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OSTWALD – DILUTION LAW 1. Calculate the dissociation constant of monobasic acid which is 3.5% dissociated in N/20 solution at 20o C. (6.34x10-5) 2. Calculate the hydrogen ion concentration in 10 liters of 0.1 N solution of an acid having dissociation constant 4.0x10-10 . (6.32x10-6g ion liter-1 ) 3. Nicotinic acid (Ka =1.4x10-5) is represented by the formula HNic. Calculate its percent dissociation in a solution which contains 0.10 mol of nicotinic acid per 2.0 liter of solution. (1.66%) 4. A certain weak acid has Ka=1.0x10-4. Calculate the equilibrium constant for its reaction with strong base. (1010) 5. 0.16 g of N2H4 are dissolved in water and the total volume made upto 500 ml. Calculate the percentage of N2H4 that has reacted with water in this solution. The Kb for N2H4 is 4.0x10-6M. (2%)

6. An aqueous solution of aniline of concentration 0.24M is prepared. What concentration of sodium hydroxide is needed in this solution so that anilinium ion concentration remains 1x10-3M?
(Ka for C6H5NH3+ =2.4x10-5M) (10-2M) 7. An aqueous solution contains 10% ammonia by mass and has a density of 0.99g cm-3. Calculate hydroxyl and hydrogen ion concentration in this solution.(Ka for NH4=5.0x10-10M) (9.28x10-13 mol L-1)

CALCULATION OF pH 8. Calculate pH value of (a) .00001M HCl solution, and (b) 0.04M HNO3 solution assuming complete dissociation in each case. (4)(1.398) 9. Calculate the hydrogen ion concentration in moles/liter of a solution whose pH is 5.4 (3.98x10-6mole/liter) 10. Will the pH of water be same at 4oc and 25oC? Explain?

11. Saccharin (Ka=2x10-12) is a waek acid represented by formula HSac. 4x10-4 mole amount of saccharin is dissolved in 200 cm3 water of pH3. Assuming no change in volume, calculate the concentration of Sac- ions in the solution at equilibrium. 4x10-12M

12. A solution of HCl in water has a pH of 5. If 1 ml of this solution is diluted to one liter, what will be pH of the resulting solution? (6.98)

13. Calculate the pH value of 0.0001 M NaOH solution. (10)

14. Taking barium hydroxide to be completely ionized, calculate the pH of 0.001 M solution of it.

15. How many moles of calcium hydroxide must be dissolved to produce 250 ml of an aqueous solution of ph 10.65? Assume complete dissociation56x10-4 16. What is the pH of a 0.50 M aqueous NaCN solution? pKb of CN- is 4.70. (11.5) 17. Calculate the pH of a 0.01 M solution of acetic acid, Ka for CH3OOH is 1.8x10-5 at 25oC. (3.37) 18. The pH of 0.10 M hydrocyanic acid solution is 5.2. what is the value of Ka for hydrocyanic acid? (39.6x10-11) 19. The pH of 0.05 M aqueous solution of diethylamine is 12. Calculate its Kb. (2.5x10-3) 20. The value of Kw is 9.55x10-14 at a certain temperature, calculate the pH of water. ( 6.51) 21. Find the pH of 0.002 M acetic acid solution, if it is 2.3% ionized at this dilution. (4.3372) 22. Calculate the pH value of the mixture containing 50 c.c M-HCl and 30 c.c. M-NaOH solution assuming both to be completely ionized. (0.6021) 23. Calculate the pH value of the mixture containing N HCl and 30 c.c. of N NaOH solution both to be completely dissociated in normal solution.
24. What would be pH of a solution that contains 100ml of 0.1 N HCl and 9.9 ml of 1.0N NaOH solution? (3.05) 25. What will be the resultant pH when 200 ml of an aqueous solution of HCl (pH=2.0) is mixed with 300 ml of an aqueous solution of NaOH (pH=12.0)?
26. Calculate the pH of a solution made by diluting 25 c.c. of N/100 HCl to 500 c.c. assuming complete ionization of HCl. (3.3) 27. How many grams of NaOH must be dissolved in one liter of solution to give a pH value of 12? (0.40 gm ion/liter)

28. The dissociation constant of weak acid HA is 4.9 x10-8.after making the necessary approximation, calculate (i) percentage ionization, (ii) pH and (iii) OH- concentrationin a decimolar solution of the acid. Water has a pH of 7. 29. How many grams of NH4Cl should be dissolved in 500 ml of water to have solution of pH 4.5? Kb for ammonium hydroxide is 1.8x10-5.

30. What is the pH of a 1.0 M solution of acetic acid? To what volume must one liter of this solution be diluted so that the pH of the resulting solution will be twice the original value? Given Ka=1.8x10-5. (2.78x104 lit)
COMMON ION EFFECT 31. Calculate the hydrogen ion concentration in a solution containing 0.04 mole of acetic and 0.05 mole of sodium acetate in 500 ml of the solution. Dissociation constant for acetic acid is 1.8x10-5. 1.44x10-5M 32. A solution contains 0.10 M H2S and 0.3 M HCl. Calculate the concentration of S2- and HS- ions in the solution. For H2S, Ka1 = 1.0x10-7 Ka2 = 1.3x10-13

33. Two acids A1 and A2 have their dissociation constant as 0.00018 and 0.0037 respectively at 25oC. What would be the relative dilution of the acids so that the solutions becomes isohydric? (1:20.5)

34. Determine the concentration of OH- in 0.4 M NH4OH solution and also in the above solution having 5.35g of NH4Cl in a liter of the solution; Kb for NH4OH is 1.8x10-5

BUFFER SOLUTION 35. 0.1 mol of methyl amine (kb=5x10-4) is mixed with 0.08 mol of HCL and the solution is diluted to 1 liter. Determine the hydrogen ion concentration of the resulting solution. (8x10-11M) 36. Calculate composition of an acid buffer solution of total molarity of 0.09 and having a pH of 4.4. dissociation constant of the acid 1.8x10-5. (Salt =0.09M acid=0.20M) 37. Calculate the amount of NH3 and NH4Cl required to prepare a buffer solution of pH 9.0, when total concentration of buffering reagents is 0.6 mol L-1. pKb for NH3=4.7, log2=0.30. (0.04 mo/lt, 0.2 mo/lt)

38. Calculate the amount of (NH4)2SO4 in grams which must be added to 500 mL of 0.200 M NH3 to yield a solution with pH 9.35(Kb for NH3=1.78x10-5) (10.49g) 39. How many grams moles of HCl wioll be required to prepare one liter of a buffer solution (containing NaCN and HCN) of Ph 8.5 using 0.01 gram formula weight of NaCN? K dissociation (HCN)=4.1x10-10 (8.85×10-3) 40. A 40.0 ml solution of a weak base, BOH is titrated with 0.1 N HCl solution. The pH of the solution is found to be 10.04 and 9.14 after respectively. Find out the dissociation constant of the base. (1.828 x10-5) 41. The concentration of HCN and NaCN in a solution is 0.01M each. Calculate the concentration of Hydrogen and hydroxyl ions if the dissociation constant of HCN is 7.2x10-10. (H+=7.2 x10-10M, OH-= 1.39 x10-5M) 42. What volume of 0.10 M sodium formate solution should be added to 50 mL of 0.05 M formic acid to produce a buffer solution of pH 4.0? pKa for formic acid is 3.80. (39.62 ml) 43. 0.15 mol of pyridinium chloride has been added into 500 cm3 of 0.2 M pyridine solution. Calculate pH and hydroxyl ion concentration in the resulting solution assuming no change in volume. (Kb for pyridine = 1.5x10-9 M) (5, 10-9mol/lt) 44. A base B has a Kb of 8.1x10-8. In what amounts should 0.02 m HCl and 0.02 m base be mixed to make 200 mL of a buffer of pH7? (61.8 ml,138.2ml) 45. How many moles of sodium propionate should be added to one liter of an aqueous solution containing 0.020 mole of propionic acid to obtain a buffer solution of pH 4.75? what will be the pH if 0.010 mole of hydrogen chloride is dissolved in the above buffer solution? Compare the last pH value with the pH of 0.010 molar HCl solution. Dissociation constant of propionic acid, Ka at 25oC=1.34x10-5. (1.5072 x10-2mo, 4.09, 2) 46. The [H+] in 0.2M solution of formic acid is 6.4x10-3 mole liter-1. To this solution sodium formate is added so as to adjust the concentration of sodium formate to one mole liter-1. What will be pH of this solution? Ka for HCOONa is 2.4x10-4 and dissociation of HCOONa is 0.75. (4.19) 47. A buffer solution of acetic acid and sodium acetate of 1 M concentration was prepared and its pH was found to be 4.74. Calculate pH of system (i) when 0.01 mole of HCl is added to a liter of the above solution (ii) when 0.01 mole of NaOH is added per liter of the above solution (Ka=1.8 x10-5) (4.73, 4.75)

48. An acidic type indicator, HIn differs in colour from its conjggate (In-). The human eye is sensitive to color difference only when the ratio [In-]/[HIn] is greater than 10 or smaller than 0.01. what would be the minimum change in pH of the solution to observe a complete colour change(Ka=1.0x10-5) (2) 49. Calculate the change in pH of one liter of buffer solution containing 010 mole each of NH3 and NH4Cl upon addition of (i) 0.02 moledissolved gaseous HCl (ii) 0.02 mole of dissolved NaOH Assume no change in solution volume.(Kb for NH3=1.8x10-5)
(Decreases by 0.1761, Increases by 0.1761 ) 50. The pH of blood stream is maintained by a proper balance of H2CO3 and NaHCo3 concentration. What volume of 5 M NaHCO3 solution should be mixed with a 10mL sample of blood which is 2M in H2CO3, in order to maintain a pH of 7.4? Ka for H2CO3 in Bolood is 7.8x10-7. (78.36 ml) 51. What is the pH of the solution when 0.20 mole of hydrochloride acid is added to one liter of a solution containing (i) 1 M each of acetic acid and acetone ion? (ii) 0.1M each of acetic acid and acetone ion?
The dissociation constant of acetic acid is 1.8x10-5 (4.5686,1) 52. The dissociation constant of an acid HA at 25oC is 1.34x10-5. How many moles of sodium salt of this acid should be added to one liter of an aqueous solution containing 0.020 moles of this acid to obtain a buffer solution of pH 4.75? What will be pH if 0.010 mole of hydrogen chloride is dissolved in the above buffer solution? (0.015) (4.09) 53. 20 mL of 0.2M NaOH is added to 50 mL of 0.2M acetic acid to give 70 mL of solution. What is the pH of the solution? Calculate the additional volume of the solution 4.74. the ionization constant of acetic is 1.8x10-5 (4.5686)(4.86 ml) 54. 500 mL of 0.2 M aqueous solution of acetic acid is mixed with 500 ml of 0.2M HCl at 25oC (i) Calculate the degree of dissociation of acetic acid in the resulting solution and pH of the solution. (ii) If 6 g of NaOH is added to the above solution, determine the final pH.[Assume there is no change in volume on mixing ; Ka of acetic acid is 1.75 x10-5 mol L-1] (1) (4.75) 55. Two buffers, (X) and (Y) of pH 4.0 and 6.0 respectively are prepared from acid HA and salt NaH. Both the buffers are 0.50 M in HA. What would be the pH of the solution obtained by mixing equal volumes of the two buffers?(KHA = 1.0x10-5) (5.7) 56. When 0.002 mole of acid is added to 250mL of a buffer solution, pH decreases by 0.02 units. Calculate the buffer capacity of the system. (0.4)

HYDROLYSIS OF SALT 57. Calculate the hydrolysis constant of the salt containing NO-2 ions, Ka for HNO2=4.5x10-10 (2.2 x10-3) 58. Calculate the degree of hydrolysis of N/10(i.e. , 0.1 M) solution of sodium acetate at 25oC; Ka=1.8x10-5 (7.452 x10-2) 59. Calculate the percentage of hydrolysis in 0.003 M aqueous solution of NaOCN. (Ka for HOCN=3.33x10-4 M) (0.01%) 60. For 0.50 M aqueous solution of sodium cyanide, (pKb of CN- is 4.70), calculate (i) hydrolysis constant, (ii) degree of hydrolysis and (iii) pH. (2 x10-5)(6.3 x10-3)(11.5) 61. Calculate the percentage hydrolysis of a mixture of aniline and acetic acid in 0.1 M solution (Ka=1.8x10-5 and Kb=4.6 x10-10) (0.523) 62. Calculate the degree of hydrolysis and pH of 0.1M sodium acetate solution. Also calculate the concentration of all the ions at equilibrium. Hydrolysis constant of sodium acetate is 5.6x10-10 (7.5x10-6)(7.5x10-7mol/lt) 63. Ka for ascorbic acid (HAsc) is 5x10-5. Calculate the hydrogen ion concentration and percentage of hydrolysis in an aqueous solution in which concentration of Asc- ions is 0.20M. (5x10-9)(0.1%) 64. When 0.20 M acetic acid is neutralized with 0.20M NaOH in 0.50 liter of water, the resulting solution is slightly alkaline, calculate the pH of the solution (Ka for acetic acid = 1.8 x10-5) (8.873) 65. Ka for butyric acid is 2.0 x10-5. Calculate pH and hydroxyl ion concentration of 0.2M aqueous solution of sodium butyrate. (9)(10-5M) 66. Calculate the pH of an aqueous solution of 1.0M ammonium formate assuming complete dissociation. (pKa of formic acid=3.8 and pKb of ammonia =4.8) (6.5) 67. Calculate the pH at the equivalence point when a solution of 0.10 M acetic acid is titrated with a solution of 0.10 M sodium hydroxide. Ka for acetic acid is 1.9x10-5 (8.71) 68. 0.1 M NaOH is titrated with 0.1 M HA till the end point; Ka for HA is 5.6x10-6 and degree of hydrolysis is less compared to 1. Calculate pH of the resulting solution at the end point. (9) 69. Calcium lactate is a salt of weak organic acid and represented as Ca(Lac)2 contains 0.13 mol of this salt in 0.50 litre solution. The pH of this solution is 5.60 . assuming a complete dissociation of the salt, calculate Ka of lactic acid (8.26x10-4.)
SOLUBILITY PRODUCT 70. A sample of hard water contains 0.005 mole of CaCl per litre. What is the minimum conc. Of Na2SO4 which must be added for removing Ca2+ ions from the water sample. Ksp for CaSO4 is 2.4x10-5 at 25oC.

71. The solubility product of Mg(OH)2 at 25oC is 1.4x10-11. What is the solubility of Mg(OH)2 in gm per litre?

72. The solubility product of AgCl in water is 1.5x10-10. Calculate its solubility in 0.01 M NaCl aqueous solution.

73. Calculate the solubility of AgCl(s) in pure water and in 0.1 M NaCl at 25oC.
Ksp(AgCl)=2.8x10-10Comment on the influence of [Cl-] on the solubility of AgCl.

74. The solubility product of SrF2 in water is 8x10-10. Calculate its solubility in 0.1M NaF aqueous solution.

75. If the solubility of calcium sulphate in water is 1.03x10-5, what will be its solubility in 0.005 M solution of sulphuric acid? 76. The solubility product (Ksp) of Ca(OH)2 at 25oC is 4.42 x10-5. A 500 ml of saturated solution of Ca(OH)2 is mixed with equal volume of 0.4 M NaOH. How much Ca(OH)2 in milligram is precipitated?

77. A sample of AgCl was treated with 5.00 mL of 1.5 M Na2CO3 solution to give Ag2CO3. The remaining solution contained 0.0026 g of Cl- per liter. Calculate the solubility product of AgCl.[Ksp for Ag2CO3=8.2x10-12]

78. The solubility product of BaSO4 is 1.5x10-9. Find out its solubility in (i) pure water and (ii) 0.1 M BaCl2.

79. The solubility of Pb(OH)2 in water is 6.7x10-6M. calculate the solubility of Pb(OH)2 in a buffer solution of pH=8. 1.2x10-3 M

80. Calculate the solubility of AgCN in a buffer solution of pH 3.00; Ksp for AgCN is 1.2x10-16 and Ka for HCN is 4.8 x10-10. 81. Calculate the simultaneous solubility of AgCNS and AgBr, Ksp for AgCNS and AgBr are 1.0 x10-12 and 5.0x10-13 respectively.

82. Determine the number of moles of AgI which may be dissolved in 1.0 liter of 1.0 M CN- solution; Ksp for AgI and Kf for [Ag(CN),]- are 1.2x10-17 M2 and 7.1 x1019, respectively.

83. The solubility product Ksp of lead bromide is 8x10-5. If the salt is 80% dissociated in saturated solution, find the solubility of the salt.

84. The concentration of the Ag+ ion in a saturated solution of Ag2C2O4 is 2.2x10-4 mole per liter. Determine the solubility product of Ag2C2O4.

85. Calculate the solubility product of lead iodide at 25oC. Its solubility at given temperature is 0.7g liter-1.

86. Calculate the pH at which Mg(OH)2 begins to precipitate from a solution containing 0.10 M Mg2+ ions. Ksp for Mg(OH)2=1.0x10-11

87. The solubility product of Ag2C2O4 at 25oC is 1.29x10-11 mol3 L-3. A solution of K2C2O4 containing 0.1520 moles in 500 mL water is shaken at 25oC with excess Ag2CO3 till the following equilibrium is reached:
Ag2CO3 + K2C2O4 ==Ag2C2O4 + K2CO3
At equilibrium, the solution contains 0.0358 moles of K2CO3. Assuming the degree of dissociation of K2C2O4 and K2CO3 to be equal, calculate the solubility product of Ag2CO3. 88. Freshly precipitated aluminium and magnesium hydroxides are stirred vigorously in a buffer solution containing 0.25 mol/L of ammonium chloride and 0.05 mol/L of ammonium hydroxide. Calculate the concentration of aluminium and magnesium ions in solution.

89. Given : Ag(NH3)+2==Ag++2NH3, Kc=6.2x10-8 and Ksp of AgCl=1.8x10-10 at 298 K. Calculate the concentration of the complex in 1.0M aqueous ammonia.

90. Predict if a precipitate will be formed or not in a solution having concentration of Ba2+ ions of 1x10-3 M and that of SO2-4 ions of 2X10-4 M; solubility product of BaSO4 is 1x10-10.

91. Predict whether a precipitate will be formed or not when equal volumes of 2x10-6 M BaCl2 solution and 2x10-5 M Na SO4 solution are mixed. The solubility product of barium sulphate is 1x10-10.

92. ½ liter of 2x10-3 M AlCl3 and ½ liter of 4x10-2 M solution of NaOH are mixed and the solution is diluted to 102 liters with water at room temperature will a precipitate exist? Given Ksp for Al(OH)3=5x10-33.

93. Calculate the NH+4 ion concentration (derived from NH4Cl) needed to prevent Mg(OH)2 from precipitating in a liter of solution which contains 0.010 mole of Mg2+. The ionization constant of ammoni a is 1.8x10-5 and Ksp of Mg(OH)2 is 1.23x10-11

94. A solution has 0.05 M Mg2+ ions 0.05 M NH3. Calculate the concentration of NH4Cl required to prevent the formation of Mg(OH)2 in this solution Ksp of Mg(OH)2 = 9.0x10-12 and ionization constant of NH3=1.8x10-5. 95. You are provided with a 500 mL of hard water, containing 0.005 mole of CaCl2 and two sulphuric acid sample of 0.001 M and 0.02 M concentration. Which one or both or none can be used for precipitating out calcium ion? The solubility product of calcium sulphate in water at 25oC is 2.4x10-5. 96. What [H3O+] must be maintained in a saturated H2S solution to precipitate Pb2+, but not Zn2+ from solution in which each ion is present at a concentration of 0.01M? [Ksp H2S=1.1x10-22 and Ksp ZnS=1.0x10-21]

97. A lead salt is dissolved in HCl which is 94% ionized. It is found to have 0.1M Pb2+ and 0.28M[H+] ions. The solution is saturated with hydrogen sulphide gas; find out the amount of Pb2+ ions that remains 4x10-10 and that of H2S is 1.1 x10-22.

98. A solution contains a mixture of Ag+(0.10M) and Hg2+2 (0.01M) which are to be separated by selective precipitation. Calculate which one of them gets precipitated almost completely. What percentage of that metal ion is precipitated?
[Ksp : Agl=8.50x10-17; Hg2I2=2.5x10-26]

99. An aqueous solution of a metal bromide MBr2 (0.05M) is saturated with H2S. what is the minimum pH at which MS will precipitate ? Ksp for MS=6.0x10-21: concentration of saturated H2S=0.1M : K1=10-7 and K2=1.3x10-13 for H2S.

100. The average concentration of SO2 in the atmosphere over a city on a certain day is 10ppm, when the average temperature is 298K. given that the solubility of SO2 in the water at 298K is 1.3653 moles liter-1 and the pKa of H2SO3 is 1.92, estimate the pH of rain water on that day.

Law of Electrolysis

1. From thevalues of the a faraday (996500C and ) Avogadro number (6.023x1023),calculet the Coulombic charge on an electron. 1.6x10-19coul 2. Find the charge in coulomb on 1 g ion of N3-. 2.89x105C 3. Hoe many atoms of calcium will be deposited from a solution of CaC12 by a current of 25 mA flowing for 60sec? 4.68x1018atoms of Ca 4. Copper sulphate solution (250mL) was electrolysed using a platinum anode and a copper cathode. A constant current of 2mA was passed for 16 min. It was found that after electrolysis the of the solution was reduced to 50% of its original value. Calculate the concentration of copper sulphate in the solution to begin whit. 7.95x10-5mol L-1 5. In a fuel cel, hydrogen and oxygen react to produce electricity. In the process hydrogen gas is oxidised at the anode and oxygen at the cathode. If 67.2 liter of H2 at STP react in 15 min, what is the average current is used for electro-decomposition of copper from copper(ll) solution, how many grams of copper will be deposited ?
Anode reaction: H2+ 2OH- 2H2O+2e-
Cathode reaction: O2+2H2O+2e- 4OH- (643.3A)(190.50g) 6. A solution of a salt of a metal of atomic mass 112 was electrolysed for 150 min with a current of 0.15A. The mass of metal deposited was 0.783 g. Find the equivalent mass and valency of the metal in the salt. (55.97) 7. A100W, 110V incandescent lamp is connected in series with an electrolyte cell containing cadmium sulphate solution. What mass of cadmium will be deposited by the current flowing for 10h? (19.06 g) 8. Chromium metal can be planted out from an acidic solution containing Cro3according to the following equation :
Cro3(aq)=6H+(aq)+6e- cr(s)+3H2O
Calculate (i) how many grams of chromiumwill be plated out by 24,000C and (ii) how long will it take to plate out 1.5g of chromium by using 12.5 A current? (2.1554g)(1336.15 sec) 9. The following reaction Zn(s)+Co2 Co(s)+Zn2+
Accurs in a cell. Write the electrode reactions and compute the standard EMF of the all cell. Give that
E0zn Zn2+= 0.76V
E0co Co2+=0.28V (0.48V) 10. An electric current of 0.5 A was passed through acidulated water for 1h. galculate.the volum of hydrogen at NTP peoduced. 1 G of electricity Deposisits0.00001 g of hydrogen. 0.2016liters 11. How many grams of silver could be plated out on a serving tray by electrolysis of a solution containing silver in +1 oxidation state for a period of 8.0 h at a current of 8.46A? What is the area of the tray if the thickness of the silver plating is 0.00254 cm? Density of silver is 10.5g/cm3. (272.178g)(1.02x104 cm2) 12. Electrolysis of a solution of MnSo4 in aqueous sulphuric acide is a method for the preparation of MnO2as per reaction.
Mn2+(aq)+2H2O Mno2(s) + 2H+(aq)+H2(g)
1kg of MnO2. What is the value of current efficiency? Write the reactions taking place at the cathode and the anode. (94.8%) 13. Silver is electrodeposited on a metallic vessel of surface area 800 cm2 by passing a current of 0.20 A for 3.0hrs. Calculate the thickness of silver deposited, given its density as 10.47g/cc [Atomic mass of Ag=107.92] 2.88x10-4cm

14. a current of 1.70 A is passed through 300.0mL of 0.160 M solution of ZnSo4 for 230 sec with a cuerrent efficiency of 90%. Find out the molarity of Zn2+ after the deposition of Zn. Assume the volumeof the solution to remain constant during the electrolysis. (0.154M) 15 (i) What is the mass of sodium bromated and molarity of solution necessary to prepare 85.5 mL of 0.672 N solution when the half-cell reaction is
BrO-3+6H++6e- Br-+ 3H2O (iii) What would be the mass as well as molarity if the half-cell reaction is
BrO-3 +12H+ 10e- Br2+6H2O (1.446g)(1.7352g) 16. Calculate the quantity of electricity that would be required to reduce 12.3 g of nitrobenzene to aniline, if the current is 50%. If the potential drop across the cell is 3.0V, how much energy will be consumed? (347.4J) 17. Calculate the mass and volume (at STP) of hydrogen and chiorine that will be formed by passing 10,000 C of charge through an aqueous solution of potassium chloride. the cell reaction is 2KCI+2H2O 2KOH+H2+Cl2 (1.160lit) 18. An acidic solution of cu2+salt containing 0.4 g of Cu2+is electrolysed until all the copper is deposited. The electrolysis is continued for seven more min with the volume of solution kept at 100mL and the current at 1.2A. calculate the volume of gases evolved at NTP during the entire electrolysis. (58.48mL) 19. 100 mL of a neutral solution containing 0.2g of copper was electrolysed till the whole of copper was deposited. The current strength was maintained at 1.2 A and the volume of solution was maintained at 100mL. Assuming 100% efficiency, find out the time taken for deposition of copper.[Atomic mass of copper =63.58] (506 sec) 20. Molten aluminium chloride is electolysed with a current of 0.5A to produce 27.0g of aluminium. (i) How many gram equivalent of aluminium were produced? (ii) How many gram atoms of aluminium were produced? (iii) How many atoms of aluminium were produced? (iv) How many electrons were produced? (v) What is the number of faraday of electricity consumed? (vi) How long did the electrolysis took place ? (vii) How many liters of chlorinz at STP were produced?
[atomic mass of Al=27, Avogadro No.=6.02x1023] Ans: (3geq of Al) (1g atom of aluminium) (6.02x1023)(18.06x1023) (3Fof electricity)(570240sec) 22. Calculate the quantiy of electricity that will be required for liberating 710g of chorine gas by the electrolysis of a concentrated solutionof NaCl. What (i) mass of NaOh, and (ii) what volume of hydrogen measured at 270cand 1 atm pressure will be obtained during the process? (20faradays of electricity)(246.1 lit) 23. Electric current is passed through two cells A and B in series. Cell A contains aqueous solution of Ag2SO4 and platinum electrodes. Cell B contains aqueous solution of CuSO4 and copper electrodes. The current is passed till 1.6g of oxygen is liberated at the quantities of copper and silver deposited at the cathodes of the two cells. [Atomic mass O=16,Cu=Ag=108] (6.35g of Cu) 24. Ten grams of a fairly concentrated solution of cupric sulphate is electrolysed using 0.01F of electricity. Calculate (i)the mass of the resulting solution and(ii) the number of equivalents of acid or alkali in solution. [Atomic mass O= 16,S=32,Cu=63.5] (9.6025g)(0.01g equivalent acid) 25. A current of 3.7A is passed for 6hrs between nickel electrodes in 0.5 liter of a 2M solution of Ni(NO3)2. What will be molarity of solution at the end of the end of the electrolysis?

26. 27. 28.…...

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