Acids, bases, and solubility rules for AP Chem Unit 1 Exam
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| Alkali metals are always _____ | Soluble
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| Other soluble ions are: | NH4, NO3, ClO3, ClO4, C2H302 Ammonium, Nitrate, Chlorate, Perchlorate, Acetate
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| O and OH (oxide and hydroxide are generally insoluble except | when they are combined with alkali metals, NH4, Ca^2+, Sr^2+, Ba^2+ when they are somewhat soluble
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| CO3, PO4, S, SO3, C2O4, CrO4 are insoluble except | when combined with alkali metals and NH4
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| Cl^-, Br^-, I^- are soluble except | when combined with Ag+, Pb^2+, Hg2^2+
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| F^- is soluble except | when combined with Ca, Sr, Ba, Pb^2+, and Mg
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| SO4 is soluble except | when combined with Ca, Sr, Ba, and Pb^2+
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| Arrhenius' Acid Base Theory | Acids yield a hydrgeon ion and bases yield a hydroxide ion when dissolved in acqueous solution
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| Bronsted-Lowry Acid Base Theory | Acids donate protons, or hydrogen ions; bases accept protons, or hydrogen ions
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| Solution | A homogenous mixture in which a substance is dissolved in another
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| Solute | The substance that dissolves the solute
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| Solvent | The substance that dissolves in the solute
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| Acqueous Solutions | Solutions in which water is the solute
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| Electrolytes | Ions that conduct electricity. Strong acids and bases are strong electrolytes because they completely ionize in water
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| Precipitates | A solid that forms from the reaction of two substances in acqueous solutions
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| What is Ksp? | Ksp is the K equation for the solubility product that is formed. It is usually very small because only fractional amounts of insoluble solids are actually soluble in water.
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| What is a complex ion? What makes it more stable? | A complex ion is formed by a metallic ion and a Lewis base. The charge of the metallic ion determines how many anions will bond to it (it will be double). The larger the exponent, the more stable it is.
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| What is the Kw equivalent to? | Kw: 1.0x 10^-14
Use this to solve for Kb if given a Ka by division.
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| What must you do to the pOH to solve the pH? | Subtract from 14
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| If the base is not 1.0M (as in 1.0x 10^-3), then the exponent will not be the pH because of differences in molar concentration, what must you do? | Negative log it! -log()
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| Lewis acid-base theory | Acids accept electrons, and bases donate electrons. Whatever is an Arrhenius or Bronsted acid or base, is the same by Lewis' definition as well.
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| When are ice boxes used? | When there is a weak acid or base involved, because only partial dissociation occurs. When it is strong, assume there is 100% ionization.
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| Trick to remember what to do when the acid/base is weak for an ice box? | The ionization is so small, that the x is largely negligible. Only 1-10% will actually ionize.
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| What are the 7 strong acids? | HCl, HBr, HI, H2S04, HNO3, HClO4, H3PO4
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| What are the 7 strong bases? | Ba(OH)2, Ca(OH)2, LiOH, NaOH, KOH, RbOH, CsOH
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| Why is HF not a strong acid, but the rest of the halogens are? | HF has hydrogen bonds!
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| What makes an acid/base strong, rather than weak? | The more polar an acid/base is, the stronger it will be because the H+ will come right off, creating ions
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| If heat were added, would the pH of water still be 7.0x 10^-4? | No, the water would be more acidic.
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| What does neutralization really mean? | Neutralization means that the moles of acid= the moles of base?
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| What is special about the half-titration point? | pH= pKa
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| What are the scenarios in which pH=pKa? | 1. A perfect buffer
2. pH= pKa
3. The pH change (exponent) of the indicator's color
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| When looking at a titration curve, when can you expect a bump, meaning a buffer has formed? | When a weak acid or base is involved, when the acid is di or triprotic, and if the acid is originally in the beaker.
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| What equation should you use to calculate the pH of a buffer solution? | Henderson-Hasselbalch
pH= pKa + log(S/A)
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| When calculating the pH during a titration, what must always be the first step? | Find the number of moles used (moles times volume) and then subtract to find which one is left over.
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| When a strong acid and a strong base are mixed, what are the results? | Water and a neutral salt
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| Why do strong acids/bases burn? | Because they are ionizing on your skin, and changing the pH by donating or accepting excess hydrogens.
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| When writing net ionic equations, what are the only things that ionize? | Strong substances and aqueous solutions. Leave the rest alone, and there must always be a driving force: the evolution of a gas, or the formation of a precipitate
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