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!! |
