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# MCAT Acids/Bases

Question | Answer |
---|---|

What is the relation of K(sp), solubility constant to soulubility? | K(sp) is directly related to solubility; therefore the larger the K(sp) the more soluble the product |

What is the common ion effect? | Another form of Le Chatelier's Principle, the the decrease in the solubility of a salt occurs because another salt is added that contains one of its ions. |

What is the relatonship bw autoionization of water K(w) and temp | it increases when temp increases |

polyprotic | can accept or donate more than one H+ |

high [H] means... | low pH and the solution is acidic |

pH + pOH = | 14 |

pH = | -log[H] or -log[H3O+] |

pOH = | -log[OH] |

What is the relation bw K(a) and pKa? | The larger the K(a) value the smaller the pKa value and therefore the stronger the acid |

What is the Henderson-Hasselbalch equation? | pH = pKa + log {[conjugate base]/[weak acid]} |

what happens at a half-equivalence point? | the pKa equals the pH |

K(w) | = [H3O+][OH-] |

Titration equation | pH = [vol acid]/ [vol base] |

pKa + pKb = | 14 |

Created by:
studypants
on 2009-08-19