Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: richie94sho on May 20, 2006, 10:25:00 AM
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This question is for a high school chemistry class. This question was assigned friday, may 19th. the first person to report to class before school monday, may22nd is promised 10 % on the final exam. The question goes as following:
You are given three flasks containing different substances in aqueous solution.
1.00 M AgNO3, 1.00 M NaClO3, and 1.00 M Na3PO4.
You have access to the following pieces of equipment:
1 evaporating dish
1 funnel
1 hot plate
1 stirring rod
1 triple beam balance
1 graduated cylinder
2 empty beackers
2 pieces of filter paper
To solve the equation I must describe and show all calculations for the steps I would take to produce 50 grams of solid crystal sodium nitrate. (NaNO3)
I dont have much to offer other than as many gmail invites as you can take, but i would be extremeley grateful for an answer or help solving this problem. If you have the knowlege it requires to solve it. please describe and show the calculations neatly so I can earn the extra credit. Thank you very much and any help is greatly appreciated.
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Write a balanced reaction: AgNO3 + Na3PO4
Calculate, how many mole equivalent for 50 g NaNO3
Do reaction
Filtate solid Ag3PO4
Remowe water from filtrate
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thanks for the help. keep the comments coming. i'd like to see consistant responses just to be sure i thats the correct process
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Write a balanced reaction: AgNO3 + Na3PO4
Calculate, how many mole equivalent for 50 g NaNO3
Do reaction
Filtate solid Ag3PO4
Remowe water from filtrate
that's it.
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alright lets dumb this down to a tenth grade level. perhaps a little more in detail. I'm not asking for the answer, just a how to.
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How hard is to measure the required volume of reagents, then mix them in a beaker?
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Write a balanced reaction: AgNO3 + Na3PO4
Calculate, how many mole equivalent for 50 g NaNO3
Do reaction
Filtate solid Ag3PO4
Remowe water from filtrate
Can somebody please explain the do reaction part in detail perhaps with an answer. Time is ticking!
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You can do a reaction by mixing two reactants together in a suitable solvent and stirring.
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to be more specifice i need to know how much of each reactant to be mixing. if somebody could answere me that, i'm set.
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As the others have already said start by writing a balanced equation...
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done that, im on step three of the equation which is to do the reaction. i need somebody to explain the whole step.
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Well that is what I am trying to do, so first step is write the balanced equation for me....
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AgNO3+Na3PO4=NaNo3+AgNa2PO4
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Ok so first you need the correct equation:
3AgNO3 + Na3PO4 = Ag3PO4(s) + 3NaNO3
And I think you said you want to make 50g of sodium nitrate so you need to calculate how many moles of sodium nitrate that is and use this number and the ratios from the balanced equation to work out how many moles of reactants you need for this. You can then convert this to how much 1 M solution you need.
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(https://www.chemicalforums.com/proxy.php?request=http%3A%2F%2Fi43.photobucket.com%2Falbums%2Fe373%2Frichie94sho%2Fscan.jpg&hash=9792fdbe9b6667c2d237fae0171fc23ee253b4c3)
this is my final conclusion tell me what you think.
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Ok, but your calculations are a bit wrong. Firstly the original question says that you have 1.00M solutions of your salts so you will need to measure out volumes of the reactants, ie how many mL's of AgNO3 solution of 1.00M is required to make 50g (0.59moles) of NaNO3. Second don't forget that for every 1 mole of silver nitrate you only need 1/3 as much Na3PO4.
Otherwise it is looking good. :)
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In Step 4, you're filtering out the precipitated Ag3PO4. There shouldn't be any Na3PO4 left at this point, just NaNO3 & water.
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In Step 4, you're filtering out the precipitated Ag3PO4. There shouldn't be any Na3PO4 left at this point, just NaNO3 & water.
Yes, good catch there wereworm definitely filtering out the solid Ag3PO4 :)