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help calculating pH. not sure if answwer is correct
(B)Increases concentration of O2 (C) Equilibrium constant...
Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 200(g) =...
Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 200(g) = CO2(g) + C(s) A. [CO][C]/[CO] B. K [CO] C. [CO] / [CO2) D. [CO]/[CO] E. 2[CO] /[CO][C] In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Châtelier's principle? ООООО A. 2N, () + 0,02N,0 () B. N.O. (g) 2NO, (g) C. N2(g) + 3H2(g)2NH3 (9) D. N2 (9) + 202...
7. The equilibrium constant for the auto-ionization of water HO () (aq)OH (aq) is 1.0x 10 at 25°C and 3.8 x 10 at 4...
7. The equilibrium constant for the auto-ionization of water HO () (aq)OH (aq) is 1.0x 10 at 25°C and 3.8 x 10 at 40C. a. Is the forward process endothermic or exothermic? b. What is the pH of the water at 40 C? c. Based on your calculated pH, is this solution acidic or basic? d. Which of the following statements is consistent with this behavior? i. The autoionization of water is an endothermic reaction i. The autoionization of water...
help please 1-4 consider the reaction A+B 3 C + D. which has an equilibrium constant,...
help please 1-4
consider the reaction A+B 3 C + D. which has an equilibrium constant, K, equal to 3.4 x 10. 1. IT one begins a reaction by placing 0.600 moles of A in a 1.0L container as well as 0.150 moles on , what will be the equilibrium concentrations of A.B.C. and D? Write your answers in the spaces provided below. a. (A) = b. [B]= = C. (C)= d. (D)= 2. Once the reaction in problem 1...
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e)...
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e) HSO (d) F (b) Н:0" 6, Use Table 15.2 (page 529) to decide whether the species on the left or those on the right are favored by the reaction. a. NH4 (aq) + H2PO4" (aq) # NH3(aq) + HsPO b. HCN (aq) + HS(aq) CN" (aq) +H2S c. HCO +OH CO2 H2S d. Al(H20)6 3+ +OH = Al(H20) s2+ OH 7. The equilibrium constant...
A buffer solution is able to maintain a constant pH when small amounts of acid or...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
Please I need help on this. I'm so lost 1. Acetic acid (H)CO2H) has k, =...
Please I need help on this. I'm so lost
1. Acetic acid (H)CO2H) has k, = 1.8 x 10- and acetate (H:C:01") has ks = 5.6 x 10-10. (a) Write balanced chemical equilibrium equations (with physical states) for acid dissociation of acetic acid and base hydrolysis of acetate ion. (b) Write K, and equilibrium constant expressions for the above reactions. (c) Use your expressions from part b to show that Kx. = 1.0 x 10-* = [H,O'][OH). 2. For each...
Please help with solving Question 1 (A-C) Thank you! Unless otherwise specified in the problem, you...
Please help with solving Question 1 (A-C) Thank you!
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. Carbonic acid: Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857...
Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 200(g) = CO2(g) + C(s) A. [CO][C]/[CO] B. K [CO] C. [CO] / [CO2) D. [CO]/[CO] E. 2[CO] /[CO][C] In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Châtelier's principle? ООООО A. 2N, () + 0,02N,0 () B. N.O. (g) 2NO, (g) C. N2(g) + 3H2(g)2NH3 (9) D. N2 (9) + 202...
7. The equilibrium constant for the auto-ionization of water HO () (aq)OH (aq) is 1.0x 10 at 25°C and 3.8 x 10 at 40C. a. Is the forward process endothermic or exothermic? b. What is the pH of the water at 40 C? c. Based on your calculated pH, is this solution acidic or basic? d. Which of the following statements is consistent with this behavior? i. The autoionization of water is an endothermic reaction i. The autoionization of water...
help please 1-4
consider the reaction A+B 3 C + D. which has an equilibrium constant, K, equal to 3.4 x 10. 1. IT one begins a reaction by placing 0.600 moles of A in a 1.0L container as well as 0.150 moles on , what will be the equilibrium concentrations of A.B.C. and D? Write your answers in the spaces provided below. a. (A) = b. [B]= = C. (C)= d. (D)= 2. Once the reaction in problem 1...
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e) HSO (d) F (b) Н:0" 6, Use Table 15.2 (page 529) to decide whether the species on the left or those on the right are favored by the reaction. a. NH4 (aq) + H2PO4" (aq) # NH3(aq) + HsPO b. HCN (aq) + HS(aq) CN" (aq) +H2S c. HCO +OH CO2 H2S d. Al(H20)6 3+ +OH = Al(H20) s2+ OH 7. The equilibrium constant...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
Please I need help on this. I'm so lost
1. Acetic acid (H)CO2H) has k, = 1.8 x 10- and acetate (H:C:01") has ks = 5.6 x 10-10. (a) Write balanced chemical equilibrium equations (with physical states) for acid dissociation of acetic acid and base hydrolysis of acetate ion. (b) Write K, and equilibrium constant expressions for the above reactions. (c) Use your expressions from part b to show that Kx. = 1.0 x 10-* = [H,O'][OH). 2. For each...
Please help with solving Question 1 (A-C) Thank you!
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. Carbonic acid: Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857...
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