Question

Which response has *both* answers
correct?

Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added
to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4) = 1.1 × 10–12] What is the
concentration of the silver ion *remaining* in solution?

A) Yes, [Ag+] = 2.9 × 10–6 M. D) No, [Ag+] = 0.060 M.

B) Yes, [Ag+] = 0.060 M. E) No, [Ag+] = 0.105 M.

C) Yes, [Ag+] = 1.3 × 10–4 M.

Part 1:

Ksp = [Ag+]^2[CRO4]

Q = [0.06 M]^2[0.165 M]

Q = 5.9 x 10^-4

Q > Ksp

Yes, a precipitate will form.

Part 2:

[Ag2CRO4] = 2[Ag+][CRO4]

-s +2s +s

1.1 x 10^-12 = 4s^3

s = 6.5 x 10^-5

Ag+ ion concentration = 1.3 x 10^-4

That is as far as I get. I just can't seem to grasp how to get the remaining ion concentration. Any help would be appreciated. Thanks.

Lastly. the ANSWER is A. I just don't know how they got it. Thanks.

Answer #1

Solution :-

**Q> ksp means precipitate will form**

After mixing the solutions the volume will be 250 ml +250 ml = 500 ml

Therefore the concentrations of the both compound will be halved

Therefore new concentrations are as follows

Na2CrO4 = 0.33 M /2 = 0.165 M

AgNO3 = 0.12 M / 2 = 0.06 M

Now lets calculate the concentration of the Ag+ remain after the precipitation

Ksp = [2Ag^+]^2 [ CrO4^2-]

1.1*10^-12 = [2x]^2 * [0.165]

1.1*10^-12 / 0.165 = 4x^2

6.66*10^-12 = 4x^2

6.66*10^-12/ 4 = x^2

1.66*10^-12 = x^2

Taking square root of both sides we get

1.29*10^-6 = x

**Therefore the concentration of the Ag^+ = 1.29*10^-6
M**

Will a precipitate form when 250.0 mL of 0.330 M Na2CrO4 is
added to 250.0 mL of 0.12 M AgNO3? KSP for silver chromate is 1.1 x
10-12.
Please show your work instead of just yes or no, thank you!

Will a precipitate form if 100.0 mL of 2.5 x 10-3 M
Cd(NO3)2 and 75.0 mL of 0.0500 M NaOH are
mixed at 25o C? (Yes or No) Calculate the concentration
of cadmiun ion in solution at equilibrium after the two solutions
are mixed. (Ksp is 7.2 x 10-15 for
Cd(OH)2 at 25o C) Please show all work.

You have been given a 100 mL volumetric aliquot (exact volume)
of a sample containing an unknown concentration of
CrO42-. You perform gravimetric
analysis of a 25 mL aliquot of the original 100 mL sample by
precipitation with sufficient Ag+ (forming
Ag2CrO4). The mass of the empty crucible is
26.252 g. The mass of the crucible containing the precipitate is
26.458 g.
(a) Determine the mass of precipitate
formed.
(b) Report the concentration of the
CrO42- in the original sample...

Silver chloride has Ksp = 1.6 x 10-10 and silver chromate has
Ksp = 9.0 x 10-12. We have 1.00 liter of a
solution which contains both NaCl (0.10 M) and Na2CrO4 (0.10 M).
Solid AgNO3 is added slowly and the solution is stirred well.
a) Which salt precipitates first, AgCl or Ag2CrO4? (Show
your work!)
b) What are the concentrations of [Ag+], [Cl-], and [CrO42-] at
the point when the second salt just begins to
precipitate?
c) Is this...

a) A 0.1500 M of AgNO3 solution was employed to titrate a 25.00
mL of 0.1250 M of NaI and 0.2500 M NaCl. Given that Ksp, AgI(s) =
8.3*10-17, and Ksp, AgCl(s) = 1.8*10-10, please calculate the
concentration of Ag+ ion after 6.00 mL of AgNO3 was added.
Answer: 1.2 x 10-15 M
b) please calculate the pAg after 100.00 mL of AgNO3 was
added
Answer: 1.35
I just want to see how they got that.

Is a precipitate expected to form when 25.0 mL of 0.020 M Copper
(ll) nitrate is added to 50.0 mL of 0.00010 M sodium hydroxide? The
solubility product constant for barium sulfate is 1.1 x 10^-10

Which of the following precipitate form a solution that has the
concentrations indicated? (Show work for each one) a) KClO4: [K+]=
0.01M, [ClO4-]= 0.01 M b) K2PtCl6: [K+]= 0.01 M, [PtCl6^2-]= 0.01
c) PbI2: [Pb2+]= 0.003 M, [I-]= 1.3*10^-3 d) Ag2S: [Ag+]= 1*10^-10
M, [S^2-]= 1*10^-13 M

Can you please check my answers and tell me if they are
correct? thanks
8. Write the ionic equation for dissolution and the solubility
product (Ksp) expression for each of the following slightly soluble
ionic compounds:
(a) PbCl2
PbCl2(s) --> Pb2+(aq) +
2Cl-(aq)
Ksp
= [Pb2+][Cl-]2
(b) Ag2S
Ag2S(s) --> 2Ag+(aq)
+
S2-(aq) Ksp
=[Ag+]2[S2-]
(c) Sr3(PO4)2 Sr3(PO4)2(s)
--> 3Sr2+(aq) +
2PO43-(aq) Ksp
=[Sr2+]3[PO43-]2
(d) SrSO4 SrSO4(s)
--> Sr2+(aq) +
SO42-(aq) Ksp
=[Sr2+][SO42-]
14. Assuming that no equilibria other than dissolution are
involved,...

1. Strong base is dissolved in 565 mL of 0.400 M weak acid (Ka =
3.85 × 10-5) to make a buffer with a pH of 4.07. Assume that the
volume remains constant when the base is added.
a. Calculate the pKa value of the scid and determine the number
of moles of acid initially present.
b. When the reaction is complete, what is the concentration
ratio of conjugate base to acid?
c. How many moles of strong base were...

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