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?

A student mixes 31.0 mL of 3.24 M Pb(NO3)2(aq) with 20.0 mL of 0.00217 M NaI(aq)....

A student mixes 31.0 mL of 3.24 M Pb(NO3)2(aq) with 20.0 mL of 0.00217 M NaI(aq). How many moles of PbI2(s) precipitate from the resulting solution? What are the values of [Pb2 ], [I–], [NO3–], and [Na ] after the solution has reached equilibrium at 25 °C?

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?

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