B3☀?Time Remaining: 01:45:23You mix 21 mL of 0.080 M hydrogen cyanide (HCN), K₂ = 4.0x10-10, with 8.4 mL of 0.20 M NaOH to react. What is the equilibrium pH of the solutionthat results after the reaction is complete?A. 1.10B. 3.84EscC. 5.32OD. 5.25Reset SelectionNextE. None of the aboveLast autosaved at 10:12:30 AM71°FMostly sunnyTE4F1Save@A+#3F4$4сF5%5QLF66OF711O&7FB88F9DEF10(9*-F11)O*+F12P45Ins+(363110:16 AM11/3/2022Delete

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Time Remaining: 01:45:23 You mix 21 mL of 0.080 M hydrogen cyanide (HCN), Ka = 4.0x10-10, with 8.4 mL of 0.20 M NaOH to react. What is the equilibrium pH of the solution that results after the reaction is complete? A. 1.10 B. 3.84 C. 5.32 OD. 5.25 OE. None of the above Reset Selection

Time Remaining: 01:45:23 You mix 21 mL of 0.080 M hydrogen cyanide (HCN), Ka = 4.0x10-10, with 8.4 mL of 0.20 M NaOH to react. What is the equilibrium pH of the solution that results after the reaction is complete? A. 1.10 B. 3.84 C. 5.32 OD. 5.25 OE. None of the above Reset Selection

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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MISSED THIS? Read Section 16.6 (Page); Watch IWE 16.5. Consider the following reaction: SO₂ Cl2 (g) SO2 (g) + Cl2 (g) A reaction mixture is made containing an initial [SO₂ C1₂] of 2.0×10-² M . At equilibrium, [Cl₂] = 1.1×10-² M. Part A Calculate the value of the equilibrium constant (Kc). Express your answer to two significant figures. for Part A for Part A do for Part redo fol Part A reset for Part. Ke= 2.2410-² Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
You are an industrial chemist working for a company that makes methanol (CH3OH) according to the equilibrium reaction shown below. You love your job, except that your assistant does not have the best notebook keeping skills. One day you set up the reaction with the equilibrium concentrations shown below. CO (g) + 2 H2 (g) <--> CH3OH (g) 0.24 M 1.1 M 0.15 M at 327oC Later on your assistant mentions that he added some more CO, but he doesn't remember how much. But he also remembers that as the equilibrium was being reestablished, the hydrogen concentration changed by 0.3 M, although he doesn't remember if it went up by that much, or down by that much. How much carbon monoxide did he add, in M?
The initial concentrations of four species involved in an equilibrium are: [Cl2] = 1.40 M, [HCl] = 0.100 M, [O2] = 0.300 M and [H2O] = 0.500 M. Is the reaction at equilibrium? If not, in what direction must the reaction shift for the equilibrium to be reached? Set up Kc in terms of the initial amounts and x as done in class. Do not try to solve for x. Set it up so x is positive. 4 HCl(g) + O2(g) <====> 2 Cl2(g) + 2 H2O(g) Kc = 52 At equil? ______ Direction? _______ Expression ____________
8 Chem101 14.4 Hydrolysis of Salt X Microsoft PowerPoint X |M Inbox (569) - mirandae X M Lab 3/1-elaine.mirand X Sy -log (10)(2.54*10^(-3)) x Question 25 of 66 Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 200 mL reaction vessel contained a mixture of 0.55 atm NO,, 6.5 x 10-5 atm NO, and 4.5 x 10-5 atm O, at 103.0 °C. What are the values of Kp and Kc for the reaction at this temperature? 2 NO:(g) = 2 N0(g) + O2(g) 2 NEXT Based on the given data, set up the expression for Kp. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Kc. %3D 5 RESET (0.55) (6.5 x 10-5) (4.5 x 10-) (2.75) (3.3 x 10-4) (2.3 x 10-4) (2.75 x 10-9) (3.25 x 10-7) (2.25 x 10-7) 2(0.55) 2(6.5 x 10-5) 2(4.5 x 10-5) (0.55)? (6.5 x 10-5)2 5.3 x 10-9 gp א a-0E) 1.9 x 108 1.6 x 1012 6.3 x 10-13 * 23 2$ 7. 6 5. 9. 3. in
34. At 25 C, only 1.9 g CaSO4 will dissolve in 2.00 L of water. What is the equilibrium constant for the reaction below? a. b. C. d. e. CaSO4(s) Ca²+(aq) + SO4²-(aq) 4.9 x 10-5 1.9 x 104 1.4 x 10-² 7.0 x 10-3 0.90 Letter answer to question #34:
None
Experiment 3, Part 1: Write the equilibrium equation established in a saturated potassium chloride, KCl, solution. equilibrium reaction:
Determine the pH of a solution of HCIO2 by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 A 0.020 M aqueous solution of HCIO2 is prepared. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) -2x 1.2 x 10-² - 2x 0 0.020 + x 1 HCIO₂(aq) 0.020 0.020 - x + 2 H₂O(l) 1.2 x 10-² 0.020 + 2x 0.010 0.020 - 2x H3O+ (aq) +X 1.2 x 10-² + x -X + NEXT 1.2 x 10-² - x CIO₂ (aq) RESET +2x 1.2 x 10-² + 2x >