acids and bases

• Basic (alkaline) solutions have pH values greater than 7.
• Acidic solutions have pH values less than 7.
• Neutral solutions have pH values equal to 7.
• The pH scale is logarithmic, meaning that each whole number change represents a tenfold increase or decrease in acidity/basicity.
• solute: substance getting dissolved
• solvent: substance doing the dissolving
• solution: the homogenous mixture of solute & solvent
• random molecular motion will allow the solute & solvent to mix completely
• increasing the surface area, pressure, and temperature increase the rate of dissolving
• concentration: the amount of a particular substance, the solute, in a given quantity of solution
• a solution with a greater concentration will have more total solute dissolved in a solution
• molarity: a concentration unit that measures the number of moles of a solute dissolved per liter of solution
• what does it mean when a solution has a lower concentration?

  less total solute dissolved
• molar mass: 1L=1000mL
• Aqueous solutions of acids taste sour
• Acids and bases react together to produce salt and water
• Acids react with some metals to produce hydrogen gas.
• Acids and bases change the color of acid-base indicators, conduct electric current, and are electrolytes.
• Aqueous solutions of bases taste bitter and are slippery
• Self-ionization: when two water molecules produce a hydronium ion, H3O+, and a hydroxide ion, OH-.
• pH scale: a scale ranging from 0-14 used to convey the relative acidity and/or basicity of solutions
• Acid-Base Indicator: any substance whose color is sensitive to the relative pH
• A higher concentration means a lower pH.
• HIn is the protonated form of an acid base indicator, it is red in Litmus.
• In- is the deprotonated form of an acid base indicator, it is blue for Litmus.
• Litmus: a dye obtained from certain lichens that is red under acid conditions and blue under alkaline (basic) conditions.
• Universal Indicator is a dye that changes color depending on the pH of the solution.
• The pH meter measures the voltage of a solution based on the amount of hydronium ion present and converts that to a numerical pH value.
• Hydrochloric acid


  HCL
• Nitric acid

  HNO3
• Sulfuric Acid


  H2SO4
• Acetic acid (vinegar)


  HC2H3O2
• Carbonic acid


  H2CO3
• Phosphoric acid


  H3PO4
• Ammonia (base)


  NH3
• Metal hydroxide (base)

  M(metal)OH
• Sodium hydroxide


  Na(M)OH
• pH means "potential of hydrogen
• arrenius acids and bases are weak acids and bases that can be used to test for acids and bases
• bronsted-lowry acids and bases are proton acceptors and donors