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yan [13]
4 years ago
7

A solution containing sodium fluoride is mixed with one containing calcium nitrate to form a solution that is 0.015M in NaF and

0.010M I. Ca(NO3)2. Calculate the reaction quotient (Q) for the possible cross product CaF2, and compare Q to the solubility product constant of CaF2 to determine if a percipitate will form.
Chemistry
1 answer:
julsineya [31]4 years ago
5 0
According to the reaction equation:

CaF2(s) ⇄  Ca2+(aq)  +  2F-(aq)

So the Q expression will be = [Ca2+][F-]^2 

and we will neglect the [ CaF2] as it is solid 

so, by substitution:

when we have [Ca2+] = 0.01

and [F-] = 0.015

Q = 0.01 * (0.015)^2

   = 6.3 x 10^-2

by comparing Q value which is 6.3 x 10^-2 and Ksp value which is 1.8 x 10^-5

So, we can see that Q > Ksp 

-that means precipitation will form as ion concentration are greater than

equilibrium concentration So, the reaction will proceed in reverse to achieve 

equilibrium . and the solution will be then supersaturated. 
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2 years ago
How many grams of HCL are needed to make 500.0 mL of a 0.100 M solution?
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Answer:

1.44 g

Explanation:

The problem gives you the molarity and volume of the target solution, so right from the start you know that you can use that information to determine the number of moles of hydrochloric acid that it must contain.

So, molarity measures a solution's concentration in terms of how many moles of solute, which in your case is hydrochloric acid, you get per liter of solution.

A

0.158 M

hydrochloric acid solution contains

0.158

moles of hydrochloric acid for very liter of solution. Since you're dealing with

250 mL

, the equivalent of

1

4

th

of a liter, your solution will contain

250

mL

⋅

1

L

10

3

mL

⋅

0.158 moles HCl

1

L

=

0.0395 moles HCl

Now that you know how many moles of hydrochloric acid are needed to prepare your solution, use the compound's molar mass to convert this to grams

0.0395

moles HCl

⋅

36.46 g

1

mole HCl

=

∣

∣

∣

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

a

a

1.44 g

a

a

∣

∣

−−−−−−−−−−

Explanation:

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