(iv) surface area of electrodes. 2. In the absence of dissolved ions, little current is passed. Calcium sulfate is slightly soluble; at equilibrium, most of the calcium and sulfate exists in the solid form of calcium sulfate. Calculate the molar conductivity. Solution: Molar conductivity = (1000 × k) /M = (1000 × 0. The molar conductivity of OH-is 3-5 times the conductivity of other small anions. The relation is applied to the λ ∞ and D s of alkali, tetra. Nov 19,2023 - Directions: In the following questions, A statement of Assertion (A) is followed by a statement of Reason (R). There are also some limited shock wave data for the conductivity of dilute (0. View solution > The molar conductivity of cation and anion of salt B A are 1 8 0 and 2 2 0. Conductivity of an electrolytic solution depends on (b) concentration of electrolyte (d) distance between the electrodes Solution: (a, b) Conductivity of electrolyte solution is due to presence of mobile ions in the solution. The correct Answer is: A, C. The common part of two methods is 19. The conductance of the water used to make up this solution is 0. (iv) surface area of electrodes. , and similarly for the anion. 1,2 The electrochemically active ion in alkaline electrolytes is the hydroxide ion. 1 mol L−1. Conductivity κ , is equal to _____. 10. mol L -1) We, know the unit of specific conductance k. Λ o = λ Ag + + λ Cl– = 138. Specific conductivity passes through a maximum with an increase in the concentration of electrolyte in aqueous solutions (Figure 10 a) and in non-aqueous solutions of ionic liquids (Figure 12 a). It is used to determine the efficiency of the electrolyte in the conducting electricity in solution. Size of ion: Ionic mobility is inversely proportional to the size of the ion. 51 × 10 −5 S cm −1) at ambient temperature (303 K). Solution. If the cell constant of the cell is 0. The polar water molecules are attracted by the charges on the K + and Cl − ions. On which factor does the conductance of electrolytic solutions depend? a) Temperature and pressure b) Number of charge carriers c) Dielectric constant of the solvent d) All of the mentioned View Answer. The molar conductivity, Λm, of protic ionic liquids (PILs) in molecular solvents is measured at 298. Λ = κ / C or Λ = κV. Compare this with the pH obtained using the [H 3 O +] of 5. The reduction potential of an electrode depends upon the concentration of solution with which it is in contact. (iii) the concentration of electrolytes in solution. The mis often determined using a. 7. where K is a constant. (iv) The conductivity of the solution increases with temperature. The more the ions in the solution, the less resistant the solution is (inverse proportion) and the more conductive it is (direct. In other For a salt solution prepared using a 1:1 salt , the molar conductivity can be expressed as the sum of ionic conductivities , λ+ λ + and λ− λ −. C. The size of the cation increases as we move from Li+ to Rb+. 1 ). This means that at a given structural relaxation rate, the molar ionic conductivity in aqueous solutions can be regarded as an upper limit for liquid electrolytes. Smaller the cation higher is the molar conductivity. For example, with increases in dilution, the number of ions present in the solution increases and the conductance of the solution increases. (M = Molar concentration or the number of moles of solute per litre solution) = k ×1000M ( ∵ The unit of M is expressed in molarity i. Explanation: Molar conductivity of ionic solution depends on the temperature and the concentration of electrolytes in solution. 1 litre of a solvent which develops an osmotic pressure of 1. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Molar conductivity for strong electrolytes increases due to increase in mobility of ions (as molecular interaction decreases on dilution). The molar. The strongest evidence for this is the molar conductivity of the salt (1. Hard. e. Electrical Conductivity of Ionic Surfactant Solutions. 3. Pour 100 (±1) cm of 1 (±0. pH = -log(H 3 O +)Molar conductance is defined as the conductance of all ions produced by dissociation of 1 gram mole of an electrolyte dissolved in V cc of the solution when electrodes are 1 cm apart and the area of the electrode is so large that the whole solution is contained between them. The conductance of a solution depends upon its dilution, no. In this work the conductivity data of three carboxylate surfactant systems: sodium (NaDec), potassium (KDec) and cesium (CsDec) decanoates aqueous solution in the concentration range 10 −3 − 0. Since the salt molar conductivity is the sum of the ionic contributions, it can be written in terms of the sum of the ion self-diffusion coefficients as (/ )( )FRTD D2 Λ =+ SS ∞ + ∞ − ∞ (2) for a solution of a 1:. Define molar conductivity and explain its significance. The molar conductivity of OH-is 3-5 times the conductivity of other small anions. 