Gooferking Science
Hazard to Self
Posts: 97
Registered: 17-7-2013
Location: Somewhere in Kansas, USA...
Member Is Offline
Mood: Halogenated
|
|
From sodium bromide to bromine equation question
I know the first part of the reaction:
NaBr + HCl --> HBr + NaCl
But what is the byproduct of the second reaction:
HBr + Ca(ClO)2 --> Br2 + ?
Anyone know?
|
|
|
bfesser
|
Thread Moved
19-7-2013 at 07:23 |
neptunium
National Hazard
Posts: 987
Registered: 12-12-2011
Location: between Uranium and Plutonium
Member Is Offline
|
|
4HBr+Ca(ClO)2 = CaCl2 + 2Br2 + 2H2O
|
|
|
Gooferking Science
Hazard to Self
Posts: 97
Registered: 17-7-2013
Location: Somewhere in Kansas, USA...
Member Is Offline
Mood: Halogenated
|
|
Thanks neptunium!
|
|
|
AJKOER
Radically Dubious
Posts: 3026
Registered: 7-5-2011
Member Is Offline
Mood: No Mood
|
|
A word of advice on anyone providing a reaction equation like below:
4HBr+Ca(ClO)2 = CaCl2 + 2Br2 + 2H2O
without noting it is, in fact, a net summary equation. As such, it may be highly conditional with respect to the observed products. For example, any
excess amounts of either starting reactants and the reaction conditions (temperature, solid or aqueous, pH,...) could introduce other
unwanted/unexpected products (see thread http://www.sciencemadness.org/talk/viewthread.php?tid=25415 ).
As an extreme case, I will cite an example where a possible intermediate product includes NH4NO2. For example, the rapid heating of aqueous NaNO2 and
NH4Cl would be unwise in a low pH and concentrated solution. The success of the net reaction (to ostensibly form N2 gas) is not only in doubt, but
ones physical well being with respect to an inventory of remaining body parts is also a open question. Another example, the apparent simple action of
Oxalic acid on a chlorate to produce Chloric acid. However, do not use an excess of H2C2O4 so as to avoid an explosion from ClO2 liberated from the
reduction of the newly formed HClO3 by the excess Oxalic acid! Similarly, the action of H2C2O4 on sulfate can form H2SO4, but concentrated Sulfuric
acid oxidizes any excess Oxalic acid to CO, CO2 and H2O in apparently a violent and extremely dangerous manner. Please see http://www.theodora.com/encyclopedia/o/oxalic_acid.html and my thread at http://www.sciencemadness.org/talk/viewthread.php?tid=18963&... to quote Formatik:
"I made another attempt with the copper sulfate and oxalic acid. But this time used larger amounts. This time I only filtered and siphoned the
filtrate, and did not evaporate and collect more solids. But this time I just boiled down the filtrate. Something very bad happened on boiling near
the end, all of the sulfuric acid and contents in the 600mL beaker ejected entirely!..."
Now, I understand that chemical reaction equations are a favorite among academics, but I would advise anyone actually practicing chemistry to
research, ask questions, and consider all steps comprising a net summary reaction (and even new products with excess reactants per my second example)
for more important issues than just improving yield.
[Edited on 22-8-2013 by AJKOER]
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
