Jump to content

Borek

Senior Members
  • Content Count

    101
  • Joined

  • Last visited

Community Reputation

11 Neutral

About Borek

  • Rank
    Meson
  1. Go to chemspider and search for the formula - this yields list of a known compounds, not every possible one (whether it exists or not). And some compounds that look OK on paper don't exist in reality.
  2. Try. I don't see why not, I believe around 200 deg C is enough to dry it. I can be wrong though. Note: if it absorbed enough water it will melt first (actually it will not melt, but it will dissolve in its own hydration water). You may have to wait several hours before it dries out. Question is if you need it perfectly dry, could be partial drying will be enough to make it possible to prepare a powder.
  3. Sodium chloride is either solid - when it is solid, or aqueous - when it is dissolved. "Just sodium chloride" doesn't say anything about whether it is solid or aqueous.
  4. 5 second googling: http://www.ncbi.nlm.nih.gov/pubmed/15653512 Even if not perfect, it is a starting point.
  5. Basically that's what chemical warfare is about. Wikipedia has a List_of_chemical_warfare_agents
  6. I trolled your wall

  7. M is usually used for molarity, not molality, so it can be a little bit confusing here. Borek
  8. Check this solution preparation example. Especially operating procedure at the bottom of the page. Borek -- concentration conversion
  9. Try this limiting reagent lecture. Borek -- equation balancer and stoichiometry calculator
  10. C1V1 = C2V2 - yes, but 1 means NaOH solution and 2 means HCl solution. The equation looks the same as in teh case of dilution, but it is not the same. So what you have is 18.32ml*0.08045M=25ml*C(HCl). Solve for C(HCl). Looks to me like your error was about 0.55%. Borek -- Stoichiometry calculator www.pH-meter.info/pH-electrode
  11. See water ion product to check how water dissociation constant changes with temperature. In general no ion can facilitate water dissociation, however, if you dissolve an inert salt increasing ionic strength of the solution, you will observe changes in the water dissociation. But this effect is universal, it is not limitied just to water dissociation. See ionic strength and activity coefficients lecture for details.
  12. Exponentially, just like Gauss curve. In fact Gauss curve is a solution of diffusion equation for the initial concentration being 1 at x=0 and 0 elsewhere. Borek -- Stoichiometry calculator www.pH-meter.info/pH-electrode
  13. Download BATE and play with titration curves to get familar with them Program is commercial but there is a 30-day free trial. Borek -- Chemical calculators at www.chembuddy.com BATE - pH calculator
  14. You must find out how to convert molarity to molality. Correct conversion formula will contain density and molar mass - you have to solve for density. Check out these concentration lectures for hints on converting (read about %ww to molarity conversions for general outline). Strange thing is that 1.0000M solution of KCl is 1.0312 molal. Looks like the data in question are questionable. Borek -- Chemical calculators at www.chembuddy.com concentration conversion calculator
  15. Borek

    Titrations

    Start with learning about Henderson-Hasselbalch equation. Then check buffer pH question 1 and buffer pH question 2 - although they don't address specifically your problem, they show how to deal with buffer preparation. Acetic buffer case is not different.
×
×
  • Create New...

Important Information

We have placed cookies on your device to help make this website better. You can adjust your cookie settings, otherwise we'll assume you're okay to continue.