A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3, 4.00 mL of 2.00 x...

A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3, 4.00 mL of 2.00 x 10-3 M KSCN, and 1.00 mL of distilled water and finds that in the equilibrium mixture, the concentration of FeSCN2+ is 1.31 x 10-4 M. The equation describing the equilibrium is Fe3+ (aq) + SCN- (aq) →← →← FeSCN2+ (aq) Calculate the concentration of FeSCN2+ at equilibrium. Include appropriate significant figures and units in your response. Example input: 1.31x10^-4 M.

Expert Solution

queen_honey_blossom answered 2 years ago

A student mixes 5.00 mL of 2.00 x 10‐3 M Fe(NO3)3 with 5.00 mL 2.00 x...

A student mixes 5.00 mL of 2.00 x 10‐3 M Fe(NO3)3 with 5.00 mL 2.00 x 10‐3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN+2 is 1.40 x 10‐4 M. What is the initial concentration in solution of the Fe+3 and SCN‐? What is the equilibrium constant for the reaction? What happened to the K+ and the NO3‐ ions in this solution?

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- ____________

A sample is prepared by adding 750 mL of 4.00 × 10–3 M Ce(NO3)3 solution to...

A sample is prepared by adding 750 mL of 4.00 × 10–3 M Ce(NO3)3 solution to 300 mL of 2.00 × 10–2 mol L–1 KIO3 solution. Will any Ce(IO3)3 (Ksp = 1.9 × 10–19) precipitate be observed for the final solution? Show all working.

1. Suppose 50.00 mL of 2.0 × 10–4 M Fe(NO3)3 is added to 50.00 mL of...

1. Suppose 50.00 mL of 2.0 × 10–4 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-6 M KIO3. Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0 × 10–14. A) A precipitate forms because Qc > Ksp. B) A precipitate forms because Qc < Ksp. C) No precipitate forms because Qc < Ksp. D) No precipitate forms because Qc = Ksp. E) No precipitate forms because Qc > Ksp. 2. For which of the following...

1. a.) A student mixes 47.0 mL of 3.30 M Pb(NO3)2(aq) with 20.0 mL of 0.00183...

1. a.) A student mixes 47.0 mL of 3.30 M Pb(NO3)2(aq) with 20.0 mL of 0.00183 M Na2C2O4(aq). How many moles of PbC2O4(s) precipitate from the resulting solution? What are the values of [Pb2 ], [C2O42–], [NO3–], and [Na ] after the solution has reached equilibrium at 25 °C? Ksp of PbC2O4 (s) is 8.5e^-9 M^2 b.) What are the values of [Pb^2+], [C2O4^2-], [NO3^-], and [Na^+] after the solution has reached equilibrium?

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 =...

adding 50.0 mL of 1.0 x 10^-3 M Sr(NO3)2 and 50.0 mL of 1.0 x 10^-3...

adding 50.0 mL of 1.0 x 10^-3 M Sr(NO3)2 and 50.0 mL of 1.0 x 10^-3 M Na2CO3wpuld produce how many grams of SrCO3 precipitate? ksp of SrCO3 = 1.1 x 10^-10

A 1.00 L solution contains 2.00 X 10^-4 M Cu(No3)2 and 1.2 x 10^-3 M Ethylenediamine...

A 1.00 L solution contains 2.00 X 10^-4 M Cu(No3)2 and 1.2 x 10^-3 M Ethylenediamine (en). The Kf for Cu(en)2 2+ is 1.0X10^20 What is the concentration of Cu 2+ (aq) in the solution?

If we mix 40.0 mL of 3.00 M Pb(NO3)2 (aq) with 20.0 mL of 2.00 x...

If we mix 40.0 mL of 3.00 M Pb(NO3)2 (aq) with 20.0 mL of 2.00 x 10-3 M NaI (aq), does PbI2 (s) precipitate from solution? I yes, calculate how many moles of PbI2 (s) precipitate and the values of [Pb2+], [I-], [NO3-], and [Na+] at 25 C at equilibrium?

1) A student mixes 150. mL of 0.20 M Na2CO3 with 130. mL of 0.25 M...

1) A student mixes 150. mL of 0.20 M Na2CO3 with 130. mL of 0.25 M CaCl2 to obtain CaCO3 precipitate. Which is the limiting reactant? Select one: a. sodium carbonate b. calcium chloride 2) What mass of CaCO3 should be produced? Report your answer to the proper significant digits and include units. ii) The student was able to obtain 2.3 g of precipitate. Calculate the percent yield for the reaction. Report your answer to the proper significant digits and...

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