THis is a ph Equilibirum problem.
10^(-2)M of acetic acid at 25 degrees Celcius. What are the ion
concentrations?
ka= 1.8x10^-5
Final Answers:
[H+]= 4.15 x10 ^-4
[HAc]=9.59x10^-3
[OH+]=2.41x10^-11
[Ac-]=4.15x10^-4
Calculate the pH and pOH for the following solutions:
a) 0.0450 M NaOH
b) 0.160 M Ca(OH)2
c) a 1:1 mixture of 0.0125 M HCl and 0.0125 M Ca(OH)2
d) a 2:3 mixture of 0.0125 M HNO3 and 0.0125 M KOH
Calculate the pH at 25 degrees Celcius of a 0.35M aqueous
solution of phosphoric acid (H3PO4). (Ka1, Ka2, and Ka3 for
phosphoric acid are 7.5x10^-3, 6.25x10^-8, and 4.8x10^-13,
respectively.)
a) Calculate the pH and pOH for a solution of 0.09952 M NaOH
b) How many acidic protons are there in 0.6137 g of KHP?
c) What volume of 0.1157 M NaOH is required to obtain the
endpoint of a reaction with 0.5938 g of KHP?
1a) The system is at 25 degrees Celsius and the surroundings are
at degrees Celcius. The system is a closed system.
a) thermal energy will flow from system to surrounding
b) thermal energy will flow from surrounding to system
c) there will be no net flow of thermal energy
1b) The system is at 25 degrees Celsius and the surroundings are
at 0 degrees Celcius. The system is an isolated system
a) thermal energy will flow from system to surrounding...
Consider the titration of 0.050 M HCl with 0.050 M NaOH.
Calculate the pH: (a) of the pure HCl solution; (b) of 25.00 mL
acid plus 12.50 mL base; (c) at the quivalence point; and (d) of
25.00 mL acid and 37.50 mL base.