o lvl chesmistry help plz
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Methanoic acid + calcium -----> calcium methanoate
y is there a ate behind??? -
Possibly due to the nature of acid that the molecules combined gave to dat? (I am rubbishing, sorry)Originally posted by Classyfied:Methanoic acid + calcium -----> calcium methanoate
y is there a ate behind???
You got try asking your teacher? I left "O" level era long long ago so abit rusty......
So far all I know is 1 + 1 = 2, mass & volume, Singapore was called Temasek in da past (I not geography grp) and Pi (da maths calculation) = 22/7. You cannot find an absolute in decimal points.
Work hard for your "O" levels. You will be glad if you did after many many yrs later.
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This is the ate- group lor. Just like alcohol ie. Ethanol have the ol- group.
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acid+metal=water +metal salt
so easy.
zzzzzzzzzzz
common sense.
the "ate" is just a name what.
you cannot possibly have calcium methanoic rt?
plus the acid is neutralised already. -
cuz methanoic is CH3OH
then got the O
which then makes up the ate -
neutralised..sure?Originally posted by missqi:acid+metal=water +metal salt
so easy.
zzzzzzzzzzz
common sense.
the "ate" is just a name what.
you cannot possibly have calcium methanoic rt?
plus the acid is neutralised already.
and try writing "ate" is just a name during exams
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It's a naming convention, so as to easily recognize the same groups of chemicals, and the reactions they have to certain chemicals.Originally posted by Classyfied:Methanoic acid + calcium -----> calcium methanoate
y is there a ate behind???
For example, all elements of Group VII -ine. One look at their names, you would know they are Group VII elements.
Organic Chemistry Nomeclature
IUPAC -
i forgot everyth leh. lol but i did get a2 for pure chem.Originally posted by mystiv:neutralised..sure?
and try writing "ate" is just a name during exams -
just a naming convention for the salt.....e.g. methanoate from methanoic acid, sulphate from sulphuric acid etc
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The 'ate" behind is the oxygen produced
"ate" jz means oxygen -
H-C=O + Ca ---> H-C=0 + H2Originally posted by Classyfied:Methanoic acid + calcium -----> calcium methanoate
y is there a ate behind???
xxx|xxxxxxxxxxxxx|xxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxx
xxxOHxxxxxxxxxxxO-Na+xxxxxxxxxxxxxxxxxxxxxxxxxxxx
The C=O group is the "oate" part. Similarly, CH3COO- is ethan "oate"...
xxxx|xxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxx
xxxxO-xxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxx
don't mind the xxx cos the forum does not format nicely. -
Quite a number of pple here have already correctly answered your question. Just to add to their replies :Originally posted by Classyfied:Methanoic acid + calcium -----> calcium methanoate
y is there a ate behind???
The methanoate ion is the HCOO- ion. In the 'O' level syllabus, it is usually the ethanoate ion (CH3COO-) that is featured in the exams, since ethanoate acid (commonly known as vinegar), is more commonly used in daily life than methanoate acid.
The ionic eqn is :
2 H+ (aq) + 2 HCOO- (aq) + 1 Ca (s) ------> 1 Ca2+ (aq) + 2 HCOO- (aq) + 1 H2 (g)
Notice that the participating ions are hydrogen and calcium, while the spectator ion is the methanoate ion. You have to delete away the spectator ions for ionic eqns, but I left it in there for explanation's sake.
Also notice that the hydrogen is reduced, the calcium is oxidized, while the oxidation state of the methanoate ion remains unchanged. Thus the calcium acts as the reducing agent, while the (hydrogen ions in the) acid acts as the oxidizing agent.
I'm an 'O' level Chem teacher and tutor. But at the 'A' level or 'H2' level (which I tutor), I much prefer Biology. It's a lot more enjoyable than Chem. -
Posted by missqi:
plus the acid is neutralised already.
Posted by mystiv :u say neutralised.. u sure?
My 2 comments :
1st comment.
Neutralization technically occurs between an acid and a base. A base is a substance that absorbs hydronium / hydroxonium ions (H3O+) when dissolved in water (a proton acceptor). Other than the common bases (oxides of metals and hydroxides of alkali metals), sodium carbonate and ammonia are by this definition also considered bases.
Metals by *themselves* however, such as calcium, are not quite considered bases. But when they react with oxygen or water, as long as they're reactive enough, such as calcium is, they *do* form metal oxides and hydroxides which are bases, and thus can carry out neutralization.
And this is what occurs here.
2nd comment.
To determine if the acid is truly "completely neutralized", which was the topic of discussion between "missqi" and "mystiv", one would have to determine (by simple mathematics) the limiting reactant.
