Question

In: Chemistry

56.0 mL of 2.50 M Fe(NO3)2 is combined with 25.0 mL of 0.0525 M Na2CO3. Ksp...

56.0 mL of 2.50 M Fe(NO3)2 is combined with 25.0 mL of 0.0525 M Na2CO3.

Ksp of FeCO3 is 2.1 × 10-11.

What mass of FeCO3(s) will be produced? in grams

What is the [Fe2+] in the solution final solution? in M

What is the [CO32-] in the solution final solution? in M

Solutions

Expert Solution

Given that 56 mL of 2.5 M Fe(NO3)2

                = 56 mL x 2.5 mole / 1000 mL

                = 0.14 moles

Given that 25 mL of 0.0525 M Na2CO3

                = 25 mL x 0.0525 mole / 1000 mL

                = 0.0013125 moles

Consider the equation

                                                  Fe(NO3)2         +         Na2CO3       FeCO3      +      2 NaNO3

Initial moles                                   0.14            0.0013125    0         0

after reaction                  (0.14 - 0.0013125)    0              0.0013125    0.002625

                                           = 0.1387

mass of FeCO3 produced = 0.0013125 x molecular mass of FeCO3

                                     = 0.0013125 x 115.85 = 0.152 g

Total volume after reaction = 56 + 25 = 81 mL = 0.081 L

Therefore concentration of Fe(NO3)2 after reaction = 0.1387 mole / 0.081 L

                                                                         = 1.712 M

Therefore concentration of Fe2+ in the resultant solution = 1.712 M

This is due to the excess of Fe(NO3)2

Given that the solubility product of FeCO3 is 2.1 x 10-11

                                      [Fe] [CO3] = 2.1 x 10-11

Consider the equation FeCO3    Fe2+ + CO32-

                                                      [x]                   [ x]

Where [x] is the concentration of Fe2+ CO32- and in the solution

But already we have the concentration of Fe2+ due to the excess of Fe(NO3)2 = 1.712 M

Therefore the total conc of Fe2+ = [Fe2+] = [1.712 + x]

                          and         [CO32-] = [x]

Ksp = 2.1 x 10-11 = [1.712 + x] * [x]

                        = 1.712x        [since x is small compared to 1.712 it is neglected in [1.712 + x]

therefore x = 2.1 x 10-11 / 1.712 = 1.23 x 10-11 M

Thus

The mass of FeCO3 produced = 0.152 g

[Fe2+] in the final solution = 1.712 M

[CO32-] in the final solution = 1.23 x 10-11 M

                                                                         


