Chapter 18

25 July 2022
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acidic solution
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An acid is a substance that donates hydrogen ions. Because of this, when an acid is dissolved in water, the balance between hydrogen ions and hydroxide ions is shifted. Now there are more hydrogen ions than hydroxide ions in the solution. This kind of solution is acidic.
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basic solution
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A solution that has a higher concentration of hydroxide ions that hydrogen ions; a pH between 7 and 14.
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arrhenius model
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As defined by Arrhenius, acid-base reactions are characterized by acids, which dissociate in aqueous solution to form hydrogen ions (H+) and bases, which form hydroxide (OH−) ions. Acids are defined as a compound or element that releases hydrogen (H+) ions into the solution.
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brønsted-lowry model
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The formation of conjugate acids and bases is central to the Brønsted-Lowry definition of acids and bases. The conjugate base is the ion or molecule remaining after the acid has lost its proton, and the conjugate acid is the species created when the base accepts the proton.
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conjugate acid
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A conjugate acid, within the Brønsted-Lowry acid-base theory, is a species formed by the reception of a proton (H+) by a base—in other words, it is a base with a hydrogen ion added to it. On the other hand, a conjugate base is merely what is left after an acid has donated a proton in a chemical reaction.
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conjugate acid-base pair
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The conjugate base of an acid is formed when the acid donates a proton. In the equation, OH- is the conjugate base to the acid H2O because H2O donates a hydrogen ion to form OH-, the conjugate base. Note: The stronger the acid or base, the weaker the conjugate
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amphoteric
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A chemical species that behaves both as an acid and as a base is called amphoteric. This property depends upon the medium in which the species is investigated: H2SO4 is an acid when studied in water, but becomes amphoteric in superacids.
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lewis model
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A Lewis structure is a structural representation of a molecule where dots are used to show electron position around the atoms and lines or dot pairs represent covalent bonds between atoms.
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strong acid
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This determines an acid's strength. A strong acid is any acid that ionizes completely in solutions. This means it gives off the greatest number of hydrogen ions or protons when placed in a solution. Ions are charged particles.
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weak acid
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Most acids are weak acids. A weak acid is an acid that dissociates incompletely, releasing only some of its hydrogen atoms into the solution. Thus, it is less capable than a strong acid at donating protons. These acids have higher pKa than strong acids, which release all of their hydrogen atoms when dissolved in water.
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acid inization constant
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An acid dissociation constant, Ka, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions.
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strong base
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A strong base is something like sodium hydroxide or potassium hydroxide which is fully ionic. You can think of the compound as being 100% split up into metal ions and hydroxide ions in solution. Each mole of sodium hydroxide dissolves to give a mole of hydroxide ions in solution.
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base ionization
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the equilibrium constant for the reaction in which a weak base is in equilibrium with its conjugate acid in aqueous solution.
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ion product constant for water
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Water molecules can function as both acids and bases. One water molecule (acting as a base) can accept a hydrogen ion from a second one (acting as an acid). This will be happening anywhere there is even a trace of water - it doesn't have to be pure.
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pH
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High pH means that a solution is basic while high pOH means that a solution is acidic. Neutral solutions have pH and pOH of 7.
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pOH
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pOH denote the negative log of the concentration of hydrogen or hydroxide ions.
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neutralization reaction
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a chemical reaction in which an acid and a base interact with the formation of a salt; with strong acids and bases the essential reaction is the combination of hydrogen ions with hydroxyl ions to form water
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salt
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salt is an ionic compound that results from the neutralization reaction of an acid and a base. [1] Salts are composed of related numbers of cations (positively charged ions) and anions (negative ions) so that the product is electrically neutral (without a net charge).
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titration
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A titration is a technique where a solution of known concentration is used to determine the concentration of an unknown solution. Typically, the titrant (the know solution) is added from a buret to a known quantity of the analyte (the unknown solution) until the reaction is complete.
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titrant
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A titration is a technique where a solution of known concentration is used to determine the concentration of an unknown solution. Typically, the titrant (the know solution) is added from a buret to a known quantity of the analyte (the unknown solution) until the reaction is complete.
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equivalence point
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The equivalence point, or stoichiometric point, of a chemical reaction is the point at which chemically equivalent quantities of acid and base have been mixed. In other words, the moles of acid are equivalent to the moles of base. It can be found by means of an indicator, most often phenolphthalein
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end point
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the point at which the indicator used in a titration changes color
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salt hydrolysis
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the anions of the dissociated salt accept hydrogen ions from water or cations of dissociates salt donate hydrogen ions to water
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buffer
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the resist changes in pH when limited amounts of acid or base are added
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buffer capacity
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the amount of acid or base a buffer solution can absorb without significant change in pH