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53 Cards in this Set
- Front
- Back
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What is a Bronsted-Lowry acid?
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a substance that donates a proton to another substance
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What is a BL base?
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a substance that accepts a proton from anouther sumstance
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What is water in regards to acids and bases?
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it is an amphoteric substance. one that can function as either a BL acid or a base
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What determines how water will function in a reaction (act as a acid or base)
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the substance with which it reacts
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What did Arrhenius first recognize in order to classify acids and bases?
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the properties of acidic solutions are due to the H+ ion and those of basic solutions are due to OH- ions
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What is the Conjugate base of BL acid?
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the species that remains when a proton is removed from the acid
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What is the Conjugate acid of a BL base?
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the species formed by adding a proton to the base
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What are the acid and its conj. base (or a base and its conj acid) called?
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Cojugate acid-base pair
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How are the acid-base strenghts of a conjugate acid-base realted?
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The stronger the acid the weaker its conjugate base. the weaker the acid the stronger the conj base.
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In every acid-base reaction the position of equal. favors what?
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the transfer of the proton from the stronger acid to the stronger base
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1.What is Kw called
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1.the ion-product constant for water
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Water can be both a + acceptor and a + donor, and can donate to anouther water molecule. What is this process called?
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The autoionization of water
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Describe the process of autoionization.
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equalibrium, but rapid reactions in both directions and no molecules are ionized for long.
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Kw=
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=[H][OH]=1.0E-14
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using the Kw expression, what relationships can be determined involving H and OH?
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as H increases OH decreases and Visa Versa. Acidic solutions contain more H than OH and Basic more OH than H
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pH=
pOH= pH+pOH= |
pH=-log[H]
POH=-log[OH] =14 |
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How can the Ph of a solution be measured?
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using a pH meter or estimated using an acid-base indicators
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As pH decreases what increases?
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[H]
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What [H] is concidered to be > than what
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1E-7
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1. Strong acids and bases are both strong_____.
2. How do they exist? |
Electrolytes.
2. in aqueous solution entirely as ions. |
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Why are equal. arrows not used in equations for stron acids and bases?
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because the reaction lies entirely to the right (with the ions)
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What are weak acids and bases?
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partially ionized in aqueous solution
can be in equalibrium |
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What is Ka
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the acid-dissociation constant
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What does the magnitude of Ka indicate?
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the tendency of an acid to ionize in water
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What does it mean if the value of Ka is larger
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The acid is stronger.
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percent ionization of reactants=
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(final M (x)/ intial M)100
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When is it better to use the quadratic formual in solvin for x in and "ICE" equal. equation
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when the quantity of x is more than 5% of the initial value.
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When does the % ionization of a weak acid decrease?
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as concentration increases
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What acids are known as Polyprotic acids?
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acids that have more than one ionizable H atom
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What observation can you make about about the removal of protons from a polyprotic acid?
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it is always easier to remove the first proton from a poly. acid than the second, and so on.
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What is Kb called?
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The base-dissociation constant
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What does the constant Kb always refer to?
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the equalibrium in which a base reacts with water to form corresponding conjugate acid and OH-
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1. As the strength of an acid increases (larger Ka) what happens to the conj base?
2. Why is this? |
1.the strength of CB must decrease (smaller Kb)
2. The product of Ka X Kb must equal 1.0 E -14 |
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What results when you multipky Ka x Kb?
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Kw ( the ion-product constant for water)
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If Ka is known how can you calculate Kb for weak base
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Ka x Kb = 1.0 E -14
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PkA + pKB =
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=PkW=14
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How do we know that almost all salts are strong electrolytes?
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Th completely dissociate in water
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What is Hydrolysis?
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The reaction of ions with water and result in a change of pH
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in general anions can be considered what?
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the conj. base of an acid.
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What ions do not undergo hydrolysis?
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cations of alkali metals and earth metals and anions of strong acids
Spectator ions |
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What can the tendency of a substnce to show acidic or basic characteristics in water be correlated to?
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Its Chemical structure
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What does acid character require?
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presence of highly polar H-X bond or when H-X bond is weak and when X- ion is stable
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for oxyacids with the same central atom "y" when does acid strength increase?
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as number of O atoms attatched to the central atom increases
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What are Oxyacids?
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Acids in which OH groups and any additional atoms are bound to a central atom
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for oxyacids that have the same number of OH groups and same number of O atoms when does acid strength increase?
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with increasing electronegativity of central atom
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What occurs when y is a nonmetal?
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bonds are covalent-does not readily lose OH-electroneg inc. acidity
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What makes up the largest catagory of organic acids?
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Carboxylic acids
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The lewis concept of acids and bases emphasizes what?
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the shared electron pair rather than the proton
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a lewis acid is what?
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a electron pair acceptor
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a lewis base is what?
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a electron pair donor
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Why is the lewis concept more general than Bronsted lowry concept?
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it can apply to cases which the acid is some substance other than H
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What does the Lewis concept help to explain?
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why many hydrated metal cations form acidic aq. solns
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The acidity of cations generally increases as what increases and what decreases?
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their charge increases and as the size of the metal ion decreases
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