CHEM 1C Chapter Notes - Chapter 18: Ionic Compound, Chemical Equation, Lewis Acids And Bases
Document Summary
Calculating the ph of a buffer solution: common ion effect = solution contains two substances that share a common ion. Use the stoichiometry of the neutralization equation to calculate the changes in the amounts (in moles) of the buffer components upon addition of the acid or base: the equilibrium calculation. Use the new amounts of buffer components to work an equilibrium problem to find ph. Buffers containing a base and its conjugate acid: calculate ph of solution same as before but must find pka of conjugate acid. 18. 3 buffer effectiveness: buffer range and buffer capacity. Absolute concentrations of the acid and conjugate base: a buffer is most effective when the concentrations of acid and conjugate base are high, more dilute the buffer components, the less effective the buffer. Acid-base titration = a basic (or acidic) solution of unknown concentration reacts with an acidic (or basic) solution of known concentration. Indicator = a substance whose color depends on the ph.
