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
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.
25 ml of 0.105 M HCl is titrated with 0.210 M NaOH
a. What is the ph after 5 ml of the base is added?
b. what is the ph at the equivalence point?
c. What is the ph after 15 ml of the base added?
d. how many ml of the base will be required to reach the end
point?
A 50.0ml aliquot of 0.100 M NaOH is titrated with
0.200 M HCl. Calculate the pH of the solution after addition of
0.0, 5.0, 10.0, 25.0, 35.0, 45.0, 55.0 of HCl. Plot the titration
curve in a graph paper.