6. 5xx10^ (-5)" S "m^ (-1). Molar ionic conductivities of a bivalent electrolyte are 57 and 73. The molar conductivity of ionic solution depends upon various factors. Class 12. Molar conductivity of ionic solution depends on: This question has multiple correct options. Molar Conductivity Page 7 R 1 R2 R3 Null point detector A. Doubt Solutions - Maths, Science, CBSE, NCERT, IIT JEE, NEET. Solution: Using the formula for molar conductivity, Λm = (1000 × k) / M. surface area of electrodes. Add a third drop of 1. It was shown by many researchers that the structure of liquid electrolyte solutions depends on the type of the salt and solvent and their. 1 mol/L. Using equation (a), the electrolytic conductivity κ κ is related to the ionic conductivities using equation (c) The curvature of the plots for intermediate electrolytes is a simple consequence of the Le Chatelier effect, which predicts that the equilibrium. Here κ κ is the conductivity. κ = l RA κ = l R A. In otherFor a salt solution prepared using a 1:1 salt , the molar conductivity can be expressed as the sum of ionic conductivities , λ+ λ + and λ− λ −. It also depends on the viscosity and the temperature. 1 M C H 3 C O O H solution is 7. The cell constant is the ratio of the known conductivity (µS/cm) to the mea-sured conductance (µS). 45, 426. 3 OH has. Molar ionic conductivites of a bivalent electrolyte are 57 and 73. The ionic conductivity can be determined by various methods. 6 g of a solute is dissolved in 0. S. When considering weak electrolytes, molar conductivity and molar concentration share an inverse relationship. (iii) concentration of electrolytes in solution. C. The molar conductivity of a solution rises as the concentration of the solution decreases. (i) temperature. The influence of ion-ion interactions on the conductivity of strong electrolytes was studied by Debye and Huckel. We have selected these salt-water systems primarily because it is expected that ion-pairing in these. The molar conductivity of an ionic solution depends on (a) Concentration of electrolytes in solution (b) Distance between electrodes (c ) Surface area of electrodes. 02 M solution of KCl at 298 K is 0. For this purpose, the molar conductivity ratio (Λ i m p Λ N M R) of an IL is used as a measure of the ionicity: I = Λ i m p Λ N M R. 15 K, are analyzed by a transport theory in the frame of the mean spherical approximation. The electrical conductances of very dilute solutions of the ionic liquids 1-ethyl-3-methylimidazolium tetrafluoroborate [emim][BF4] and 1-butyl-3-methylimidazolium tetrafluoroborate [bmim][BF4] in the low-permittivity solvent dichloromethane have been measured in the temperature range from 278. (ii) distance between electrodes. 2) I = 1 2 ∑ i C i z i 2. Conductivity ( mS/cm) vs Ionic Radius. However, the "molar ionic conductivity" of H+ and OH- is greater than all other ions, so in a solution containing many species of ion, the H+ and OH- ions would usually have the most effect on. where c is the molar concentration of the added electrolyte. The usual symbol is a capital lambda, Λ, or Λ m. where V is the volume of the solution in cm3 containing one gram mole of the electrolyte. In more dilute solutions, the actual. To calculate the conducting electricity of an ionic solution, molar conductivity comes into play. Therefore, molar conductivity (Λ) is usually helpful in evaluating the contribution of the ion mobility (μ) to the ionic conductivity: [2] Λ = σ i c c : salt concentration in moles per liter. (i) 1 l R A (ii) * G R (iii) Λm (iv) l A 26. 15 K at 5 K intervals. The coefficients S and E depend only on the ion charges, whereas coefficients J 1 and J 2 show additional dependence on the distance of closest ion approach (R) in the solution. 