122 – Chemistry – Flashcards

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Acid
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a proton donor
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Base
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proton acceptor
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conjugate Acid
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formed by the addition of a proton to the reactant base
base-add proton-->conj. acid
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conjugate Base
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formed by the removal of a proton from the reactant acid
acid--subtract proton--->conj. base
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Acids React with MEtals
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acids will react with metals ABOVE hydrogen on the activity series to produce an ionic compound and H2 gas.
Ex. 6HC2H3O(aq)+2Al(s)-->3H2(g)+2Al(c3H3O2)3(aq)
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Acids Reaction With Bases
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neutralizes reactions to produce a new salt and water. Use Solubility RULES.
Ex. HBr(aq)+KOH(aq)-->KBr(aq)+H2O(l)
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Acids Reaction with Metal Oxides
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Produce a salt and water. Use Solubility RULES.
Ex. H2SO4(aq)+MgO(s)-->MgSO4(aq)+H2O(l)
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Acids Reaction with Carbonates(CO3 2-) & Bicarbonates (HCO3 -)
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These reactions produce a new ionic compound and carbonic acid. Carbonic acid is unstable and immediately go to CO2 & H2O. Use Solubility Rules.
Ex. H2SO4(aq)+MgCO3(s)-->MgSO4(aq)+H2O(l)+CO2(g)
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Amphoteric
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meaning they can either react as an acid or a base
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BASE reactions with Acids
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neutralization reactions
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Reactions of BASES
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1. with acids=neutralization reaction
2. Hydroxides of certain metals such as zinc, aluminum and chromium are amphoteric.
3. Some amphoteric metals react directly with KOH & NaOH to produce hydrogen.
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SALTS
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recall that salts are the produce of a neutralization reaction.
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STRONG ACIDS
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HCl, HBr, HI, H2SO4, HClO3, HClO4, HNO3
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STRONG BASES
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Hydroxides of alkali metals and alkaline earth metals.
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ELECTROLYTES
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Have Ions, Conduct electricity.
ionic compounds are electrolytes.
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NON Electrilytes
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Do not dissociate into ions in water, they are molecular compounds, do not conduct electricity.
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Strong Electrolytes
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100% dissociates into ions; all salts(ionic compounds) and Strong Acids and Bases.
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Weak Electrolytes
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NOT 100% dissociated into ions in water, weak acids and bases, Nh3, Fe(OH)3, HNO2.

*do not confuse with nonelectrolytes HC2H3O2.
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pH
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water is amphoteric and reacts as follows:
H2O+H2O-->H3O(hydronium)+OH-(hydroxide)
The ionization of water at 25'C produces a hydrogen (hydronium) ion concentration of 1.0x10^-7 M and a hydroxide ion concentration of 1.0x10^-7 M.
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pH: the Greater the acidity the...
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the greater the H+ the less the pH.
pH less than 7 is acid.
less OH-=greater pH
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pH: the less the Acidity the....
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less the H+, the greater the pH.
pH greater than 7=Base.
greater the OH-=less pH.
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pH: the acidity of the solution depends on the concentration of the hydrogen or hydronium ions.
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Titrations
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are neutralization reactions involving the mixing of an acid and a base to get a salt and water.
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Equivalence Point
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the equivalence point in a neutralization reaction is where moles of base added are equal to the moles of acid in the beaker.
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Endpoint
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where the indicator changes colors.
it is an approximation of the equivalence point.
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Net Ionic Equations
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show only the species that are involved with the chemical reaction.
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Spectator Ions
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they are not directly involved with the chemical reaction.
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steps to writing a Net Ionized Equation
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1. Write the complete balanced equation including phases of each compound.
2. IONIZE everything that is an (aq)-put in proper coefficients.
3. Cancel out the spectator ions.
4. Write the equation you have left..this is the net ionic equation!!
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