Chapter 15 Problem Set KEY

13. What is the molar solubility of Pbl2 in an aqueous solution containing 0.15 M Nal? The Ksp of Pblz is 1.4x10-8. a. 6.2x107 M b. 9.3x10-8 M 4.7x10-8 M d. 1.6x107 M e. 2.5x107 M   Only typedc solution

I need help with this problem

What is the Kf expression for the following complexation reaction? Al* (aq) + 6F (aq) TAIF* (aq) Select one: | AIF| K = Al- || F]° A. | AIF ° | A || F| K = | A13+ ][ F| Kf = | AIF,3- 1 C. | AP || F]° Kf = | AIF-| D. B.

0 Calculate the minimum concentration of Cr³+ required in a 0.095 M (aq) NaF solution in order to initiate a precipitate of chromium (III) fluoride. (For CrF3, Ksp = 6.6 x 10-¹¹) A. 0.023 M B. 0.032 M C. 6.9 × 10-10 M 2.9 x 10¹9 M 7.7 x 108 M D. E.

What is the Kf expression for the following complexation reaction? Al3* (ag) + 6F (aq) [AIFP (aq) Select one: | AIF ° A1 А. | AP* ]| F |* | AIF3- | 6 KĘ = В. | AIF,3- | K = | AI* ]| F]° K = | AIF3- |6 D.

Please don't provide handwritten solution ....

What is the solubility-product expression for La(IO3)3 (s)? a. Ksp = [La3+] [IO3-]1/3 b. Ksp = [La3+] [IO3-] c. Ksp = [La3+]3[IO3-] d. Ksp = [La3+]3[IO3-]3 e. None of the above

A solution is prepared such that the initial concentration of A2+ is 1.50x103 M and the initial concentration of X is 4.60x10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9x10-4 M. A2* (aq) + X (aq) =Ax2+ (aq) %3D Complete the ICE table below by selecting the correct value or expression to place in the ICE table from the drop-down menu. A2+ (aq) X (ад) АХ2+ (aq) Initial concentration Change in concentration Equilibrium concentration expression Equilibrium concentration value

What is the solubility-product expression for La(IO3)3 (s)?     A. Ksp = [La3+] [IO3-]1/3 B. Ksp = [La3+] [IO3-] C. Ksp = [La3+]3 [IO3-] D. Ksp = [La3+]3 [IO3-]

For AgOH, Ksp = 1.5 x 10-8. What is the molar solubility of AgOH in a solution containing 0.1 M of NH3 buffered at pH = 7? (K;[Ag(NH3)2')= 1.6 x 107). A. 0.20 M B. 0.025 M C. 0.25 M D. 0.05 M

According to the equilibrium equation, which ion(s) do you have when solution dissolved?Explain how you know the identity of the ion(s) present.

A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial concentration of X is 4.60×10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9×10-4 M. A2+ (aq) + X (aq) AX2+ (aq) Use your correct answers from #7 to answer this question. What is Kf, the formation constant, for this complex?

A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial concentration of X is 4.60×10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9×10-4 M. A2+ (aq) + X (aq) AX2+ (aq) What is Kf, the formation constant, for this complex?

After completing the experiment, a student finds that the equilibrium concentrations of the reactants and product are as follows. Calculate the equilibrium constant for the complex ion formation. [SCN¯]eg= 6.45x10-4 M [Fe3*]eq = 8.43x10-4 M [FENCS2+]eg = 1.49x10-4 M %3D

I need help answering number 5

Which of the following is the correct Kf expression for the formation of the complex ion tetraiodoplumbate(II) ion, [PbI4]2–?   Pb2+ (aq) + 4 I1- (aq) < === > [PbI4]2– (aq)     Kf = [PbI4]2– / {[Pb2+] [4 I1-]}     Kf = {[Pb2+] 4[I1-]} / [PbI4]2–     Kf = {[Pb2+] [I1-]4} / [PbI4]2–     Kf = [PbI4]2– / {[Pb2+] [I1-]4}

multiple choice

Calculate the Ksp for magnesium fluoride if the solubility of MGF2 in pure water is 0.000234 M. a. 5.1 x 10-11 O b.5.8 x 10-5 C. 9.3 x 10-4 d. 1.3 x 10-11

Write the equilibrium constant for the following reactions: a. 3NO(g) ↔ N2O(g) +  NO2(g) b. Ni(CO)4(g) ↔ Ni(s) + 4CO(g) c. C(s) + 2H2(g) ↔ CH4(g)

Calculate the equilibrium isothiocyanatoiron(III) ion concentration, [FENCS2*leg• you will report when making your standard curve. Give your answer to three decimal places. Also give your answer in millimolar (mM) (because you won't be able to enter an answer in scientific notation here). Fe(NO3)3 0.10 M HNO3 NaSCN 0.194 M 1.97 x 10-3 M initial buret reading (mL) final buret reading (mL) 0.02 0.03 0.01 1.87 0.39 7.57

Choose the best answer below. Consider the following complex ion formation equilibrium and it's equilibrium constant, Kf. Which of the following statements is FALSE? Cu2+ (aq) + 4CN" (aq) Û Cu(CN)42- (aq) Kf = 1.0x1025 O Adding more CN- will cause more complex ion to form The equilibrium lies in favor of the complex ion Cu2+ is a Lewis acid in the reaction, and CN is a Lewis base Removing some of the Cu2* (e.g., by precipitation) will cause some of the complex ion to dissociate The complex ion is a Lewis acid-base adduct O If enough CN- is added, the equilibrium mixture would contain zero Cu2+

Assume we are to tackle a complex equilibria problem using the process we learned in class. In this example, we’re going to look at dissolving CuS in water.  The relevant equilibrium reactions are as follows: CuS   ⇋   Cu2+   +   S2–                                                                                                                                   Cu2+   +   OH–   ⇋   Cu(OH)2 S2–   +   H2O   ⇋   HS–   +   OH–                                                                                                           H2O   ⇋   H+   +   OH– HS–   +   H2O   ⇋   H2S   +   OH– Write 1 charge balance equation.

11:39 PM Mon May 29 Question 14 of 34 What is the charge of the complex formed by a platinum (II) metal ion coordinated to two ammonia molecules and two chloride ions? Tap here or pull up for additional resources

Calculate the molar solubility of Mg 3(PO 4) 2. The Ksp of Mg 3(PO 4) 2 is 2.2 x 10 -19. A. 7.3 x 10-5 M B. 3.0 x10-9 M C. 7 x 10-10 M D. 1.5 x 10-4 M