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Questions and Answers
Which of the following best describes what happens when an ionic compound dissolves in water?
Which of the following best describes what happens when an ionic compound dissolves in water?
- he compound forms a new molecular structure by bonding with water molecules.
- The compound remains intact, evenly dispersed throughout the water.
- The compound undergoes a chemical reaction, producing entirely new substances.
- The compound dissociates into individual ions, each surrounded by water molecules. (correct)
All molecular compounds dissociate into ions when dissolved in water.
All molecular compounds dissociate into ions when dissolved in water.
False (B)
What is the key difference between a strong electrolyte and a weak electrolyte when dissolved in water?
What is the key difference between a strong electrolyte and a weak electrolyte when dissolved in water?
A strong electrolyte dissociates completely, while a weak electrolyte only dissociates partially.
A substance that dissolves in water but does not dissociate into ions is called a(n) ______.
A substance that dissolves in water but does not dissociate into ions is called a(n) ______.
Match each term with its correct description:
Match each term with its correct description:
When a precipitation reaction occurs, what is the observable result?
When a precipitation reaction occurs, what is the observable result?
All ionic compounds are soluble in water.
All ionic compounds are soluble in water.
Which of the following is the best definition of a solution?
Which of the following is the best definition of a solution?
In a dilution process, what is the relationship between the molarity and volume of the concentrated and diluted solutions?
In a dilution process, what is the relationship between the molarity and volume of the concentrated and diluted solutions?
In a titration, the concentration of the standard solution must be unknown to determine the concentration of another solution.
In a titration, the concentration of the standard solution must be unknown to determine the concentration of another solution.
What is the purpose of performing a titration?
What is the purpose of performing a titration?
A solution of known concentration used in a titration is called a __________ solution.
A solution of known concentration used in a titration is called a __________ solution.
What is the oxidation state of Arsenic (As) in the polyatomic ion $AsO_4^{3-}$?
What is the oxidation state of Arsenic (As) in the polyatomic ion $AsO_4^{3-}$?
By analogy to the corresponding phosphorus compound, what is the name of $Ag_3AsO_4$?
By analogy to the corresponding phosphorus compound, what is the name of $Ag_3AsO_4$?
What piece of lab equipment is typically used to accurately deliver a specific volume of solution when performing a dilution?
What piece of lab equipment is typically used to accurately deliver a specific volume of solution when performing a dilution?
If 25.0 mL of a 2.0 M NaCl solution is diluted to 500.0 mL, what is the molarity of the diluted solution?
If 25.0 mL of a 2.0 M NaCl solution is diluted to 500.0 mL, what is the molarity of the diluted solution?
In a metathesis reaction, what is the fundamental process that occurs between the reactant compounds?
In a metathesis reaction, what is the fundamental process that occurs between the reactant compounds?
In a complete ionic equation, insoluble ionic salts are dissociated into their ions to accurately reflect the species in the reaction mixture.
In a complete ionic equation, insoluble ionic salts are dissociated into their ions to accurately reflect the species in the reaction mixture.
What is the key criterion for identifying the formation of a precipitate in a metathesis reaction, according to the provided steps?
What is the key criterion for identifying the formation of a precipitate in a metathesis reaction, according to the provided steps?
In a complete ionic equation, strong electrolytes are represented as ______ ions, while non-electrolytes are represented as molecules.
In a complete ionic equation, strong electrolytes are represented as ______ ions, while non-electrolytes are represented as molecules.
Match the type of equation with its description:
Match the type of equation with its description:
Which type of equation best represents the actual chemical species present in a reaction mixture?
Which type of equation best represents the actual chemical species present in a reaction mixture?
Which of the following steps is essential when completing and balancing metathesis equations?
Which of the following steps is essential when completing and balancing metathesis equations?
The molecular equation accurately represents the ionic nature of compounds in a solution.
The molecular equation accurately represents the ionic nature of compounds in a solution.
What is the oxidation number of an element in its elemental form?
What is the oxidation number of an element in its elemental form?
Fluorine can have a positive oxidation number in oxyanions.
Fluorine can have a positive oxidation number in oxyanions.
What is the oxidation number of oxygen in the peroxide ion?
