In a .1M aq. soln of NaCN, how would you determine the major species (other than water)? And how would you determine the pH (not exact pH, I just want to know how to know if it is acidic ie. <7, etc). Thanks in advance
I figured out what I was doing...I ended up using the Van't Hoff Equation and the enthalpies of formation to solve for K at 100 C. This stuff is so time consuming...
Calculate the equilibrium constant at 25°C and at 100.°C for each of the following reactions, using data available in Appendix 2A. Remember that the organic molecules are in a separate section behind the organic molecules in Appendix 2A. (a) HgO(s) Hg(l) + O2(g) at 25&...
When 1.00 g of gaseous I2 is heated to 1000. K in a 1.00 L sealed container, the resulting equilibrium mixture contains 0.830 g of I2. Calculate Kc for the dissociation equilibrium below. I2 <--> 2 I What I did was converted the initial I2 into moles then molarity since...
When 1.00 g of gaseous I2 is heated to 1000. K in a 1.00 L sealed container, the resulting equilibrium mixture contains 0.830 g of I2. Calculate Kc for the dissociation equilibrium below. I2 <--> 2 I What I did was converted the initial I2 into moles then molarity since ...
I've heard this one before: "A meteor is a flash of light made by a falling meteorite"
nevermind--after 50 hours of pulling my hair out I finally arrived at the answer :)
And when solving for molality do I need to use the formula dT=Kf*molality? Or do I find it independently of this equation?
I am confused by the 1% by mass part...I don't understand what it really even means or if I am multiplying something by 1% or what? I did eventually realize I had to multiply by 3--I have never seen a problem like that before so I was slow to catch on. Thanks for your help
A 1.00% by mass MgSO4(aq) solution has a freezing point of -0.192°C. Water has a kf of 1.86 (K·kg)/mol. (a) Estimate the van't Hoff i factor from the data. (b) Determine the total molality of all solute species. I can probably figure out the second part of the q...