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- HF(g) + H,O(1) H,0*(aq)+ F"(aq) K = 1.1 x 10-3 F (aq) + HF(g) HF;(ag) K= 2.6 x 10- a. Is fluoride in pH 7.00 drinking water more likely to be present as F"(aq) or HF2 (aq)? O HF2 (aq) O F(aq) b. What is the equilibrium constant for this equilibrium? Number 2 HF(g) + H,0(1) H,0*(aq) + HF, (aq) c. What are the pH and equilibrium concentration of HF2" in a 0.150 M solution of HF? (HF, - Number Number pH = M Check Answer View SolutionHow long would it take (in minutes) to reduce 1 mole of each of the following ions using the current indicated? (Ampere (A) = Coulomb/second (C/s), I = C/s, F= 96500 C/mol e-) (C = Charge unit Coulomb, n = electron mole number) Q=I×t=n×F(a) Fe3+ , 2.344 A (b) Cu2+ , 25.260 A(c) 0.02 M CH3COOH solution has a resistance of 240 ohm with a cell constant of 0.366 cm'. Calculate the degree of dissociation and dissociation of CH3COOH at 0.02 M concentration. Given A° HCI, NaCl, CH3COONA are 435, 138 and 99 scm2 mol respectively.
- The autoionization of water at 25°C can be expressed as H,0(l) → H*(aq) + ОН (ад); Кw %3D 10-14 13. Using appropriate calculations, (a) Determine if this reaction is exothermic or endothermic. (b) Show whether this reaction will occur spontaneously. (c) Using the thermodynamics of the reaction, explain how Kw will change at temperatures (1) greater than 25°C and (2) less than 25°C. Species дн? (кJ/mol) AS: (J/K-mol) AG: (kJ/mol) H2O(g) H*(aq) оН ад) -241.8 188.71 -228.6 0.00 0.00 0.00 -230.0 -10.75 -157.2 H2O(1) -237.18 -285.8 69.91 O(aq) 249.17 160.95 231.75(c) 0.02 M CH3COOH solution has a resistance of 240 ohm with a cell constant of 0.366 cm!. Calculate the degree of dissociation and dissociation of CH3COOH at 0.02 M concentration. Given Aº HCI, NaCl, CH3COONA are 435, 138 and 99 scm? mol" respectively.How long would it take to titrate 1.00 mmol H2S with a current of 100.0 mA?
- At 298 K, if the bond dissociation of Clao) to Clo) is +57 kJ/mol while the electron affinity of Clg) to form Cro) is-349 kJ/mol, then the Gibbs energy of the reaction, Clao) + 2e – 2 Clg), is negative. Select one: O True O False(a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a current of 81.2 A for a period of 59.2 min? The unbalanced chemical reaction representing this electrolysis is shown below.NaCl(aq) + H2O(l) Cl2(g) + H2(g) + NaOH(aq) liters of Cl2(g) is generated by this electrolysis.(b) How many moles of NaOH(aq) are formed in the solution in this process? moles of NaOH(aq) are formed.R = 8.314 mol·K F = 96,485 mot AG = AG° + RT · In(Q) ΔΕΔΕ-).In(O) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (1) 1.229 2 z" (aq) Z2 (s) + 2 e 3+ (aq) + 3 е 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e H2 (g) + 2 OH (aq) - 0.828 G (s) - 1.245 > M2+ (aq) + 2 e - 1.893 → M (s) A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate AG° in kJ/mol for this galvanic cell. Report your answer with 4 significant figures. You do not need to report units with your answer. If your value is negative, make sure to include a "-" symbol.
- 3.81944444 Be sure to answer all parts. The AG° for the reaction H;2) + I;(2) = 2HI(g) is 2.60 k.J'mol at 25°C. In one experiment, the initial pressures are PH, = 3.96 atm P, = 0.020 atm PHI = 0.55 atm Calculate AG for the reaction and predict the direction of the net reaction. kJimol The net reaction proceeds from left to right The reaction proceeds from right to leftThe conductivity of a 0.0312 M solution of a weak base is 1.53 x 104 Scm'. If the sum of the limiting ionic conductances for BH* and OH-' is 237.0 Scm²mol·' what is the value of the base constant K6? 4.5 x 10s mol.dm (i) 2.3 x 103 mol.dm (iii) 2.89 x 10 mol.dm3 (ii) 1.37 x 10-5 mol.dm3 (iv) (v) 4.78 x 103 mol.dm3Consider the reaction at 25 degrees celsius 2NO3-(aq)+8H+(aq)+3Cu(s)=3Cu2+(aq)+2NO(g)+4H2O(l) At what pH is the reaction at equilibrium with all other ionic species at 0.01M and gases at 1 atm?