What is the oxidation number of oxygen in the peroxide ion?
In displacement reactions, ______ oxidize an element.
In displacement reactions, ______ oxidize an element.
Which statement best describes the relationship between an element's position in the activity series and its reactivity?
Which statement best describes the relationship between an element's position in the activity series and its reactivity?
What is the oxidation number of hydrogen when bonded to a metal?
What is the oxidation number of hydrogen when bonded to a metal?
Aqueous copper(II) ions, $Cu^{2+}$, are mixed with metallic silver, $Ag(s)$. Based on the provided example, what is the expected outcome?
Aqueous copper(II) ions, $Cu^{2+}$, are mixed with metallic silver, $Ag(s)$. Based on the provided example, what is the expected outcome?
Match the following rules with the appropriate description regarding oxidation numbers:
Match the following rules with the appropriate description regarding oxidation numbers:
Which of the following statements regarding molarity is correct?
Which of the following statements regarding molarity is correct?
According to the activity series, silver (Ag) will react with copper sulfate ($CuSO_4$) to produce copper metal.
According to the activity series, silver (Ag) will react with copper sulfate ($CuSO_4$) to produce copper metal.
A metal reacts with an acid to produce hydrogen gas. What happens to the metal during this reaction?
A metal reacts with an acid to produce hydrogen gas. What happens to the metal during this reaction?
To prepare a solution of known molarity, a known mass of solute is added to a ______ flask, and solvent is added to the line on the neck of the flask.
To prepare a solution of known molarity, a known mass of solute is added to a ______ flask, and solvent is added to the line on the neck of the flask.
What is the purpose of the activity series?
What is the purpose of the activity series?
If 10.0 g of sodium chloride ($NaCl$) is dissolved in enough water to make 500.0 mL of solution, what is the molarity of the solution? (Molar mass of $NaCl$ = 58.44 g/mol)
If 10.0 g of sodium chloride ($NaCl$) is dissolved in enough water to make 500.0 mL of solution, what is the molarity of the solution? (Molar mass of $NaCl$ = 58.44 g/mol)
Which of the following affects the concentration of a solution?
Which of the following affects the concentration of a solution?
Match the following terms with their appropriate descriptions:
Match the following terms with their appropriate descriptions:
In the reaction $Ag^+(aq) + NO_3^−(aq) + K^+(aq) + Cl^−(aq) → AgCl(s) + K^+(aq) + NO_3^−(aq)$, which ions are considered spectator ions?
In the reaction $Ag^+(aq) + NO_3^−(aq) + K^+(aq) + Cl^−(aq) → AgCl(s) + K^+(aq) + NO_3^−(aq)$, which ions are considered spectator ions?
A net ionic equation includes all ions present in the solution before and after the reaction.
A net ionic equation includes all ions present in the solution before and after the reaction.
What is the key difference between a strong acid and a weak acid in terms of dissociation in water?
What is the key difference between a strong acid and a weak acid in terms of dissociation in water?
According to Arrhenius, acids increase the concentration of _____ when dissolved in water.
According to Arrhenius, acids increase the concentration of _____ when dissolved in water.
Which definition of a base is attributed to Brønsted and Lowry?
Which definition of a base is attributed to Brønsted and Lowry?
Strong bases only partially react to produce hydroxide anions.
Strong bases only partially react to produce hydroxide anions.
Which of the following steps is NOT part of writing net ionic equations?
Which of the following steps is NOT part of writing net ionic equations?
Match the acid-base definition with the scientist(s) who proposed it:
Match the acid-base definition with the scientist(s) who proposed it:
Flashcards
Solutions
Solutions
Homogeneous mixtures of two or more pure substances.
Solvent
Solvent
The substance present in the greatest abundance in a solution.
Solutes
Solutes
Substances dissolved in a solvent.
