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formed by the addition of a proton to the reactant base
base-add proton-->conj. acid |
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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 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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Definition
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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Definition
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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| meaning they can either react as an acid or a base |
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| BASE reactions with Acids |
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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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| recall that salts are the produce of a neutralization reaction. |
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| HCl, HBr, HI, H2SO4, HClO3, HClO4, HNO3 |
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| Hydroxides of alkali metals and alkaline earth metals. |
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Have Ions, Conduct electricity.
ionic compounds are electrolytes. |
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| Do not dissociate into ions in water, they are molecular compounds, do not conduct electricity. |
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| 100% dissociates into ions; all salts(ionic compounds) and Strong Acids and Bases. |
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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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Definition
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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Definition
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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Definition
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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| are neutralization reactions involving the mixing of an acid and a base to get a salt and water. |
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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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where the indicator changes colors.
it is an approximation of the equivalence point. |
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| show only the species that are involved with the chemical reaction. |
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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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Definition
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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