The mathematical procedure/working is simple (memorize this method, 'O' level Chem students!) :
Compare the Experiment Reactant Mole Ratio to the Equation Reactant Mole Ratio. Remember that the Experiment is "what you have", while the Equation is "what you need".
Let's take a simple equation, 2H2O + O2 ---> 2H2O2
Say you have (you might be given values in mass (g) or (for gases) in volume (dm3), if so convert to moles) 1 mole of H2O and 2 moles of O2, for the experiment. Therefore, taking H2O as numerator and O2 as denominator, we have Experiment mole ratio (of reactants) of 1:2 or 0.5
From Eqn mole ratio, the corresponding Equation mole ratio (of reactants) is 2:1 or 2.0
Comparing Exp mole ratio with Eqn mole ratio, we see that our Exp mole ratio is less than our Eqn mole ratio.
And (ALWAYS) looking at the NUMERATOR reactant (in our case we have chosen H2O), we realize that "what we have" (ie. Exp mole ratio) of H2O, is less than "what we need" (ie. Eqn mole ratio) of H2O.
Therefore, H2O is the limiting reactant.
If, on the other hand our Exp mole ratio was greater than our Eqn mole ratio, which means what we have (for the numerator reactant) is more than what we need, so the numerator reactant (in this case H2O) is the excess reactant, therefore the limiting reactant must be the other reactant (in this case O2).
May this be of some usefulness or helpfulness to any 'O' level Chem student reading this. I make sure my students use this very clear, simple method, to determine limiting reactants. -
LOLX>Originally posted by missqi:acid+metal=water +metal salt
so easy.
zzzzzzzzzzz
common sense.
the "ate" is just a name what.
you cannot possibly have calcium methanoic rt?
plus the acid is neutralised already.
Acid + Metal --> Hydrogen + (Metal)Salt
It's Hydrogen not Water, dude. -
I never cared about equations since I keep blowing the labs up with acetone peroxide.Originally posted by UltimaOnline:Posted by missqi:
My 2 comments :
1st comment.
Neutralization technically occurs between an acid and a base. A base is a substance that absorbs hydronium / hydroxonium ions (H3O+) when dissolved in water (a proton acceptor). Other than the common bases (oxides of metals and hydroxides of alkali metals), sodium carbonate and ammonia are by this definition also considered bases.
Metals by *themselves* however, such as calcium, are not quite considered bases. But when they react with oxygen or water, as long as they're reactive enough, such as calcium is, they *do* form metal oxides and hydroxides which are bases, and thus can carry out neutralization.
And this is what occurs here.
2nd comment.
To determine if the acid is truly "completely neutralized", which was the topic of discussion between "missqi" and "mystiv", one would have to determine (by simple mathematics) the limiting reactant.
The mathematical procedure/working is simple (memorize this method, 'O' level Chem students!) :
Compare the Experiment Reactant Mole Ratio to the Equation Reactant Mole Ratio. Remember that the Experiment is "what you have", while the Equation is "what you need".
Let's take a simple equation, 2H2O + O2 ---> 2H2O2
Say you have (you might be given values in mass (g) or (for gases) in volume (dm3), if so convert to moles) 1 mole of H2O and 2 moles of O2, for the experiment. Therefore, taking H2O as numerator and O2 as denominator, we have Experiment mole ratio (of reactants) of 1:2 or 0.5
From Eqn mole ratio, the corresponding Equation mole ratio (of reactants) is 2:1 or 2.0
Comparing Exp mole ratio with Eqn mole ratio, we see that our Exp mole ratio is less than our Eqn mole ratio.
And (ALWAYS) looking at the NUMERATOR reactant (in our case we have chosen H2O), we realize that "what we have" (ie. Exp mole ratio) of H2O, is less than "what we need" (ie. Eqn mole ratio) of H2O.
Therefore, H2O is the limiting reactant.
If, on the other hand our Exp mole ratio was greater than our Eqn mole ratio, which means what we have (for the numerator reactant) is more than what we need, so the numerator reactant (in this case H2O) is the excess reactant, therefore the limiting reactant must be the other reactant (in this case O2).
May this be of some usefulness or helpfulness to any 'O' level Chem student reading this. I make sure my students use this very clear, simple method, to determine limiting reactants.
But according to logic, you are right in your equations. -
is ammonium nitrate explosives?
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in very pure form with a charge detonatorOriginally posted by ceecookie:is ammonium nitrate explosives? -
yes, so are a lot of things.Originally posted by ceecookie:is ammonium nitrate explosives? -
Hell, gimme a detonator and very fine flour, I show you how to blow things up.Originally posted by the.owl:yes, so are a lot of things.