Aqueous Solution
Aqueous Solution
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Electrolyte
Electrolyte
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Nonelectrolyte
Nonelectrolyte
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Strong Electrolyte
Strong Electrolyte
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Weak Electrolyte
Weak Electrolyte
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Metathesis Reaction
Metathesis Reaction
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Steps for Balancing Metathesis Equations
Steps for Balancing Metathesis Equations
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Molecular Equation
Molecular Equation
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Complete Ionic Equation
Complete Ionic Equation
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Precipitate
Precipitate
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Aqueous Reactions
Aqueous Reactions
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Oxidation Number
Oxidation Number
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Elemental Form Oxidation Number
Elemental Form Oxidation Number
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Monatomic Ion Oxidation Number
Monatomic Ion Oxidation Number
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Oxygen Oxidation Number
Oxygen Oxidation Number
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Hydrogen Oxidation Number
Hydrogen Oxidation Number
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Fluorine Oxidation Number
Fluorine Oxidation Number
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Activity Series
Activity Series
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Dilution
Dilution
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Dilution Equation
Dilution Equation
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Titration
Titration
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Standard Solution
Standard Solution
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Equivalence Point
Equivalence Point
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Stoichiometric Calculations
Stoichiometric Calculations
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Arsenate Formula
Arsenate Formula
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Ag3AsO4 Name
Ag3AsO4 Name
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Net Ionic Equation
Net Ionic Equation
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Spectator Ions
Spectator Ions
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Steps to Net Ionic Equations
Steps to Net Ionic Equations
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Acids
Acids
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Bases
Bases
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Strong Acids
Strong Acids
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Weak Acids
Weak Acids
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Strong base
Strong base
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Metal/Acid Displacement
Metal/Acid Displacement
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Concentration
Concentration
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Molarity (M)
Molarity (M)
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Molarity Calculation: Example 1
Molarity Calculation: Example 1
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Molarity Calculation: Example 2 (Ethanol)
Molarity Calculation: Example 2 (Ethanol)
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Molarity Calculation: Example 3 (Glucose)
Molarity Calculation: Example 3 (Glucose)
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Mixing a Solution (Known Molarity)
Mixing a Solution (Known Molarity)
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Study Notes
- Solutions are mixtures of two or more pure substances that are homogeneous.
- The solvent is the substance present in the greatest amount.
- All other substances in a solution are solutes.
- Aqueous solutions exist when water is the solvent.
Aqueous Solutions
- Substances dissolve in water in different ways.
- Ionic compounds dissociate into ions when dissolved in water.
- Molecular compounds typically interact with water but do not dissociate.
- Some molecular substances chemically react with water when dissolving.
Electrolytes & Nonelectrolytes
- Electrolytes dissociate into ions when dissolved in water.
- Nonelectrolytes may dissolve in water but do not dissociate into ions.
- Strong electrolytes completely dissociate when dissolved.
- Weak electrolytes only partially dissociate when dissolved.
- Nonelectrolytes do not dissociate when dissolved.
- Not all ionic compounds dissolve in water.
- Solubility rules are used to determine which combination of ions will dissolve.
Precipitation Reactions
- When two solutions containing soluble salts are mixed, an insoluble salt sometimes precipitates out.
Metathesis Reactions
- Metathesis means "to transpose" from Greek.
- In these reactions, ions in reactant compounds appear to exchange or transpose.
- Follow these steps to completely balance metathesis equations:
- Use chemical formulas of the reactants to determine which ions are present.
- Write formulas for the products using the cation from one reactant and the anion from the other, using charges to write proper subscripts.
- Check solubility rules to see if either product is insoluble and forms a precipitate.
- Balance the equation.
Ways to Write Metathesis Reactions
- Molecular Equation
- Complete Ionic Equation
- Net Ionic Equation
- A molecular equation lists the reactants and products without indicating the ionic nature of the compounds.
- A complete ionic equation is an equation where all strong electrolytes, including strong acids, strong bases, and soluble ionic salts, are dissociated into their ions.
- Spectator ions includes K+ and 𝑁𝑂3−
- The net ionic equation involves crossing out anything that does not change from the left side of the equation to the right.
- Spectator ions are the ions that are crossed out in the equation.
- The remaining ions are the reactants that form the product, an insoluble salt in a precipitation reaction.
Steps to Write Net Ionic Equations
- Write a balanced molecular equation.
- Dissociate all strong electrolytes.
- Cross out anything that remains unchanged on both sides of the equation.