10. Measurement of the Conductivity of Ionic Solutions. Molar Conductivity (Λ) behaviour of 1-butyl-3-methylimidazolium (Bmin) acetate and Bmin chloride (Bmin Cl) ionic liquids compared to lithium perchlorate (LiClO 4) has been studied in aqueous and acetonitrile (ACN) solution at ambient temperature. Note:The specific conductivity of the solution depends on the size of the ions present in the solution. Ionic liquids and the surfactant were stored in a vacuum desiccator. Kohlrausch's law greatly simplifies estimates of Λ 0. Repeat steps 1–10 with 1. Updated on: 21/07/2023. The value of Λ m for a given solvent and temperature depends upon the nature of the electrolyte, i. The mis often determined using a. The salts don't have to be ionic all of the time. Measurement of the Conductivity of Ionic Solutions. At infinite dilution, all ions are completely dissociated. The molar conductivity of an electrolyte is defined as the electrolytic conductivity divided by the molar concentration C of the dissolved electrolyte. 4. FIG. Ionic Electrolytes Water and other polar molecules are characterized by a slightly positive. 1 25. Temperature. (ii) distance between electrodes. where: λ+ = F ⋅u+ and λ− = F ⋅u− are the molar conductivity of the cation and the anion re-spectively. If M is the concentration of the solution in mole per litre, then. Concentration of electrolytes in solution d. The ionic strength is calculated using the following relation for all the ions in solution: (4. 1) M X ( a q) = M ( a q) + + X ( a q) –. 15 K. If Kohlrausch's law is valid, then molar conductance of aluminium sulphate at infinite dilution will be_____. A. Figure 1 shows the temperature and concentration dependence of the molar conductivity of potassium iodide in ethanol. The measurements were done in five replicate runs. For an ideal measurement cell and electrolyte it is defined as. Example: The order of size. (iv) surface. For measuring the resistance of an ionic solution, we face two difficulties: 1) For. (iv) Copper will deposit at anode. CBSE Science (English Medium) Class 12. Temperature b. Table 3. Some majorly used electrolytes are potassium, chloride, sodium, magnesium, phosphate, and calcium. The limiting ionic molar conductivity (λ ∞) of an electrolyte solution depends on the self-diffusion coefficient (D s) of the pure solvent when the temperature (T) changes. 9C. The structure and stability of the aggregates depend on the ions and the solvent, Coulombic attractions, the hydrogen bonds between anion and the hydrogen atoms in. The Debye-H"uckel-Onsager theory successfully predicts the conductivity at very low ionic concentrations of up to a few millimolars, but there is no well-established theory. Λ = λ+ +λ− (1. Distance between electrodes c. 01 to 50,000 uS/cm. (a, b) 2. The molar conductivity of solution is equal to the sum of the ionic contributions. It is affected by the nature of the ions, and by viscosity of the water. Analysis of the available thermal conductivity data for the molten alkali and alkaline-earth salts, performed with the standard least square method and the interval analysis, reveals that the molar thermal conductivity of the molten alkali halides and alkali nitrates at temperatures close to their melting point has a constant value, equal to 19. (B) Nature of solvent. 1 Study App and Learning App with Instant Video Solutions for NCERT Class 6, Class 7, Class 8, Class 9, Class 10, Class 11 and Class 12, IIT JEE prep, NEET preparation and CBSE, UP Board, Bihar Board, Rajasthan Board, MP Board, Telangana Board etcThe ionic strength of a solution is a measure of the concentration of ions in that solution. 01 M. To determine a solution’s conductivity using Eq. Stability of ionic crystal depends on lattice energy which is released in the form of heat when two ions are brought together to form a solid. 0200- M solution of acetic acid. In this work, the experimental conductivity data will be analyzed by Barthel's low-concentration chemical model (lcCM) to obtain the association constants, K A (T), and limiting molar conductivities at infinite dilution, Λ ∞ (T). mol -1 (Siemens X meter square per mol). Equation 2 is called Kohlrausch's law and sure enough was derived by Kohlrausch based on the. The number of ions furnished by an electrolyte in solution depends upon the degree of dissociation with dilution. Assertion (A): Molar Conductivity of an ionic solution depends on temperature. In 1880 the German physicist George Kohlrausch introduced the concept of molar conductivity which is used to compare conductance of different solutions. ). 1 M C H 3 C O O H solution is 7. 