CHEM 1001 Exam 4 Study Guide

A set of flashcards covering key concepts in acid-base chemistry and nuclear chemistry for CHEM 1001.

What is an acid?

An acid is a substance that donates protons (H+) in a chemical reaction and typically has a sour taste. They can react with bases to form salts and water.

base

A base is a substance that accepts protons (H+) in a chemical reaction and usually has a bitter taste. Bases can react with acids to form salts and water.

A substance that can accept protons or donate electron pairs in a chemical reaction. Bases increase the concentration of OH- ions in a solution.

Arrhenius acid

An acid that ionizes into H+ or H3O+ in solution and increases the concentration of these ions in a solution.

Arrenhius bases

Bases that ionizes into OH- ions in solution.

They typically feel slippery and taste bitter.

Bronsted-Lowry acid

An acid that donates protons (H+) in reactions. It can react with a base to form a conjugate base.

Bronsted-Lowry bases

Bases that accept protons (H+) in reactions and can form a conjugate acid.

Strong acid

An acid that is a strong electrolyte, fully ionizing in solution.

These acids have a high degree of dissociation, resulting in a greater concentration of H+ ions.

Strong bases

Bases that are strong electrolytes, fully dissociating in solution, resulting in a high concentration of OH- ions.

They completely ionize, leading to strong alkaline properties.

Weak acid

An acid that is a weak electrolyte, partially ionizing in solution.

Weak acids do not fully dissociate into ions when dissolved in water, resulting in a lower concentration of H+ ions compared to strong acids.

weak bases

Bases that are weak electrolytes, partially dissociating in solution. Weak bases do not fully ionize in water, leading to a lower concentration of OH- ions compared to strong bases.

Conjugate acid

The species that forms when a base accepts a proton. It can donate a proton to a base in a chemical reaction, thus forming a conjugate base.

conjugate base

The species that forms when an acid donates a proton. It can accept a proton in a chemical reaction, thus forming a conjugate acid.

Hydronium ion concentration

The concentration of H3O+ ions in a solution.

It is a measure of acidity and reflects how many hydronium ions are present, affecting the pH level.

pH of a solution

A measure of the acidity or basicity of a solution, calculated as the negative logarithm of the hydronium ion concentration.

It is commonly used to quantify how acidic or basic a solution is, with lower values indicating higher acidity.

Acidic solution

A solution with a pH less than 7.

It contains a higher concentration of hydronium ions compared to pure water, resulting in increased acidity.

Basic solution

A solution with a pH greater than 7.

It contains a higher concentration of hydroxide ions than hydronium ions, resulting in increased basicity.

Neutral solution

A solution with a pH equal to 7.

It has equal concentrations of hydronium and hydroxide ions, making it neither acidic nor basic.

Equivalence in acid-base reaction

The point in the reaction where the amounts of acid and base are equal.

It is the point at which the number of moles of hydrogen ions equals the number of moles of hydroxide ions, resulting in a neutral solution.

volume for an acid-base reaction

The amount of solution needed to fully react with a given volume of acid or base, dependent on concentration and stoichiometry.

This volume is determined by the molarity and the balanced equation of the reaction, and it indicates how much titrant is required to reach the equivalence point.

concentration for an acid-base reaction

The amount of solute present in a given volume of solution, usually expressed in molarity (moles per liter). It is crucial for determining the behavior and outcome of acid-base reactions.

Concentration is key in defining how strong an acid or base is and how they interact during the reaction.

the formula of the salt in an acid-base reaction

The compound formed from the neutralization of an acid by a base, consisting of the cation from the base and the anion from the acid. This salt may have properties and behaviors that influence the overall reaction.

The formula of the salt is determined by the specific acid and base used, and it plays a significant role in the resulting solution's pH and reactivity.

Buffer

A solution that resists changes in pH when small amounts of acid or base are added.

