. Describe how to prepare exactly 355 mL of a 0.530 M aqueous solution of cobalt

Question

. Describe how to prepare exactly 355 mL of a 0.530 M aqueous solution of cobalt(III) perchlorate using only a 1.240 M aqueous cobalt(lII) perchlorate solution and water, and give the concentrations of the cobalt(lI) ions and the perchlorate ions present in the 0.530 M aqueous cobalt(I) perchlorate solution. (12 points) 5. When aqueous iron Il nitrate is mixed with aqueous sodium carbonate, the following reaction occurs: 2 Fe(NO,)s(a) 3 Na,CO,(aa)Fe CO)(s) +6 NaNO,(ae). If this reaction produces the maximum amount of both products, what volume of 0.330 M 0.420 M Fe(NO,), and how many moles of Fe (CO), shouler be produced? (12 points) should be mixed with 45.0 mL of Glsing the strong dectrolyte considerations and the solubility guidelines, predict the products (assuming

Explanation / Answer

Q4.

V = 355 mL, M = 0.53 M from:

M = 1.24 M

We need to apply dilution law, which is based on the mass conservation principle

initial mass = final mass

this apply for moles as weel ( if there is no reaction, which is the case )

mol of A initially = mol of A finally

or, for this case

moles of A in stock = moles of A in diluted solution

Recall that

mol of A = Molarity of A * Volume of A

then

moles of A in stock = moles of A in diluted solution

Molarity of A in stock * Volume of A in stock = Molarity of A in diluted solution* Volume of A in diluted solution

Now, substitute known data

MstockVstock = M2V2

1.24*Vstock = 355*0.53

Vstock =  355*0.53/1.24 = 151.73 mL

we need to add 151.73 mL of stock solution....

in the final solution

[Co+3] = 0.53 M

[ClO4-] = 3*[Co(ClO4)3] = 3*0.53 = 1.59 M

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