11. Clarification: Conductance is dependent on the concentration of the electrolytic solution. > Small ions have small areas. A. nature of solvent and nature of solute. Answer: (a) The molar conductivity of an ionic solution depends on the concentration of electrolytes in solution. 01:27. 5. solution of known conductivity. May 7, 2020 at 15:37. Molar conductivity of ionic solution depends on _____. 0. Figure 13. 1: Variation of molar conductivity as a function of molar concentration. HCl is a strong acid and completely dissociates in water, therefore the pH will be equal to the negative logarithm of the concentration of HCl. 8 Answers 5. (a, c) are both correct options. ∴ Λ m = κ CCorrect option is B) λ m=KV With decrease in soncertration, total volume V of the solution containing one mole of electrolyte also increases and decrease in K (conductivity) on dilution of a solution is more than compensated by increase in its volume, hence molar conductivity (λ m) increases. d. Q3. . D. Solution: Question 21. First find moles of acid: grams / molar mass = moles. Molar ionic conducti. solutions at a low concentration, I < 0. asked Feb 12, 2022 in Chemistry by Harshitagupta (25. The molar conductivity was predicted with the Debye-Hückel-Onsager extended equation, Equation (11), using the viscosity of water (0. 15 to 303. ( pm) . To illustrate the relation between transference numbers and conductivity, the transport number of potassium in dilute potassium chloride solution is used to find the limiting ionic conductivity. 1 mol L−1. The relation between molar conductance (λ) and specific conductance denoted as (k) is given by. 1 EC = 1 µS/cm = 1 x 10 – 6 S/m. Solution For Molar conductivity of ionic solution depends on. On the contrary, at this stage the solu-• The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance. The area of the electrodes is 1 . (iv) surface area of electrodes. It is therefore not a constant. The ratio d/A is constant for any given. 27. 0248 S cm −1. surface area of electrodes. Ionic conductivity is electrical conductivity due to the motion of ionic charge. 1 S cm2mol-1 and 7°(C1-) = 76. 8 m h o c m 2 m o l − 1 at the same temperature. Molar conductivity, which can be determined by a solution’s ionic strength or salt concentration, is the conductance of a solution containing one mole of electrolyte. In the familiar solid conductors, i. The probes used in this experiment measure conductivity in either mS/cm or S/cm. 0 M calcium chloride solution. 1) . The equation Λ m = ( k x1000)/M can be used to get units of molar conductance. Ionic contributions of ions can be evaluated from the limiting molar conductivities of strong electrolytes containing the same ions. Size of gasesous ion : Cs + > Rb + > K + > Na + Size of aqueous ion : Cs + < Rb + < K + < Na + Conductivity : Cs + >. Use this information to estimate the molar solubility of AgCl. However, I am looking for values at 1 M, and I'm having a hard time finding that information. Water molecules in front of and behind the ions are not shown. The molar conductivity of 0. Physically, it. Solution: Question 21. 1molL −1KCl solution is 1. With the objective to fill this gap and gain further understanding on the fundamental properties of ion conducting materials, we are studying systematically the mechanical. Molar conductivity is defined as the conductivity of an electrolytic solution divided by the molar concentration of the electrolyte mkc On increasing the temperature the mobility of ions increases Hence molar conductivity increases by increasing temperature Also molar conductivity and concentration of electrolyte is inversely proportional to. Step by step video, text & image solution for Molar conductivity of ionic solution depends on_____. More concentration means more dissolved salt per volume of water, and more salt means more ions available to shuttle. 2 shows the Walden plots of ionic liquid [C4py][DCA] and other ILs. Electrolyte solutions: ions are the charge carrying particles. The formula for molar conductivity is the following:Molar conductivity \[=\dfrac{K}{C}\] So the correct option for this is option (A) and option (C). 