- Write the net ionic equation with the remaining species.
Acids
- S. A. Arrhenius defines acids as substances that increase the concentration of H+ when dissolved in water.
- J. N. Brønsted and T. M. Lowry defined acids as proton donors
Bases
- Arrhenius defines bases as substances that increase the concentration of 𝑂𝐻− when dissolved in water.
- Brønsted and Lowry defined bases as proton acceptors.
- Strong acids dissociate completely in water, while weak acids only partially dissociate.
- Strong bases dissociate into metal cations and hydroxide anions in water, but weak bases only partially react to produce hydroxide anions.
Acid-Base Reactions
- Acids donate a proton (𝐻+) to a base.
- Reactions between an acid and a base are called neutralization reactions.
- When the base is a metal hydroxide, water and a salt (ionic compound) are produced.
Net Ionic Equation
- In neutralization reactions with strong bases, the net ionic equation is: H+(𝑎𝑞)+ 𝑂𝐻−(𝑎𝑞)→ 𝐻2𝑂(𝑙)
Gas-Forming Reactions
- Some metathesis reactions may not yield the expected products.
- The combination of a carbonate or bicarbonate reacting with an acid will result in a salt, carbon dioxide, and water.
- Some gas-forming reactions generate gases in the hood with a bad oder.
Oxidation Reduction Reactions
- Loss of electrons is oxidation
- Gain of electrons is reduction.
- Oxidation and reduction cannot occur independently.
- Oxidation-reduction reactions are often called redox reactions.
Oxidation Numbers
- Assigning oxidation numbers to each element in a neutral compound or charged entity determines if an oxidation-reduction reaction has occurred
- The rules to assign oxidation numbers are:
- Elements in their elemental form have an oxidation number of zero..
- The oxidation number of a monatomic ion isthe same as its charge.
- Nonmetals tend to have negative oxidation numbers, although some are positive in certain compounds or ions.
- Oxygen typically has an oxidation number of -2 except in peroxide ions, where it has an oxidation number of -1.
- Hydrogen is -1 when bonded to a metal and +1 when bonded to a nonmetal.
- Fluorine always has an oxidation number of -1.
- Other halogens usually have an oxidation number of -1 when negative but can have positive oxidation numbers, mainly in oxyanions.
- The sum of the oxidation numbers in a neutral compound is zero.
- The total of the oxidation numbers in a polyatomic ion equals ion's charge..
Displacement Reactions
- Displacement reactions occur when ions oxidize an element
- Activity series:
- Elements higher on the activity series are more reactive.
- These elements are more likely to exist as ions.
- Elements above hydrogen will react with acids to produce hydrogen gas.
- The metal is oxidized to a cation.
Concentrations of Solutions
- Concentration is the amount of solute dissolved in a specific amount of solvent or solution.
- Term used to designate is concentration
- Chemists often need to express the concentrations of solutions quantitatively.
Molarity
- We can call this the amount dissolved concentration
- Molarity, denoted as M, is one way to measure the concentration of a solution, where: Molarity= moles of solute/volume of solution in liters Steps to create a solution
- known mass of solute is weighed.
- The solute is added to a volumetric flask, and solvent is added up to the line.
Dilution
- Solutions are diluted by:
- using a pipet to deliver a volume of a solution to a new volumetric flask
- adding solvent to the line on the volumetric flask.
- The molarity of the new solution can be determined using the equation: 𝑀𝑐𝑉𝑐 =𝑀𝑑𝑉𝑑,
- 𝑀𝑐 and 𝑀𝑑 arethe molarity of the concentrated and dilute solutions, and 𝑉𝑐 and 𝑉𝑑 are the volumes of the two solutions.
Titration
- Titration: Analytical techinque to Calculate the concentration of a solute
- Titration is an analytical technique to calculate the concentration of a solute in a solution.
- A solution of known concentration, called standard solution, is used to determine the unknown concentration of another solution.
- The point at which the reaction is complete is called the equivalence point.
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Description
Solutions are homogeneous mixtures. Aqueous solutions are created when the solvent is water. Electrolytes dissociate into ions when dissolved. Solubility rules determine if a combination of ions will dissolve.
