Nickel ion (Ni²+) and hydroxide (OH) are in equilibrium with solid Ni(OH)2 in a 1-Liter solution that was formed by adding pure Ni(OH)2 in water. Solid present: Ni(OH)2 (s) → Ni+2 + 2 OH-¹ Ksp= 5.5 x 10-16 a. What is the equilibrium concentration of Ni+2 ions (in M and mg/L)? b. What is the pH of the solution for part a? C. If the pH is adjusted to pH = 7 by adding a negligible amount of HC1 (i.e., there no change in volume), calculate the new equilibrium concentration of Nit2 (in M and mg/L).

Nickel ion (Ni²+) and hydroxide (OH) are in equilibrium with solid Ni(OH)2 in a 1-Liter solution that was formed by adding pure Ni(OH)2 in water. Solid present: Ni(OH)2 (s) → Ni+2 + 2 OH-¹ Ksp= 5.5 x 10-16 a. What is the equilibrium concentration of Ni+2 ions (in M and mg/L)? b. What is the pH of the solution for part a? C. If the pH is adjusted to pH = 7 by adding a negligible amount of HC1 (i.e., there no change in volume), calculate the new equilibrium concentration of Nit2 (in M and mg/L).

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...

See similar textbooks

Similar questions

At a certain temperature, the equilibrium constant for the reaction CO2lg) + H2(g) is K. = 2.23. If 2.00 mol of CO, and 2.00 mol of H2 are placed in a 2.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide? COg) + H20(g) %3D 0.810 M 0.599 M 0.511M 0.751M 0.631 M
5. Consider the following chemical reaction: CO(g) + 2 H2(g) = CH3OH(g) CO and H2 are added to a fiask with initial concentrations of COI = 0.200 M and [H2] = 0.400 M. After reaching equilibrium, [CH3OH] = 0.1092 M. What is the value of the equilibrium constant, Kc? aniog
1. Write the equilibrium expression and identify the specific equilibrium constant symbol possible, otherwise use K. a. 2 H2O(1) = H¿O' (aq) + OH´(aq) b. HCN (aq) + H,O (1) = H;O* (aq) + CN' (aq) c. 5 C,0,? (aq) + 2 MnO, (aq) + 16 H* (aq) = 10 CO, (g) + 2 Mn²* (aq) + 8 H¿O (1)
esuon To For the following hypothetical equilibrium, A+2 B C, what is the value of the equilibrium constant If the concentrations at equilibrium are [A] = 4.5 x 10 M, [B] = 2.1 x 102 M, and [C] = -3 9.4 x 10 M? Oa. 4.3 x 105 Ob.9.9 x 103 Oc. 9.9 105 אOdan Oe. 0.22 d. 4.7 x MacBook Air F12 F10 F11 000 000 F7 F8 F9 F5 F6 అం F3 F4 FI F2 & %23 $ dele 7 9. 1 4 Q W Y A D F J K C V B N * 00 #3
MISSED THIS? Read Section 16.8 (Pages 701 - 710); Watch KCV 16.8, IWE 16.9. Consider the following reaction and associated equilibrium constant: aA (g) + bB (g) = cC (g) Kc = 3.0 Part A Find the equilibrium concentrations of A, B, and C for a = 1, b = 1, and c = 2. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction. Express your answer using two significant figures. Enter your answers separated by commas. [A], [B]. [C] = Submit Part B X Incorrect; Try Again; 3 attempts remaining IV—| ΑΣΦ 5 Previous Answers Request Answer [A], [B], [C] = Submit Find the equilibrium concentrations of A, B, and C for a = 1, b = 1, and c = 1. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction. Express your answer using two significant figures. Enter your answers separated by commas. OF IVE ΑΣΦ Request Answer ? www M ? M
Write an expression for the equilibrium constant for each reaction. a. 2 NO(g) + O2(g) 2 2 NO2(g) b. CHĄ(g) + 2 Br,(g) CH,Br,(g) + 2 HBr(g)
Consider the reaction. A(aq) = 3 B(aq) K. = 8.37 x 10-6 at 500 K If a 4.30 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] = M * TOOLS x10
7
9. Consider the reaction: 2 A (g) + 3 B (g) = 2 C (g) + 4 E (g). The reaction is initiated with 0.60 M in A, 0.45 M in B and 0.50 M in E (Note 0 M in C). At equilibrium, the value of [B] = 0.15 M. What is the equilibrium value of [E]? a) 0.95 M b) 0.90 M c) 0.80 M d) 0.60 M e) 0.50 M f) 0.40 M g) none of the above 0 4 15 Determine the acid ionization constant
When 1.0 moles each of CO and Br2 were placed into a 1L container and allowed to reach equilibrium, the resulting mixture contained .60 Moles of CO. How many moles of Br2 and C2O2Br2 are present at equilibrium? 2CO + Br2 <---> C2O2Br2
7. Find the equilibrium concentrations for HA, H*, and A for the following reaction: K= 2.0 x 10-5 НА (ад) — А (аq) + H*(аq) НА (ад) ғ А (aд) + H* (ag) I 0.60 0.00 M 0.00 M E
Picture 1 is A) And Picture 2 is B)