Determine the mass of NH4Cl and the volume of 0.250 M
NaOH solution required to make 0.15 L of a buffer solution at
pH=9.20 and at a total concentration of 0.42 M.
pKa(NH4+)=9.25.
1) Mass of NH4Cl:
2) Volume of NaOH solution:
Determine the mass of
C6H4(CO2H)2 and the
volume of 0.400 M NaOH solution required to make 1.10 L of a buffer
solution at pH=3.00 and at a total concentration of 0.38 M.
pKa1(C6H4(CO2H)2)=2.95.
1. Mass of
C6H4(CO2H)2 (g):
2. Volume of NaOH solution (L):
Find the pH of the following solutions: a mixture of 10.0 mL
NaOH solution having pH 11.00 and 10.0 mL HClO4 having pH 1.00.
2.) Using activities calcalute the pH and concentration of H+ in
pure water containing 0.05 M CaCl2 at 25 degrees C
How do you determine the mass needed to make a certain molarity
and certain pH solution? For example, if I need to make 300 mL of
0.05 M Tris Base and 0.05 M NaCL (pH 8.2) from 2M of both, how do I
do the math for that and get the grams needed of each?
Also how do you use the Henderson-Haseelbach equation to
determine how much .1 M KH2PO4 to add to 100 mL of of K2HPO4 to
give...