Acids and Bases ALL flashcards 50

Flashcards about acids and bases

Arrhenius acid

A substance that, when dissolved in water, increases the concentration of hydrogen ions ($H^+$). This definition is limited to aqueous solutions and doesn't account for acid-base behavior in non-aqueous environments or reactions that don't involve $H^+$ transfer.

Arrhenius base

A substance that, when dissolved in water, increases the concentration of hydroxide ions ($OH^-$). This definition is restricted to aqueous solutions and substances that directly produce hydroxide ions.

Binary acid

An acid composed of only two elements: hydrogen and a more electronegative element (e.g., HCl, HBr). The strength of these acids depends on the electronegativity and size of the other element.

Brønsted-Lowry acid

A molecular entity or ion capable of donating a proton ($$H^+$​) to another species. This definition expands the concept of acids beyond aqueous solutions, focusing on proton donation.

Brønsted-Lowry base

A molecular entity or ion capable of accepting a proton ($$H^+$​) from another species. This definition broadens the scope of bases to include any species that can accept a proton.

Conjugate base

The species formed when a Brønsted-Lowry acid loses a proton. For example, the conjugate base of $HCl$ is $Cl^-$.

Conjugate acid

The species formed when a Brønsted-Lowry base gains a proton. For example, the conjugate acid of $NH<em>3$ is $NH</em>4^+$.

Lewis acid-base reaction

A reaction involving the formation of a covalent bond between a Lewis acid and a Lewis base through the donation and acceptance of an electron pair. This type of reaction extends acid-base chemistry to systems where proton transfer does not occur.

Lewis acid

A species that accepts an electron pair to form a covalent bond. Lewis acids are typically electron-deficient and can include metal ions and molecules with incomplete octets.

Lewis base

A species that donates an electron pair to form a covalent bond. Lewis bases are typically electron-rich and have lone pairs of electrons available for bonding.

Monoprotic acid

An acid that can donate only one proton per molecule during an acid-base reaction. Examples include hydrochloric acid ($HCl$) and acetic acid ($CH_3COOH$).

Neutralization

The process in which hydronium ions ($H<em>3O^+$) and hydroxide ions ($OH^-$) react to form water ($H</em>2O$). This reaction is fundamental in aqueous chemistry and is highly exothermic.

Oxyacid

An acid containing hydrogen, oxygen, and another element (typically a nonmetal). The acidity of oxyacids depends on the electronegativity and oxidation state of the central nonmetal atom.

Polyprotic acid

An acid that can donate more than one proton per molecule. Examples include sulfuric acid ($H<em>2SO</em>4$) (diprotic) and phosphoric acid ($H<em>3PO</em>4$) (triprotic).

Salt

An ionic compound formed from the reaction between an acid and a base. It consists of the cation from the base and the anion from the acid.

Strong acid

An acid that completely ionizes in aqueous solution, resulting in a high concentration of hydrogen ions ($$H^+$​) and a very low pH. Strong acids are also strong electrolytes.

Weak acid

An acid that only partially ionizes in aqueous solution, resulting in a lower concentration of hydrogen ions ($$H^+$​) and a higher pH compared to strong acids. Weak acids are weak electrolytes.

Sour

A characteristic taste of aqueous solutions of acids. This taste is due to the stimulation of taste receptors by hydrogen ions.

Hydrogen gas (H2)

The gas produced when acids react with active metals (e.g., zinc, iron). This reaction is a redox reaction where the metal is oxidized and hydrogen ions are reduced.

Salts and water

Two products that are formed when acids react with bases through a neutralization reaction. The general form is: Acid + Base → Salt + Water.

Yes, they are electrolytes

Yes, acids conduct electric current in aqueous solutions due to the presence of ions. Therefore, they are electrolytes.

Hydro-

The prefix used in the nomenclature of binary acids to indicate the presence of hydrogen and another element without oxygen. For example, hydrochloric acid ($HCl$).

