Question

A 50.00mL AgNO3 solution with unknown concentration reacts with excess Na2CO3. A precipitate of Ag2CO3 is formed.

a) write the equation for the reaction:
I think it's AgNO3 + Na2CO3 --> Ag2CO3 + NaNO3

b) after filtering and drying, the mass of the precipitate is measured as 2.76g. Calculate the number of moles of precipitate that are formed by the reaction.
I think it's 2.76/275.7453 = 0.010009mol

c) calculate the number of moles of solution that react.
I'm not really sure how to do this

d) determine the concentration of the AgNO3 solution in mol/L.
Not really sure how to do.

Answer 1

@aaronq could you help me out again

Answer 2

@JoannaBlackwelder

Answer 3

You need to balance your reaction before you can use it.

Answer 4

a)its about double displacement in a precipitate reaction. so your equation is correct.

Answer 5

b) Number of moles=Mass(g)/Molar Mass(g/mol)

Answer 6

c) i think we are going to use mole ratio according to your balanced chemical equation.
2AgNO3 + Na2CO3 --> Ag2CO3 + 2NaNO3

Answer 7

d) you are given AgNO3 volume and its number of moles from c)
Use concentration(mol/dm^3)=Number of moles/Volume(dm^3)
Make sure you Change 50.00 ml to dm^3 by dividing by 1000

Answer 8

@Abmon98 for c) which mole ratios should i be looking at though?

Answer 9

AgNO3 : Ag2CO3

Answer 10

so i use the .001mol and multiply it by 2 since the ratio is 2:1 and then I multiply that by the mass of AgNO3 right @Abmon98

Answer 11

.01mol*

Answer 12

nope thats incorrect dont multiply it by mass you need the solutions concentratio so after you solve the mole ratio to get the number of moles of solution needed to produce 0.01 mol of ppt. read part d)

Answer 13

no I mean for c not d

Answer 14

I think it's 2.76/275.7453 = 0.010009mol now you have calculate the number of moles of ppt produced. we need to know the number of moles of solution (AgNO3) that reacted to produce the 0.010009 moles of ppt we use mole ration according to the balanced chemical equation the mole ratio of AgNO3 to Ag2CO3 is 2:1

Answer 15

yeah I think that's what I said lol maybe I'm not saying it right but yeah that's definitely what I was thinking. Ok so Now I've gotten .02mol solution reacts for c. Now where do I start with D? I just convert 50mL to L and divide .02/.05 right?

Answer 16

you said i multiply it by its mass and thats incorrect.

Answer 17

exactly that's right about part D

Answer 18

thank you!

Answer 19

your welcome :)