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Q: What is ∆G0 for the reaction CN- + H2O = HCN + OH-? Ka for HCN = 4.0x10-10. R = 8.314 J/(mol*K)
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A: The enthalpy of the given chemical reaction is calculated by the formula shown below:
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Q: Consider the hypothetical cations, A* and C* and anions, B¯ and D'. Calculate the AG when 20.0 mL of…
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Q: The titration of a 15.0 mL sample of an H2SO4 solution of unknown concentration requires 21.37 ml of…
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Q: Determine the AG (in kl/mol) for a reaction at 267.69 K, for which K, = 1.21x1010, Report your…
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Q: What is the solubility product constant, Ksp? [Ag+] = 2.30 x 10-4 M [CO3-] = 1.15 x 10-4 M Ksp = [ ?…
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Q: Calculate ΔΔG° for the reaction below at 25.0°C CS2(g) + 3Cl2(g) → S2Cl2(g) + CCl4(g)…
A: Applying formula ∆G = ∆H - T∆S
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A: K3 expression depend K1 and K2 of reaction.
Q: Given these reactions, X(6) + 0,@) – xO(6) AH = -653.9 kJ/mol XCo,(6) – XO(s) + CO,(g) AH = +444.5…
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Q: Calculate AH for the following reaction, given the data in the table below: H2SO4(1) → SO3(g) +…
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Q: 4. Given the following reaction, calculate AH°, AS°, and AG°. (25°C) 2P (s) 10 HF (g) → 2 PFs(g) 5…
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Q: T= 549 K
A: ∆G° = - 2.303 R T log K Where ∆G° = -15.9 KJ/mol R = 8.314 J/mol K = 8.314 x 10-3 KJ/mol K T…
Q: Given that: AH°f [Ba(OH)2 (s)] =- 944.7 kJ/mol AH°F [Ba+2 (aq)] = - 537.6 kJ/mol AH°F [OH° (aq)] - -…
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Q: What is the equilibrium constant for the following reaction equal to? H+(aq) + OH−(aq) ⇌ H2O(l)…
A: The equilibrium reaction given is, => H+(aq) + OH−(aq) ⇌ H2O(l)
Q: Calculate T (in K) given ΔG^0= -19.4 kJ/mol and ΔH^0= 69.9 kJ/mol and ΔS^0= 253 J/mol K…
A: ∆G° = -19.4 KJ/mol ∆H° = 69.9 KJ/mol ∆S° = 253 J/mol K T = ?
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Q: Calculate AH for the following reaction, given the data in the table below: H2SO4() → SO3(g) +…
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Q: If AG°rxn is 10.9 kJ/mol, determine AGrxn at 525 K, when TiCl4(g) = 0.250 atm. TiClą(liq) →TICI4(g)
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Q: What is the value of AG° in kJ/mol for a reaction whose K = 8.28 at 75°C?
A: Gibbs energy ∆G =∆Go + RTlnK Now at equilibrium ∆G=0 So, ∆Go=-RTlnK
Q: 4. Given the following reaction, calculate AH°, AS°, and AG°. (25°C) 2P (s) + 10 HF (g) > 2 PFs(g) +…
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- Carbonic acid (H2CO3) and bicarbonate ion (HC0;) are used as a buffer system to regulate the blood pH. An exhausted marathon runner experienced acidosis as his blood pH become 7.15. What is the ratio of HC0, to H2CO3 in this pH? (Ka of H2CO3 = 4.2 x 10-7)1) The equation below represents the equilibrium process of a saturated solution of Ca(OH)2 If the following changes are made to a saturated solution, what will be the effect on the [Ca2+]? Ca(OH)2 (s) <--> Ca2+(aq) + 2 OH- (aq) ΔH = -16.6 kJ A strong base is added to the solution (Decrease, Increase, No change) More solid Ca(OH)2 is added to the container (Decrease, Increase, No change) The solution is raised to a higher temperature (Decrease, Increase, No change) A strong acid is added to the solution (Decrease, Increase, No change) Ca(NO3)2 (s) is added. Ca(NO3)2 is very soluble (Decrease, Increase, No change)B: At 25°C, what is the hydronium ion concentration in the following with discussing your result:- 1) 0.350 M chloroacetic acid? Given, K,=1.36x10, Kw=1×1014 2) 0.420 M sodium chloroacetate? Given, K= 1.36x10, K= Ku/K.
- . (a) Calculate the pH of the following solution: 2.8 x 10-4 M Ba(OH)2 (b) What is the original molarity of a solution of HF whose pH is 1.7 at equilibrium? (Ka = 6.6 x 10-4) HF (aq) ⇌ H+ (aq) + F- (aq)Methanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 3) A 35.0 mL sample of (monoprotic) lactic acid, C3H6O3, is titrated with 20.0 mL of a 4.0 x 10-4 mol/L sodium hydroxide solution. What is the pH of the resulting solution at the equivalence point, if Ka for lactic acid is 1.4 x 10-4? PLEASE HELP THIS IS VERY URGENTCalculate the pH of a 3.11 M solution of KA given that for the acid: HA Ka = 4.21⋅10−44.21⋅10-4
- Given that Ka's for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 x 10-4 and 5.4 x 10-10, respectively, calculate the pH of the following solutions: (a) The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3). (b) The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.What is the effect on the concentration of hydrofluoric acid, hydronium ion, and fluoride ion when the following are added to separate solutions of hydrofluoric acid?(a) HCl(b) KF(c) NaCl(d) KOH(e) HFThe equation for the equilibrium is:HF(aq) + H2 O(l) ⇌ H3 O+(aq) + F−(aq)When you cool down water to 10°C, Kw = 2.9 x 10-15, as compared to the value of Kw at 25°C which is 1 x 10-14 (a bigger K at a higher temp). Which statement is true? a) Dissociation of H₂O is endothermic; the pH of neutral water at 10°C is 14.5 b) Dissociation of H₂O is exothermic; the pH of neutral water at 10°C is 14.5 c) Dissociation of H₂O is endothermic; the pH of neutral water at 10°C is 7.27 d) Dissociation of H₂O is exothermic; the pH of neutral water at 10°C is 7.27 e) Dissociation of H₂O is endothermic; the pH of neutral water at 10°C is 7 f) Dissociation of H₂O is exothermic; the pH of neutral water at 10°C is 7
- Question 7 (5 points) Listen The pH of 300 mL solution made of 1.08 M acetic acid and 0.69 M potassium acetate is (K, = 1.8 x 10) after the addition of 0.02 moles HCI Your Answer: Answer7. Suppose two separate solutions are prepared. One solution contains 5.2 grams of the salt, potassium nitrate (KNO3). The other solution contains 5.2 grams of the salt, potassium carbonate (K2CO3). Which salt do you expect to dissolve more readily if 1.0 M HCI (a strong acid) is added to each solution? The Ka of HNO3 is1.4 x10-1, and the Ka of of HCO3-1 is 1.7 x10-6. You can assume no other reactions occur.Write dissociation and hyrolysis reaction for each ion produced. Is it acidic, basic or neutral.