Homework Answers
23) When you add a strong base such as NaOH, it breaks into Na+ and OH- ions. OH- ions react with H3O+ ions to produce water. So, there is a shortage of H3O+ ions. According to Le Chatalier principle, as H3O+ ion is a product in the given equation, so it's shortage will shift the equilibrium towards the products. So, more BH+ and H2O will react to produce H3O+ and B. Again this H3O+ will react with OH- ions and so on. So as you can observe, more B is formed but no B is consumed. So, the cocentration of B will increase.
Option C
24) MgS reacts with water to produce SO2 and Mg(OH)2. All other compounds are soluble in water. So, the correct answer is B.
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23) Consider the following generalized buffer solution equilibrium: BH+(aq) + H2O(1) H3O+(aq) + B(aq) 24) Select...
Now, for a complete equilibrium problem Consider the following general reaction: HC2H3O2 (aq) + H2O (l) ⇌...
Now, for a complete equilibrium problem Consider the following general reaction: HC2H3O2 (aq) + H2O (l) ⇌ H3O+ (aq) + C2H3O2–(aq) Kc = 1.8 x 10–5 (at 25 ºC) If a solution initially contains (7.9x10^-1) M of HC2H3O2, (and no H3O+ or C2H3O2– ), what is the equilibrium concentration of H3O+ (aq) in the mixture? In the appropriate blanks, provide the equilibrium [H3O+ (aq)], in the solution, in M, to two significant figures and to the appropriate power
Consider the following reaction: HC2H3O2(aq)+H2O(l)⇌H3O+(aq)+C2H3O−2(aq) Kc=1.8×10−5 at 25∘C If a solution initially contains 0.180 M HC2H3O2,...
Consider the following reaction: HC2H3O2(aq)+H2O(l)⇌H3O+(aq)+C2H3O−2(aq) Kc=1.8×10−5 at 25∘C If a solution initially contains 0.180 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25∘C? Express your answer using two significant figures.
i want answer to all questions please Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the so...
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2 (aq) + H2O (l)...
Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2 (aq) + H2O (l) <--------------> H3O+ (aq) + NO2- In which direction will the equilibrium shift if a) NaOH is added? b) NaNO2 is added? c) HCl is added? d) The acid solution is made more dilute?
1. Consider the following reaction at equilibrium. CH3COOH (aq) = CH3COO- (aq) + H+ (aq) a)...
1. Consider the following reaction at equilibrium. CH3COOH (aq) = CH3COO- (aq) + H+ (aq) a) When NaOH is added to the solution, write the reaction that occurs. (What does the OH react with?) b) When NaOH is added to the solution, will the concentration of each of the following species increase, decrease, or remain the same? Explain your answer. [H"] [CH,C00] [CH2COOH)
1. Write the equilibrium constant expression for the following reaction: H3PO4(aq) + 3 H2O(l) ↔ PO4...
1. Write the equilibrium constant expression for the following reaction: H3PO4(aq) + 3 H2O(l) ↔ PO4 3- (aq) + 3 H3O+ (aq) 2. (LeChatlier’s principle) The following reaction has Kc = 4.2 x 102 at 325oC, all gases. PBr3 + Cl2 ↔ PCl3 + Br2 ΔHo = -47 kJ/mol a. For this reaction at equilibrium, [PBr3] = [Cl2] = 0.0273 M, and [PCl3] = [Br2] = 0.560 M. What do you expect to happen to the equilibrium concentrations of each...
Equilibrium Consider the following equilibrium: CH 3COOH(aq) + H 20(1) = CH 3COO "(aq) + H...
Equilibrium Consider the following equilibrium: CH 3COOH(aq) + H 20(1) = CH 3COO "(aq) + H 30 +(aq) What would be the effect of adding sodium acetate (CH 3COONa) a strong electrolyte to the reaction and what would happen to the pH of the solution? a. the equilbrium will shift to the right and the pH will decrease O b. the equilibrium will shift to the left and there will be no change in pH O c. the equilbrium will...
