A buffer containing .40L of .40M C6H5CO2H and .20 M C6H5CO2Na is prepared. What is the pH of the solution? Ka for C6H5CO2H = 6.5 x 10^-5
pH = 3.89
100
Isotopes of Hydrogen?
protium, deuterium, tritium. Know how to draw!
100
A reaction that happens on its own with no external influence is a :
spontaneous reaction
100
If H=1.8 and S=-113, will the reaction be spontaneous? If not, at what temp would it be spontaneous?
nonspon, -15.9K. this means it would never be spontaneous because it is -K.
200
Weak Acid + Strong Base =
base dominates -> basic solution. pH>7
200
Calculate the titration of 25.0mL of .100M acetic acid by NaOH after the adition of 10.0mL of .100M NaOH. Ka for CH3COOH = 1.8x10^-5
pH = 4.57
200
What the 3 types of binary hydrides and an example of each?
Ionic Hydrides:H with group 1A 2A metals,NaH. Covalent Hydrides:H with nonmetal,CH4. Metallic Hydrides:Hwith transition metal,MH
200
What are the two types of entropy?
positional/arrangement and energy entropy
200
H2O(l) -> H2O(g). The G for H2O(l) is -237.2 and H2O(g) = -228.6Kj/mol. What is G for th reaction? spon or nonspon?
8.61Kj/mol. nonspon
300
If an anion is a base, will an ionic compound containing it be more soluble is acidic or basic solution?
Acidic solution.
300
What is the molar solubility (mol/L) os BaF2 in water at standard state conditions?
Ksp for BaF2 = 1.8 x 10^-7.
3.56 x 10^-3M
300
2 forms of phosphorous? Which is more stable? Why?
White and Red. Red is more stable because it has less angle strain.
300
What are the 3 laws of thermodynamics?
1-in any process, the total E of a system and its surroundings is constant(energy is conserved).
2-in any spontaneous process the entropy of the universe increase.
3-the entropy of a perfectly ordered crystalling substance at 0K is zero.
300
Find the deltaGprime for Fe(OH)2(s)->Fe+2(aq)+2OH-(aq). The Ksp = 1.6x10^-14. Assume standard state conditions. Find the answer in Kj/mol.
78.7Kj/mol
400
What regulates pH and can react away acid or base?
What is a buffer solution (HA/A- mix)
400
If 30.0mL of .20M Ba(NO3)2 is added to 70.0mL of .20M Na2CO3, will BaCO3 precipitate out? Ksp for BaCO3 = 8.1x10^-9
Q = 8.4x10^-5. Q>Ksp=BaCO3 will precipitate out
400
How do you synthesize H2 in the lab?
Active metal + acid. Very active metal + water. Electrolysis of water.
400
What are the requirements of G,H,S for a spontaneous reaction?
-G,-H,+S
400
Find the Kp and deltaGprime for PCl5->PCl3+CL2. delta G's are -325, -286, and 0.
G = 391Kj/mol. Kp = 1.45x10^-7.
500
Ion product IP or Qc: if IP>Ksp? if IP=Ksp? if IP<Ksp?
IP>Ksp=shift to reactants,precipitate. IP=Ksp=equilibrium,saturated solution.
IP
500
A buffer containing .50L of .50M C6H5CO2H and .30M C6H5CO2Na is prepared. Ka for C6H5CO2H = 6.5x10^-5. Calculate the pKa and the pH of the buffer using Henderson Hasselbalch equation.
pKa = 4.19. pH = 3.97
500
What are the 3 types of oxides and examples of each?
ionic oxide:O2 with metal->metal oxides, MgO. Covalent Oxides:nonmetal oxides, N2O5+H2O. Amphoteric Oxides:acid and base properties, Al,Ga,Sn,Pb.
500
At what temp will a reaction with -G,+H,+S be spontaneous?
High tempertures.
500
Consider a reaction, 2SO2(g) + O2(g)->2SO3(g). If each reactant and product has a partial pressure of 2.0atm, G=-141.8Kj/mol, find the G at 25C. spon or nonspon?