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| Tart or sour (like lemons) |
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| Bitter (like baking soda) |
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| like water or rough (from skin) |
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| Metals to produce H2 (g) and an ionic compound. |
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| Acids to produce water and salt. |
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| Acid Arrhenius definition: |
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| Substance producing H+ ions |
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| Base Arrheius definition: |
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| Substance producing OH- ions. |
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| Acid w/ metals produce... |
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| Metal carbonates and hydogen carbonates w/ acids produce... |
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| oxides that become acids or bases by addition of water. |
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| oxides of metal elements. |
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| oxides of nonmetal elements. |
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| The reaction of CO2 and H2O: |
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CO2(g)+H2O(l)<->H2CO3(aq)(carbonic acid)
->Synthesis
<-Decomposition |
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| The reaction of SO2 and H2O: |
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| Bases react with acids to form water and a salt. |
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| The reaction between Magnesium Hydroxide and Hydrochloric acid: |
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Mg(OH)2(s)+2HCl(aq)->MgCl2(aq)+2H2O(l)
(Neutralization Reaction) |
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-contain hydrogen and one other element.
-Use the prefix hydro- to name the hydrogen part of the compound.
-The rest of the name comes from the element name plus the suffix -ic and Acid.
-Examples: HCl(Hydrochloric Acid), HI(Hydroidinic Acid), Hydrobromic Acid(HBr) |
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-Any acid that contains hydrogen and a polyatomic ion with oxygen in it (also called an oxyanion).
-The name of an oxyacid contains a form of the root anion, a suffix and the word acid.
-Polyatomic ions ending in -ate change to -ic.
-Polyatomic ions ending in -ite change to -ous.
-Examples: H2SO4(Sufuric Acid), H2SO3(Sulfurous Acid), Phosphoric acid(H3PO4)
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-Generally bases have hydroxide(OH-) at the end.
-Name bases teh exact same way you named ionic compounds(metal ion followed by hydroxide).
-Examples: Ammonia(NH3), NaOH(Sodium Hydroxide), Potassium hydroxide(K(OH)) |
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| a water molecule with an extra hydrogen ion means the same as H+ |
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| The equilibrium equation for the auto-ionization of water and the simplified version: |
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H2O->H+ + OH-
H2O+H2O->H3O+ + OH- |
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| The reaction of SO2 and H2O: |
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| 0 to 14 and 7 is neutral. |
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-[H+] is used interchangably with [H3O+] called a hydronium ion.
-In a neutral solution- [H+]=[OH-]
In acid solutions- [H+]>[OH-]
In baseic solutions- [H+]<[OH-]
-As a solution becomes more acidic the pH number decreases9[H+] increasing)
As a solution becomes more basic the pH number increases ([OH-] increasing) |
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substances that contain hydrogen and dissolve in water to produce hydrogen ions(H+).
-Example:HCl(aq)->H+ + Cl- |
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| when dissolved in water, an electrolyte separates into its individual ions in a process called disscociation or ionization. |
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substances that contain hydroxide and dissolve in water to produce hydroxide ions (OH-).
-Example: Mg(OH)2(aq)->Mg^2+ + 2OH- |
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| Neutral solutions contain... |
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| equal moles of hydrogen ions and hydroxide ions and are not basic or acidic. |
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| Bronsted-Lowry Acid definition: |
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| Bronsted-Lowry Base definition: |
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| substance that can act as either an acid ofr a base depending on its environment. (ex. water) |
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| Conjugate acid-base pairs consist of... |
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two substances related to eachother by the donating or accepting of a single hydrogen ion.
-An acid will have one hydrogen ion more than its conjugate base. |
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| can only donate one H+. Example: HCl, HNO3, HCO3. |
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| can donate more than one H+. Example: H2SO4, H3PO4 |
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| are those that dissociate completly in water. Example:HCl, HBr, HI, HNO, H2SO4, HClO4. |
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