Question | Answer |
Alkali metals are always _____ | Soluble |
Other soluble ions are: | NH4, NO3, ClO3, ClO4, C2H302 Ammonium, Nitrate, Chlorate, Perchlorate, Acetate |
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 |
CO3, PO4, S, SO3, C2O4, CrO4 are insoluble except | when combined with alkali metals and NH4 |
Cl^-, Br^-, I^- are soluble except | when combined with Ag+, Pb^2+, Hg2^2+ |
F^- is soluble except | when combined with Ca, Sr, Ba, Pb^2+, and Mg |
SO4 is soluble except | when combined with Ca, Sr, Ba, and Pb^2+ |
Arrhenius' Acid Base Theory | Acids yield a hydrgeon ion and bases yield a hydroxide ion when dissolved in acqueous solution |
Bronsted-Lowry Acid Base Theory | Acids donate protons, or hydrogen ions; bases accept protons, or hydrogen ions |
Solution | A homogenous mixture in which a substance is dissolved in another |
Solute | The substance that dissolves the solute |
Solvent | The substance that dissolves in the solute |
Acqueous Solutions | Solutions in which water is the solute |
Electrolytes | Ions that conduct electricity. Strong acids and bases are strong electrolytes because they completely ionize in water |
Precipitates | A solid that forms from the reaction of two substances in acqueous solutions |
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. |
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. |
What is the Kw equivalent to? | Kw: 1.0x 10^-14
Use this to solve for Kb if given a Ka by division. |
What must you do to the pOH to solve the pH? | Subtract from 14 |
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() |
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. |
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. |
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. |
What are the 7 strong acids? | HCl, HBr, HI, H2S04, HNO3, HClO4, H3PO4 |
What are the 7 strong bases? | Ba(OH)2, Ca(OH)2, LiOH, NaOH, KOH, RbOH, CsOH |
Why is HF not a strong acid, but the rest of the halogens are? | HF has hydrogen bonds! |
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 |
If heat were added, would the pH of water still be 7.0x 10^-4? | No, the water would be more acidic. |
What does neutralization really mean? | Neutralization means that the moles of acid= the moles of base? |
What is special about the half-titration point? | pH= pKa |
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 |
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. |
What equation should you use to calculate the pH of a buffer solution? | Henderson-Hasselbalch
pH= pKa + log(S/A) |
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. |
When a strong acid and a strong base are mixed, what are the results? | Water and a neutral salt |
Why do strong acids/bases burn? | Because they are ionizing on your skin, and changing the pH by donating or accepting excess hydrogens. |
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 |