Sulfuric acid

The most widely produced industrial chemical globally, used in the production of fertilizers, detergents, and various chemical processes. Its formula is $H<em>2SO</em>4$

Muriatic acid

The common name for concentrated solutions of hydrochloric acid ($HCl$). It is used in various industrial and laboratory applications.

Acetic acid

The acid found in vinegar, produced by the fermentation of ethanol. Its chemical formula is $CH_3COOH$

Bitter

A characteristic taste of aqueous solutions of bases. This taste is attributed to the presence of hydroxide ions ($OH^−$).

Slippery

A tactile sensation caused by dilute aqueous solutions of bases. This is due to the saponification of fats on the skin.

Yes, they are electrolytes

Yes, bases conduct electric current in aqueous solutions because they dissociate into ions. Hence, they are electrolytes.

H3O+

The ion formed when a proton ($H^+$) is added to a water molecule ($H<em>2O$), with the chemical formula $H</em>3O^+$. It is the form in which protons exist in aqueous solution.

Polarity of the bond between hydrogen and the element it is bonded to and the ease with which that bond can be broken

The polarity of the bond between hydrogen and the element it is bonded to, as well as the ease with which that bond can be broken. Higher polarity and easier bond breakage lead to stronger acids.

Weak acids

Organic acids, which contain a carboxyl group (-COOH), are generally weak acids because they do not fully dissociate in solution.

Carboxyl group (-COOH)

The acidic functional group present in organic acids, consisting of a carbon atom double-bonded to an oxygen atom and single-bonded to a hydroxyl group ($-COOH$).

Metal cations and the hydroxide anion(OH-)

Most bases contain metal cations and the hydroxide anion ($OH^-$), which contribute to their alkaline properties.

Group 1

Alkali metals are located in Group 1 of the periodic table, known for forming strong bases when they react with water.

CaH2

Calcium hydride has the chemical formula $CaH_2$, and it reacts with water to form calcium hydroxide and hydrogen gas.

Polyprotic diprotic acid

Sulfuric acid ($H<em>2SO</em>4$) is a polyprotic acid that can donate two protons per molecule, making it specifically a diprotic acid.

Polyprotic triprotic acid

Phosphoric acid ($H<em>3PO</em>4$) is a polyprotic acid capable of donating three protons per molecule, thus it is classified as a triprotic acid.

Amphoteric

A substance that can act as either an acid or a base, depending on the chemical environment. Water is a common example of an amphoteric species.

Pickling

The process of removing surface impurities, such as oxides, from metals using acidic solutions. This is commonly done with sulfuric or hydrochloric acid.

Sodium hydroxide (NaOH)

Sodium hydroxide ($NaOH$), also known as lye or caustic soda, is a strong base widely used in industrial processes.

Protons are transferred from one reactant (the acid) to another (the base)

During a Brønsted-Lowry acid-base reaction, protons are transferred from an acid (proton donor) to a base (proton acceptor), leading to the formation of conjugate acid-base pairs.

Phosphoric Acid

Phosphoric acid is used as a flavoring agent in carbonated beverages, providing a tangy taste. Its chemical formula is $H<em>3PO</em>4$

Sulfuric acid

Sulfuric acid is used in lead-acid batteries found in automobiles, acting as an electrolyte. With the chemical formula $H<em>2SO</em>4$

Nitric Acid

Nitric acid stains proteins yellow due to a reaction known as the xanthoproteic reaction, where it reacts with aromatic amino acids in the proteins. Its chemical formula is $HNO_3$

Phosphoric acid

Phosphoric acid is used as a flavoring agent in beverages, contributing to their tartness. Its chemical formula is $H<em>3PO</em>4$

Perchloric acid, hydrochloric acid, and nitric acid

Examples of strong acids include perchloric acid ($HClO<em>4$), hydrochloric acid ($HCl$), and nitric acid ($HNO</em>3$), all of which completely ionize in aqueous solutions.

No

Not all ionic compounds are bases; only those that produce hydroxide ions ($OH^-$) when dissolved in water are considered bases.