Related Solutions

25.0 mL of a 1.00 M Fe(No3)2 solution was reacted with 25.0 mL of a 0.700M...
25.0 mL of a 1.00 M Fe(No3)2 solution was reacted with 25.0 mL of a 0.700M solution of K3PO4 to produce the solid Fe3(PO4)2 by the balanced chemical equation 3 Fe(NO3)2(aq)+ 2 K3PO4(aq)--->Fe3(PO4)2(s)+ 6 KNO3(aq) What is the limiting reagent? How many grams of Fe(PO4)2 will be produced?
Someone reacts 25.0 ml of 2.50 M mixture of NaOH with 37.5 ml of 1.00 M...
Someone reacts 25.0 ml of 2.50 M mixture of NaOH with 37.5 ml of 1.00 M mixture of H2SO4. The reaction that occurs is 2 NaOH + H2SO4 -> Na2SO4 + 2 H2O. What is the mass of each product that will be formed?
25.0 mL of a 4.21 M HCl solution at 25.2°C and 50.0 mL of a 2.50...
25.0 mL of a 4.21 M HCl solution at 25.2°C and 50.0 mL of a 2.50 M NaOH solution at 25.2°C are reacted together to give a final temperature of 44.1°C. The specific heat of the solution is 3.88 J/g°C and it weighs 76.6 grams. From this information, determine: a. the limiting reactant for this reaction b. the heat produced by the reaction (q) in units of Joules. c. the enthalpy of the reaction (∆H) in units of kJ/mole.
When 25.0 mL of a 2.72×10-4 M manganese(II) chloride solution is combined with 25.0 mL of...
When 25.0 mL of a 2.72×10-4 M manganese(II) chloride solution is combined with 25.0 mL of a 2.14×10-4 M potassium carbonate solution does a precipitate form? (yes/no) AND For these conditions the Reaction Quotient, Q, is equal to: _____
You titrate 25.00 mL of 0.03040 M Na2CO3 with 0.02790 M Ba(NO3)2. Calculate pBa2 after the...
You titrate 25.00 mL of 0.03040 M Na2CO3 with 0.02790 M Ba(NO3)2. Calculate pBa2 after the following volumes of Ba(NO3)2 are added. Ksp for BaCO3 is 5.0 × 10–9. (a)12.50 ml (b) Veq (c) 34.70 ml
How many grams of CaF2 will be soluble in 100 ml of 0.250 M Ca(NO3)2? (Ksp...
How many grams of CaF2 will be soluble in 100 ml of 0.250 M Ca(NO3)2? (Ksp of CaF2 = 3.90*10^-11)
1) Calculate the amount of 1.50 M Na2CO3 needed to react completely with 25.0 mL of...
1) Calculate the amount of 1.50 M Na2CO3 needed to react completely with 25.0 mL of 0.500 M CaCl2. 2) Calculate the theoretical yield of chalk (calcium carbonate) for each reaction (#1 & #2)—show all calculations. For reaction #1 CaCl2 should be limiting and for reaction #2 Na2CO3 should be limiting. You need to figure out how much sodium carbonate solution you will use in your experiment Na2CO3(aq) + CaCl2(aq) àCaCO3(s) + 2NaCl(aq)  (molecular equation) CO32– (aq)  +  Ca2+(aq)  àCaCO3(s)   (net ionic equation) Limiting reactant(determining...
20.00 mL of 3.00E-3 M Fe(NO3)3 is mixed with 8.00 mL of 2.48E-3 M KSCN and...
20.00 mL of 3.00E-3 M Fe(NO3)3 is mixed with 8.00 mL of 2.48E-3 M KSCN and 12.00 mL of water. The equalibrium molarity of Fe(SCN)2+ is found to be 6.82E-5 M. If the reaction proceeds as shown below, what is the equilibrium molarity of Fe3+ and SCN-?    Fe3+(aq) + 2 SCN-(aq) Fe(SCN)2+(aq) I have the answers (they are correct according to my online homework), but need to know how to get them. Thank you! The correct answeers are: Fe =...
10.00 mL of 3.48E-3 M Fe(NO3)3 is mixed with 4.00 mL of 2.84E-3 M KSCN and...
10.00 mL of 3.48E-3 M Fe(NO3)3 is mixed with 4.00 mL of 2.84E-3 M KSCN and 6.00 mL of water. The equalibrium molarity of FeSCN2+ is found to be 8.70E-5 M. If the reaction proceeds as shown below, what is the equilibrium molarity of Fe3+ and SCN-? Fe3+(aq) + SCN-(aq) FeSCN2+(aq) Equilibrium Concentration Fe3+ ____________ Equilibrium Concentration SCN- ____________
Q2: When 500.0 mL of 2.00 M Ba(NO3)2 solution at 25.0 °C is mixed with 500.0...
Q2: When 500.0 mL of 2.00 M Ba(NO3)2 solution at 25.0 °C is mixed with 500.0 mL of 2.00 M Na2SO4 solution at 22.0°C in a coffee-cup calorimeter, the white solid BaSO4 forms, and the temperature increases to 28.2°C. Assume that the calorimeter is insulated and has negligible heat capacity, the specific heat capacity of the solution is 4.184 J/g°C, and the density of the final solution is 1.0 g/mL. Answer the questions below using the Balanced Equation: Ba(NO3)2 (aq)+...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT