Calculate the pH of the following system if [Cd2+] = 0.2 M and PH, = 0.5 atm. Thestandard emf is -0.403 V and the measured emf is -0.332 V.Cd2*(aq) + H2(g) --> 2H*(aq) + Cd(s)

Nernst equation- Ecell = E0cell - 2.303 RTnF log Qwere,Ecell = emf of cellE0cell = standard emf of cellR = gas constant ( 8.314 J /K)T = temperature KF = 96500 Cn = number of electrons Q = reaction quotient At 298 K, Ecell = E0cell - 0.0592n log Q were,Ecell = emf of cellE0cell = standard emf of cellR = gas constant ( 8.314 J /K)T = temperature KF = 96500 Cn = number of electrons Q = reaction quotient pH = -log [H+]Reaction - Cd 2+ (aq) + H2 (g) → 2H+ + Cd (s) n = 2 Ecell = E0cell - 0.0592n log [H+]2[Cd2+] PH2-0.332 =- 0.403 - 0.05922 log [H+]20.2 x 0.5 0.071 =-0.05922 log [H+]20.2 x 0.5 - 2.3986 = log [H+]20.2 x 0.5 3.9940 x 10-3 = [H+]20.1 3.9940 x 10-4 = [H+]20.020= [H+] pH = -log [H+] pH = -log 0.020 pH = 1.70

Science

Chemistry

Calculate the pH of the following system if [Cd²*] = 0.2 M and PH, = 0.5 atm. The standard emf is -O.403 V and the measured emf is -0.332 V. Cd2*(aq) + H2(g) --> 2H*(aq) + Cd(s)

Calculate the pH of the following system if [Cd²] = 0.2 M and PH, = 0.5 atm. The standard emf is -O.403 V and the measured emf is -0.332 V. Cd2(aq) + H2(g) --> 2H*(aq) + Cd(s)

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...

See similar textbooks

Similar questions

5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.
A solution of malonic acid, H2C3H2O4H2C3H2O4 , was standardized by titration with 0.1000 M NaOHNaOH solution. If 21.68 mLmL of the NaOHNaOH solution were required to neutralize completely 13.00 mLmL of the malonic acid solution, what is the molarity of the malonic acid solution? H2C3H2O4+2NaOH→Na2C3H2O4+2H2OH2C3H2O4+2NaOH→Na2C3H2O4+2H2O
5. Hydrogen cyanide has the chemical formula HCN. The compound occurs as a colourless gas or a pale blue liquid. Its solution in water is called hydrocyanic acid. It reacts with water as per the reaction below. What is the pH of 0.176 mol/L solution of the above acid (K = 4.98 x 10')? -9 a HCN(aq) + H₂O(l) ↔ CN¯(aq) + H₂O*(aq) (answer + units)
Q3 Caleulate the pH of a solution containing (0.1 M) of [Fe+] [Mg+]. knowing that Ksp is for Fe(OH)s= 1410™, and for Mg(OH),= 110712 log3=0.47. log5=0.7
Consider the reaction below: HOCI(aq) + H2O(!) 2 OCI"(aq) + H3O*(aq) The Brønsted-Lowry bases in this reaction are: O H20(!) & OCI(aq) O HOCI(aq) & H30*(aq) O HOCI(aq) & OCI(aq) O H20(?) & H30*(aq)
For the titration of 20.0 mL of 0.400 M HCI(aq) with 0.400 M NAOH(aq): HCI(ag) + NaOH(aq) NaC(aq) + H2O) 1. What is the initial pH of the HC(aq)? pH = |Select ] 2. What is the pH of the HCI(aq) after the addition of 10.00 mL of NaOH ? pH= [ Select] 3. What is the pH of the HCI(aq) after the addition of 20.0 mL of NaOH? pH [ Select]
HA, a weak acid, also forms the ion HA, in solution. The reaction is HA(aq) + A (aq) = HA, (aq) The weak acid has K, = 8.64 × 10-7 and the reaction has K = 3.80. Calculate the concentrations of A, H*, and HA, in a 1.00 M solution of HA. [A¯] = M [H*] = M [HA,] = M
Calculate the pH for each case in the titration of 50.0 mL of 0.180 M HCIO(aq) with 0.180 M KOH(aq). Use the ionization constant for HC1O. What is the pH before addition of any KOH? КОН? pH = %3D What is the pH after addition of 25.0 mL KOH? pH = What is the pH after addition of 30.0 mL KOH? pH = What is the nH after addition of 50.0 ml. KOH? Question Source: McQuarrie, Rock, And Gallogly 4e General Chemsitry | Publisher: Ur
7. The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq) (Z) 25.0 mL of 1.0 M CH3COOH(aq) Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)True
Boric acid, BOH is used as a mild antiseptic. What is the pH of a 0.025 aqueous solution of boric acid? What is the degree of ionisation of boric acid in this solution? The hydrogen ion arises principally from the reaction: B(OH),(aq) + H,0(1) = B(OH)4 (aq) + H* (aq) The equilibrium constant for this reaction is 5.9 x 10-10
Predict the effect of adding H2O liquid to the equilibrium reaction
A solution of malonic acid, H2C3H2O4H2C3H2O4 , was standardized by titration with 0.1000 M NaOHNaOH solution. If 20.19 mLmL of the NaOHNaOH solution were required to neutralize completely 12.25 mLmL of the malonic acid solution, what is the molarity of the malonic acid solution? H2C3H2O4+2NaOH→Na2C3H2O4+2H2OH2C3H2O4+2NaOH→Na2C3H2O4+2H2O