number of moles calculated from mass?
How is the number of moles calculated from mass?
What is Avogadro's number?
What is Avogadro's number?
What is the correct formula to calculate molarity?
What is the correct formula to calculate molarity?
What unit is used for molar mass?
What unit is used for molar mass?
What mass of NaCl is present in 0.3 kg for calculating molarity?
What mass of NaCl is present in 0.3 kg for calculating molarity?
If 0.3 kg of NaCl is dissolved in 700 mL of water, how many liters does this represent for calculations?
If 0.3 kg of NaCl is dissolved in 700 mL of water, how many liters does this represent for calculations?
What is the equivalent of one Dalton in terms of molar mass?
What is the equivalent of one Dalton in terms of molar mass?
In terms of concentration, what does the term 'molar concentration' refer to?
In terms of concentration, what does the term 'molar concentration' refer to?
What formula represents the calculation of molarity?
What formula represents the calculation of molarity?
If the mass of a substance is 7.3 kg and its molar mass is 300 g/mol, how many moles does it contain?
If the mass of a substance is 7.3 kg and its molar mass is 300 g/mol, how many moles does it contain?
What is the unit of volume used in the molarity formula?
What is the unit of volume used in the molarity formula?
To find the number of moles using mass and molar mass, which formula is used?
To find the number of moles using mass and molar mass, which formula is used?
If a solution has a molarity of 1 M and a volume of 2 L, how many moles of solute are present?
If a solution has a molarity of 1 M and a volume of 2 L, how many moles of solute are present?
What is the result of dividing mass by molar mass?
What is the result of dividing mass by molar mass?
Using a molar mass of 300 g/mol, how many grams are in 5 moles of a substance?
Using a molar mass of 300 g/mol, how many grams are in 5 moles of a substance?
A solution is prepared with 4 moles of solute in 2 L of solution. What is the molarity of the solution?
A solution is prepared with 4 moles of solute in 2 L of solution. What is the molarity of the solution?
Which of the following could mislead one regarding the definition of molarity?
Which of the following could mislead one regarding the definition of molarity?
What does a higher molarity indicate about a solution?
What does a higher molarity indicate about a solution?
Flashcards
Molarity
Molarity
A measure of concentration, expressed as the number of moles of solute per liter of solution.
Solution volume
Solution volume
The total volume of the solution, measured in liters.
Number of moles
Number of moles
The amount of a substance contained in a given mass, expressed in moles.
Molar mass
Molar mass
The mass of one mole of a substance, typically measured in grams/mole.
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Solute
Solute
The substance that is dissolved in a solution.
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Solvent
Solvent
The substance that dissolves the solute to form a solution.
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Concentration
Concentration
A measure of how much solute is present in a given amount of solvent or solution.
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Periodic table
Periodic table
A table of the chemical elements, organized by atomic number.
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Mole
Mole
The SI base unit for amount of substance.
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Solution
Solution
A homogeneous mixture of two or more substances.
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Molarity
Molarity
A measure of concentration, expressed as the number of moles of solute per liter of solution.
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Molar Concentration
Molar Concentration
Another term for molarity, expressing a substance's concentration in moles per liter.
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Moles
Moles
A unit of measurement representing 6.022 x 10^23 units of a substance (atoms, molecules, or ions).
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Molar Mass
Molar Mass
The mass of one mole of a substance, usually measured in grams/mole.
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Avogadro's Number
Avogadro's Number
The constant 6.022 x 10^23, representing the number of particles in one mole of a substance.
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Solute
Solute
The substance being dissolved in a solution.
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Solution
Solution
A homogeneous mixture of two or more substances
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Mole Calculation
Mole Calculation
Calculating the number of moles from mass or vice-versa.
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Unit of Molarity
Unit of Molarity
M (Molar) or mol/L (moles per liter).
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Formula for Moles
Formula for Moles
Number of Moles = Mass (g) / Molar Mass (g/mol).
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Molarity Definition
Molarity Definition
Molarity is a measure of substance concentration, calculated by dividing solute moles by solution liters.
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Acid Definition
Acid Definition
An acid is a substance that donates a proton (H+).
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Base Definition
Base Definition
A base is a substance that accepts a proton (H+).
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pH Definition
pH Definition
pH measures the concentration of H+ ions in a solution.
