Flashcards in lab practical study guide Deck (28):
(buffers) the hydrogen ion concentration and the pH depend on the value of the .... and the ratio of the concentrations of ....
acid dissociation constant, Ka; acid and conjugate base
(buffers) pKa + pKb=
(buffers) experiment overview: in this experiment the pH of water and a number of solutions will be measured, and then acids and bases will be added to see how... Several buffer solutions of different pH values will be prepared and tested for their ability to
the pH is affected; resist change of pH
(buffers) part 1: .. mL distilled water plus ... drops HCl and ... drops ...
... mL NaCl plus ... drops .. and .. drops ...
20; 3; 3; NaOH; 20; 3; HCl; 3; NaOH
(buffers) part 2: prepare a buffer using ... mL of .. M.... and .. mL ... M...
add 3 drops ... and then ....
repeat with a buffer of ... mL ... M .... and ... mL ... M ...
10; .1M; HC2H3O2; 10; .1; NaC2H3O2
10; .1; NH3; 10; .1; NH4Cl
(buffers) part 3: unknown solid acid of mass ... to ... g; dissolve in ... mL of distilled water; pour ... mL into a second flask and add 2 drops phenolphthalein; titrate with ... M ...; add the same volume of water as titrant used to titrate to flask 1 to make the ..... of the two solutions the same
1.8; 2.0; 150; 75; .2; NaOH; concentrations
(buffers) part 3 (continued): combine ... mL of weak acid solution with .. mL of conjugate base solution to make a buffer. measure pH, ths is also the ...
create buffer of assigned pH and test effectiveness
10; 10; pKa
(electrochemistry) an electrochemical cell is produced when an oxidation reaction and a reduction reaction occurs ...., and their resulting electron transfer between the two processes occurs through an ....
spontaneously; external wire
(electrochemistry) the oxidation and reduction reactions are physically separated from each other and are called ...
(electrochemistry) a half-cell can be prepared from almost any metal in contact with a
solution of its ions
(electrochemistry) since each element has its own electron configuration, each element develops a different ...., and different combinations of oxidation and reduction half-cells result in different .... for the completed electrochemical cell
electrical potential; voltages
(electrochemistry) the standard reduction potential is the voltage that a half-cell, under standard conditions develops when it is combined with the
standard hydrogen electrode
(electrochemistry) the more positive the reduction potential, the .... the reduction
(electrochemistry) a spontaneous cell (a battery) can be constructed if two half-cells are connected internally using a ..., and externally using a ....
salt bridge; metallic connector
(electrochemistry) the symbol | refers to a
(electrochemistry) the symbol || indicates a
salt bridge between the two ion solutions
(electrochemistry) nernst equation:
E=E° - .0592V/n * logQ
(electrochemistry) part 1: a standard table of reduction potentials is constructed; microscale half-cells are constructed by placing a piece of metal into a ... M solution of its .... for each metal in the series (Cu2+, Fe3+, Pb2+, Mg2+, Ag+, Zn2+). the half-cells are connected by a salt bridge constructed of a strip of .. soaked in a solution of ....
1 M; ions; filter paper; potassium nitrate
(electrochemistry) part 1 (continued): the ... half-cell is chosen as the reference standard and is assigned a value of 0.00 volts. voltage values should correlate with those found in ..., but they will differ by the value of .... for the ...
zinc; published tables; E°; zinc electrode
(electrochemistry) part 2: the nernst equation is applied to the voltage measurement of a cell with ..... A solution of .... M Cu2+ is prepared by a ...., and the voltage of the cell Zn(s) | Zn2+ (1.0 M) || Cu2+ (0,0010 M) | Cu(s) is measured and is then compared to that calculated from the ....
nonstandard copper ion concentration; .0010; serial dilution; nernst equation
(electrochemistry) part 3: the solubility product constant of AgCl is determined from the .... and the .... in which the zinc half-cell is connected to a solution containing a trace of ... in a ... M solution of ...
nernst equation; voltage of a cell; Ag+ ions; 1.0; NaCl
voltaic/galvanic cell: apparatus that produces ... directly from the chemical energy released in a ....
electrical energy; redox reaction
electrochemical cell: a device capable of either generating ...or ....through the introduction of ....energy
electrical energy from chemical reactions; facilitating chemical reactions; electrical
electrolytic cell: A type of chemical cell in which the flow of .... causes a .... to occur.
electric energy from an external source; redox reaction
Electrode potential is defined as the potential of a cell consisting of the.... acting as a cathode and the ... acting as an anode.
electrode in question; standard hydrogen electrode
Potential of a cell is the.... between the two electrodes of a ....
electric potential difference; voltaic cell
oxidizing agent: a substance that tends to bring about ... by being ...