To 200.0 ml of a solution of Al(NO3)3 with concentration (2.000x10^-3) mol L-1,(3.0x10^2) ml of (1.00x10^-1) mol L-1 NaF is added. Determine the concentration offree aluminum ions after equilibrium has been established.(K+(AIF63-) = 7.0 x 1019)Note: Your answer is assumed to be reduced to the highest power possible.Your Answer:x10Answerunits

Step 1: Initial Concentrations and VolumesInitial concentration of Al(NO3)3 (Alinit)=…

Answered: To 200.0 ml of a solution of Al(NO3)3…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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To 200.0 ml of a solution of Al(NO3)3 with concentration (1.000x10^-3) mol L-1, (3.0x10^2) ml of (2.000x10^-1) mol L-1 NaF is added. Determine the concentration of free aluminum ions after equilibrium has been established.(K(AIF63-) = 7.0 x 1019) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:
4. If 283.0 mg of AgBr is completely dissolved in 143.0 mL of 0.2 M NH3, what is the equilibrium concentration of Ag* (aq) in the final solution? K[Ag(NH3)2] = 1.7E7 Include at least 3 significant figures in your answer. M Grade This Exercise 5. The acid ionization constant of Fe(H₂O)2+ (aq) is 3E-6. Compute the pH of a 0.11 M aqueous solution of Fe(NO3)2- Include at least 3 significant figures in your answer. D Grade This Exercise 6. Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.71. The solubility product of magnesium hydroxide is 1.2E-11 Include at least 3 significant figures in your answer. D M
Calculate the [Ag+] in a solution prepared by dissolving 1.00 g of AgNO3 and 10.0g KCN in enough water to make 1.00 L of solution. Kf[Ag(CN)2]1- = 1.0 x 1021
From the following choose the most appropriate weak base (when added to its conjugate acid) for making a buffer with pH = 4.50 O (CH3)3N (K, = 6.4 x 105) %3D O CgH5NH2 (K = 3.9 x 1010) O C2H5NH2 (Kg = 5.6 x 104) O HONH2 (K, = 1.1x 108) %3D O NH3 (K5 - 1.8 x 10 5)
Determine the pH of a 0.0525M Fe(NO3)3 solution. Ka of Fe3+ = 6.3x10-3
If 0.45 mol NaCN is added to 1.0 L 0.025 M FeSO4, what will the [Fe2+] be at equilibrium? Kf for Fe(CN)64- = 2.5x1035 ANS: 1.4*10^-34
Calculate the concentration (molarity) of Pb2+ ions in a solution made by adding 0.010 moles of Pb(NO3)2 to 1.0 L of a 2.0 M NaI solution. (Kf = 3.0 x 104 for PbI42−) - 4.9 x 10−2 -3.3 x 10−5 - 2.1 x 10−7 -1.7 x 10−7 -2.3 x 10−8
In distilled water @ 35 degrees C, transition metal hydroxides undergo the following equilibrium M(OH)2 (s)<---> M2+ + 2OH-. If M=Fe, Kc=5.3X10-16. In an equlibrium solution at 35 degrees C what is the pH?
You dissolve 0.194 g of NaOH in 2.00 L of a buffer solution that has [H2PO4] = |HPO, | = 0.188 M. What is the pH of the solution before adding NaOH? (K, for dihydrogen phosphate ion is 6.2 x 10-8.) pH = What is the pH of the solution after adding NaOH? pH =
Based on the line diagram below, which species is the electron donor? Pt(s)|Ni(s)|Niz+ (0.010 M)||Ag+ (0.0250 M)|Ag(s) а. Ag (s) b. Ag+ с. Pt (s) d. Ni (s) е. Niz+
The reaction Cu(s) + HNO3(ag) Cu(NOsh(ag) + 2 NO:) +2 H;O() is used to dissolve the copper metal Ifa 1.000 g sample of copper is used, and instructions say to use four times as much acid as the required amount, how many mL (to the nearest mL) of 15.0 M nitric acid would be used in the procedure for this sample? Select one: O a 10mL Ob 17ml O c.4mL O d 25ml O e 5mL
What is the solubility product expression for Al(OH)3? Ksp = [A1³+][3OH-] Ksp = [A1³+][OH-]³ O Ksp = [A1³+][3OH-]³ O Ksp = [A1³+][OH-] O Ksp = 3[A1³+][OH-]³

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