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pH Scale
pH Scale
The pH scale measures acidity and basicity ranges from 0-14.
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Buffer Definition
Buffer Definition
A buffer solution resists changes in pH.
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Hydroxyl Group
Hydroxyl Group
A functional group in chemistry containing an oxygen and a hydrogen atom.
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Carbonyl Group
Carbonyl Group
A functional group in chemistry containing a carbon and an oxygen atom forming a double bond.
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Carboxyl Group
Carboxyl Group
A functional group in chemistry containing a carbon, oxygen and hydroxyl functional group.
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Functional Groups
Functional Groups
Specific arrangements of atoms within molecules that give characteristic chemical properties.
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Ammonia Buffer
Ammonia Buffer
Ammonia (NH3) reacts with water to form ammonium ions (NH4+) and hydroxide ions (OH-), creating a buffer solution. The reaction shows that ammonia acts as a base.
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Buffer Solution
Buffer Solution
A solution that resists changes in pH when small amounts of acid or base are added.
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Weak Acid Dissociation Constant (Ka)
Weak Acid Dissociation Constant (Ka)
A measure of the extent to which a weak acid dissociates in water.Indicates how easily an acid releases a proton. Smaller Ka value equals weaker acid.
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pKa
pKa
The negative logarithm of the acid dissociation constant (Ka). A measure of how strong or weak an acid is.
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pKa Relationship to Strength
pKa Relationship to Strength
The lower the pKa value, the stronger the acid, and the larger the pKa value, the weaker the acid.
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Monoprotic Acid
Monoprotic Acid
An acid that can donate only one proton (H+) per molecule in a reaction.
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Polyprotic Acid
Polyprotic Acid
An acid that can donate more than one proton (H+) per molecule in a reaction.
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Buffering Capacity
Buffering Capacity
The ability of a buffer to resist changes in pH.
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pH and [H+]
pH and [H+]
pH is inversely proportional to the concentration of hydrogen ions ([H+]). A decrease in pH represents a 10-fold increase in [H+].
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Buffer Range
Buffer Range
The pH range over which a buffer solution effectively resists changes in pH. pKa ± 1.
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Molarity
- Molarity is a concentration measure.
- It's the number of moles of solute per liter of solution.
- Expressed as M (molar) or mol/L.
- Formula: Molarity (M) = moles of solute / liters of solution
- Moles of solute = mass of solute (g) / molar mass (g/mol)
Calculating Molarity
- Example: Find the molarity of 0.3 kg NaCl dissolved in 700 mL water.
- Mass of NaCl = 300 g
- Molar mass of NaCl = 58.44 g/mol
- Volume of solution = 0.7 L
- Moles of NaCl = 300 g / 58.44 g/mol = 5.1 moles
- Molarity = 5.1 moles / 0.7 L = 7.33 M (or 7.33 mol/L)
Types of Chemical Bonds
- Ionic Bond: Bond formed by transferring electrons.
- Covalent Bond: Bond formed by sharing electrons.
- Polar Covalent Bond: Covalent bond where electrons are shared unevenly.
- Non-Polar Covalent Bond: Covalent bond where electrons are shared equally.
- Hydrogen Bond: Weak bond between a hydrogen atom and an electronegative atom.
- Metallic Bond: Bond formed by the attraction between metal ions and delocalized electrons.
Functional Groups
- Hydroxyl group (-OH): Found in alcohols.
- Carbonyl group (C=O): Found in ketones and aldehydes.
- Carboxyl group (-COOH): Found in carboxylic acids.
- Amino group (-NH2): Found in amines.
- Sulfhydryl group (-SH): Found in thiols.
- Phosphate group (-OPO32-): Found in organic phosphates.
- Methyl group (-CH3): Modifies the function of molecules.
Acids and Bases
- Acid: A proton donor.
- Base: A proton acceptor.
- pH: A measure of the concentration of H+ ions in a solution.
- pH = -log[H+]
- Higher H+ concentration, lower pH (more acidic)
- Buffer: A solution that resists changes in pH when small amounts of acid or base are added.
- Buffers are composed of a weak acid/base and its conjugate.
- Ka: Dissociation constant of weak acids.
- pKa: The negative logarithm of Ka. Indicates the acidity of a weak acid. Weak acids have a pKa value.
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