G-10 Assume the equilibrium constant K 1 for a reaction A + B 2 C. You...
G-10 Assume the equilibrium constant K 1 for a reaction A + B 2 C. You prepare a solution that has the following initial concentrations. For each solution, calculate the reaction quotient Q and state if the concentrations of reactants and products will (increase, decrease, or stay the same). a) [A] 1 M, [B] 1M, [C] 2 M. b) [A] 2 M, [B] 1 M,(C] 1 M. Answers: Q 4 >K, [A, B] increase, [C] decreases Q=0.5 < K, [A,...
please show all work neatly 5. (2 pts) Consider the following acids and their dissociation constants HPO4-2(aq) + H2O.. H3O"(aq) + PO4-3(aq) Ka-2.2x 10.13 HCOOH(aq) H20 H3O (a) HCOO (aq) Ka =...
please show all work neatly
5. (2 pts) Consider the following acids and their dissociation constants HPO4-2(aq) + H2O.. H3O"(aq) + PO4-3(aq) Ka-2.2x 10.13 HCOOH(aq) H20 H3O (a) HCOO (aq) Ka = 1.8x10-4 a. Which is the weaker acid, HPO42 or HCOOH? b. What is the conjugate base of, HPO42 or c. Which acid has the weaker conjugate base? d. Which acid produces more ions? 6. (2 pts) Write a balanced equation for the neutralization of H3PO4(aq) and NaOH(aq) (3...
Consider the dissolution of AB(s): AB(s)⇌A+(aq)+B−(aq) The generic metal hydroxide M(OH)2 has Ksp...
Consider the dissolution of AB(s): AB(s)⇌A+(aq)+B−(aq) The generic metal hydroxide M(OH)2 has Ksp = 6.85×10−12. (NOTE: In this particular problem, because of the magnitude of the Ksp and the stoichiometry of the compound, the contribution of OH− from water can be ignored. However, this may not always be the case.) 1. Le Châtelier's principle tells us that an increase in either [A+] or [B−] will shift this equilibrium to the left, reducing the solubility of AB. In other words, AB...
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
1. Consider the following reaction at equilibrium. CH3COOH (aq) = CH3COO- (aq) + H+ (aq) a) When NaOH is added to the solution, write the reaction that occurs. (What does the OH react with?) b) When NaOH is added to the solution, will the concentration of each of the following species increase, decrease, or remain the same? Explain your answer. [H"] [CH,C00] [CH2COOH)
Equilibrium Consider the following equilibrium: CH 3COOH(aq) + H 20(1) = CH 3COO "(aq) + H 30 +(aq) What would be the effect of adding sodium acetate (CH 3COONa) a strong electrolyte to the reaction and what would happen to the pH of the solution? a. the equilbrium will shift to the right and the pH will decrease O b. the equilibrium will shift to the left and there will be no change in pH O c. the equilbrium will...
G-10 Assume the equilibrium constant K 1 for a reaction A + B 2 C. You prepare a solution that has the following initial concentrations. For each solution, calculate the reaction quotient Q and state if the concentrations of reactants and products will (increase, decrease, or stay the same). a) [A] 1 M, [B] 1M, [C] 2 M. b) [A] 2 M, [B] 1 M,(C] 1 M. Answers: Q 4 >K, [A, B] increase, [C] decreases Q=0.5 < K, [A,...
please show all work neatly
5. (2 pts) Consider the following acids and their dissociation constants HPO4-2(aq) + H2O.. H3O"(aq) + PO4-3(aq) Ka-2.2x 10.13 HCOOH(aq) H20 H3O (a) HCOO (aq) Ka = 1.8x10-4 a. Which is the weaker acid, HPO42 or HCOOH? b. What is the conjugate base of, HPO42 or c. Which acid has the weaker conjugate base? d. Which acid produces more ions? 6. (2 pts) Write a balanced equation for the neutralization of H3PO4(aq) and NaOH(aq) (3...
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