It usually consists of a weak acid and its conjugate base or a weak base and its conjugate acid, helping to maintain a stable pH in various chemical processes.

components of a buffer

The weak acid and its conjugate base, or the weak base and its conjugate acid, that work together to stabilize pH changes.

Weak acid and conjugate base salt

Components that make up a buffer system.

The weak acid donates protons while the conjugate base accepts them, maintaining pH stability.

Weak base and conjugate acid salt

Another set of components that make up a buffer system.

The weak base accepts protons while the conjugate acid donates them, helping to regulate pH levels in a solution.

how the concept of buffer components can influence respiratory acidosis and respiratory alkanosis

Buffer components play a crucial role in maintaining acid-base balance in the body, as they help neutralize excess acids or bases produced during respiratory acidosis or alkalosis.

This regulation ensures that blood pH remains within a narrow range, crucial for proper physiological functions.

Respiratory acidosis

A condition where CO2 accumulates in the blood, leading to decreased pH.

This can occur due to hypoventilation or respiratory diseases, resulting in an imbalance in acid-base homeostasis.

Respiratory alkalosis

A condition where CO2 is expelled too rapidly, leading to increased pH.

This can occur due to hyperventilation or stress, disrupting normal acid-base balance.

Atomic number

The number of protons in the nucleus of an atom; unique to each element.

Mass number

The sum of protons and neutrons in an atom's nucleus.

radioactive decay

The process by which an unstable atomic nucleus loses energy by emitting radiation, transforming into different isotopes or elements.

Alpha decay

A type of radioactive decay where mass number decreases by 4 and atomic number decreases by 2.

It involves the emission of an alpha particle, which consists of 2 protons and 2 neutrons.

Beta decay

A type of radioactive decay where mass number remains the same and atomic number increases by 1.

It involves the conversion of a neutron into a proton, accompanied by the emission of a beta particle (an electron).

Positron decay

A type of radioactive decay where mass number remains the same and atomic number decreases by 1.

It involves the conversion of a proton into a neutron, accompanied by the emission of a positron (the antimatter counterpart of an electron).

Gamma decay

A type of radioactive decay where mass number and atomic number remain unchanged.

It involves the emission of gamma rays, which are high-energy photons.

Nuclear equation

An equation that shows the transformation of one element into another through radioactive decay.

It typically includes the elements involved, their atomic numbers, and mass numbers, clearly indicating the process of decay.

balance nuclear equations using particles

This process involves ensuring that both the mass number and atomic number are conserved on both sides of the equation by accounting for all emitted particles, such as alpha particles, beta particles, and gamma rays.

radioactive isotopes

Atoms with unstable nuclei that undergo decay.

These isotopes can emit radiation in the form of alpha particles, beta particles, or gamma rays, transforming into more stable forms.

Half-life

The time required for half of the radioactive isotopes in a sample to decay.

It is a measure of the rate of decay and varies between different isotopes.

identify different radioactive isotopes used in medicine

This refers to recognizing various isotopes such as Technetium-99m, Iodine-131, and Cobalt-60 that are commonly employed in medical imaging and treatment.

calculate the remaining mass after a giving number of half-lives

This refers to determining the amount of a radioactive substance left in a sample after a specified number of half-lives, based on its initial mass.

It involves applying the half-life formula to find the remaining quantity of the substance.

Radiation sickness symptoms

Symptoms that arise from exposure to high doses of radiation.

They include nausea, vomiting, fatigue, and hair loss, varying in severity depending on exposure levels.

Nuclear fission

A reaction in which a large nucleus splits into smaller nuclei.

This process releases a significant amount of energy and is the principle behind nuclear reactors and atomic bombs.

Nuclear fusion

A reaction in which smaller nuclei combine to form a larger nucleus.

This process releases energy and is the source of power for stars, including the sun.

Fission reactions

Reactions that result in the splitting of heavy nuclei.

They release energy and can produce neutrons, which may induce further fission events.

Fusion reactions

Reactions that result in the combining of light nuclei.

They release energy and are the process that powers stars.