reactivity 3.1 Flashcards by nyah sharratt

equation for calculating pH

– log₁₀[H⁺]

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equation for calculating [H⁺]

10⁻ᴾᴴ

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what defines an arrhenius acid?

a substance that disassociates in water to form hydrogen ions (H+) and anions

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what defines an arrhenius base?

a substance that disassociates in water to form hydroxide ions (OH-) and cations

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what does the bronsted-lowry theory focus on?

the transfer of H+ ions during an acid-base reaction (acids donate H+ while bases accept H+)

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what is a bronsted-lowry acid?

a proton donor

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what is a bronsted-lowry base?

a proton acceptor

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define alkali

soluble bases which dissolve in water to release OH-

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define amphiprotic

substances that can act as both bronsted-lowry acids and bases

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requirement for a substance to be amphiprotic

must posses both a lone pair of electrons and hydrogen that can be released as H+

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moving left to right across a period, oxides transition from ______ ______ oxides through ______ oxides then to ______ oxides

basic metal
amphiprotic
acidic

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basic metal oxides react with an acid to form what?

a salt and water

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non-metal oxides form ______ ______ in a solution

weak acids

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amphiprotic oxides react with either an acid or a base to form what?

a salt and water

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the burning of fossil fuels releases what 3 substances

GHG, nitrous oxides ans sulfuric oxides

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what causes acid rain

increased emissions of nitrous oxides ans sulfuric oxides in the atmosphere, which turn rain water from its slightly acidic state (pH = 6) to become a stronger acid

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where is acid rain’s negative effects seen? x3

structural materials, lakes/rivers & plant life/forests

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what pH is acid rain?

pH = <5.6

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what is the [H+] range (in numerical values) for the 0-14 pH scale?

1.0mol dm^-3 →10^-14 mol dm^-3

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increasing pH by 1 = _______ [H+] by __ times

decrease, 10x

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decreasing pH by 1 = _______ [H+] by __ times

increase, 10x

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if the pH of a solution is changed from 3 to 5, how does the [H+] change?

pH = 3 => 10^-pH = 1 x 10^-3 mol dm^-3
pH = 5 => 10^-pH = 1 x 10^-5 mol dm^-3

[H+ ions] decreases by (1 x 10^-3 mol dm^-3)/(1 x 10^-5 mol dm^-3) = 100x times

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what is the relationship between [H+] and [OH-]?

higher [H+] = lower [OH-]
lower [H+] = higher [OH-]

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in terms of pH, what does a surplus of [H+] signify? what does a surplus of [OH-] signify?

surplus of [H+] = low pH = acidic
surplus of [OH-] = high pH = basic

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pH's neutral value = 7 at what temperature?

298K

how to find [H+] with value of [OH-]?

Kᵥᵥ / [OH-]

how to find [OH-] with value of [H+]?

Kᵥᵥ / [H+]

pH of pure water goes ____ as temperature goes ____

down, up

despite changes in pH, why is water is still neutral?

[H+] = [OH-]

characteristics of a strong acid x2

dissociates fully good proton donors

why do strong acids have weak conjugate bases?

because their reactions fo virtually to completion so they are not readily able to accept a proton

characteristics of a weak acid x2

dissociates only partially poor proton donors

why do weaker acids have strong conjugate bases?

their dissociation reactions are equilibria that lies in favour of reactants, their CB are readily available to accept a proton

acid dissociation reactions favour the production of a _______ conjugate. why?

weaker. better for strong acid to dissociate

characteristics of a strong base x2

ionizes fully good proton acceptors

characteristics of a weak base x2

ionizes partially poor proton acceptors

base ionization reactions favours the production of the _____ conjugate

weaker

strength of an acid or base is a measure of what?

how readily it dissociates/ionizes in aqueous solution (similar to solubility) to release H+/OH-

strong acids x5

HCl HBr HI HNO3 H2SO4

strong bases x3

LiOH NaOH KOH

weak acids x3

CH3COOH H2CO3 H4PO4

weak bases x2

NH3 C2H5NH2 (& other amines)

as the halogen atom ______ in size going down group 17, the length of the H-halogen bond ________

increases, increases

are longer bonds weaker or stronger? do they require more or less energy to break?

weaker, less

acid strength of hydrogen halides _______ down the group

decreases HF < HCl < HBr < HI

electrical conductivity depends on the concentration of what?

mobile ions

greater ionization in solution for strong acids & bases ⟹ _______ concentration of ions ⟹ ________ conductivity than weak acids and bases (only if solutions of the same concentration are compared)

higher, higher

neutralization reactions x2 products, exo or endo?

salt and water, exo

when acids react with reactive metals, they also form salts as the hydrogen in the acid is replaced by the metal. why is there no transfer of a proton?

the hydrogen is released as H2 gas

when acids react with reactive metals, electrons as a product = what type of reaction? electrons as a reactant = what type of reaction?

electrons as a product = oxidation electrons as a reactant = reduction

when acids react with reactive metals, why is the metal being ionized?

because H+ are becoming electrically neutral by accepting e- while the metal is being ionized by e- loss

acid + carbonate → ___ + ___ + ___ 2 examples of carbonates

salt, water, CO2 gas metal carbonates (CO3^2-) and hydrogencarbonates (HCO3-)

how to determine ionic/net ion equations

break up compounds, cancel out things shown on both sides of the reaction

define effercescence

reactions involving a gas being given off so they visibly produce bubbles

in neutralisation reactions, how is pure salt separated?

filtration followed by evaportation

what is the net ion reaction for reactions between an acid and a base?

H+ (aq) + OH- (aq) → H2O (l)

define spectator ions

other ions which do not change during the reaction and can be cancelled out

why are neutralisation reactions exothermic?

because for every mole of H2O that forms, 2 moles of O-H bonds are made bond making is exothermic, so overall it is an exothermic reaction

what is the enthalpy of neutralisation reaction between all strong acids and strong bases? how is it expressed?

ΔH = -57 kJ mol^-1 expressed per mole of H2O formed

define monoprotic acid

only has 1 H+ to give

what point is reached when the acid and a base neutralise each other in a titration? x2 names

equivalence point OR stoichiometric point

at the equivalence point of a strong acid and strong base titration, what does the solution contain?

water and salt

how is the reaction ratio of acid to base to reach this point is determined by what?

the stoichiometry of the neutralisation reactions (mole ratios of acid to base reactants)

review last page of r3.1 lesson 04 with volume of added base calculations

reactivity 3.1 Flashcards

(64 cards)