15 and 328. For example, Calero et al. metals and semiconductors, the charge movement, or current, is due to electrons or holes and is described as electronic conductivity. False It depends on the experimental parameters. (ii) Copper will dissolve at anode. Electrolytic conductivity is very low in dilute solutions and increases much more gradually with increase in the concentration which is for the weak electrolyte and in the solution, this increase is due to increases in active ions. 3). Molar conductivity of ionic solution depends on. Molar conductivity of ionic solution depends on _____. Distance between electrodes c. 5) Medium View solutionThe theory considers the vicinity of each ion as an atmosphere-like cloud of charges of opposite sign that cancels out the charge of the central ion (Figure 25. According to the complex structure of ionic liquids, it is expected that the thermal conductivity of ILs depends on the type and structure of the cation and anion. Samples of polymer electrolyte for transference number and conductivity measurements were cut from the films in a form of thin discs, 16. Conductivity of aqueous solution of an electrolyte depends on:. 03:04. A more general definition is possible for an arbitrary geometry or sample composition. 5 in the generally accepted form of Arrhenius plots of ln(σT) vs. With an increase in dilution of the weak electrolytic solution, the molar conductivity of the solution is observed to increase. Λ o = λ Ag + + λ Cl– = 138. Courses. Theory. The conductivity depends on the type. The molar conductance of a solution depends upon its nature, concentration, and temperature. The molar conductivity of the solution formed by them will be. Thus, aqueous solutions of lithium salts have lower conductivities than those of cesium. For example, sodium chloride melts at 801 °C and boils at 1413 °C. In dilute solutions, the conductivity of the electrolyte solution is the sum of the conductivities of the ions in the solution, which can be expressed by the following equation: 20. Molar Conductivity. E. conductivity is defined as the conducting power of all the ions produced by dissolving one mole of an electrolyte in solution. The theory of electrolytic conductivity was pioneered by Debye and Hückel. (a, c) NCERT Exemplar (Objective) Based MCQs Electrochemistry Chemistry Practice questions, MCQs, Past. The protein sample (up to 5–7 mg protein per mL of column) is loaded onto a Mono Q anion exchange column (GE Biosciences) equilibrated in HI-50 m M KCl. Molar conductivity of ionic solution depends on _____. Conductance of electrolyte solution increases with temperature. m 2 . Use this information to estimate the molar solubility of AgCl. Molar conductivity of ionic solution depends on. Thus mathematically, the limiting molar conductivity of [ A_{x}B_{y}] can. compared the charge transport mechanisms between ionic liquids and electrolyte solutions. e. For the given cell, Mg|Mg 2+ || Cu2+ |Cu (i) Mg is cathode (ii) Cu. For example, hydrated Li+ ions are larger than hydrated Cs+ ions. So, molar conductivity of HCl is greater than that of NaCl at a particular. An electrolyte solution conducts electricity because of the movement of ions in the solution (see above). 6 g of a solute is dissolved in 0. Distance between electrodes c. 3 OH − has an anomalously high mobility in aqueous. The electrostatic attraction between an ion and a molecule with a dipole is called an ion-dipole attraction. 66 cm² mol⁻¹. Model Description. 85 S cm 2 mol −1 (11) . 1) (8. 3k points) class-12 Download Google App video_libraryDemo Videos Live Videos Customer Care : 6267349244---- Molar conductivity, also known as molar conductance, is a kind of electrical conductivity. Nature of electrolyte – Strong electrolytes have high conductance whereas the weak electrolytes have low conductance. Label each flask with the corresponding concentration calculated from the prelab. The usual conductivity range for a contacting sensor is 0. Add a fourth drop of 1. the molar conductivity in the limit of zero concentration of the electrolyte). . Molar conductivity Λm (S m 2 mol−1 ) is. Pour a small amount of each solution into the corresponding beaker or vial. You need a function of the form: Conductivity = Ac − Bf(c), Conductivity = A c − B f ( c), where A A and B B are constants, c c is concentration, and f(c) f ( c) is some function of concentration. The conductivity depends on the type. A. B. What will happen during the electrolysis of aqueous solution of CuSO 4 in the presence of Cu electrodes? (i) Copper will deposit at cathode. D surface area of electrodes. M olar conductivity of a solution is the conductance of a volume of solution containing one mole of electrolyte kept between two electrodes with the same unit area of cross-section and same distance between them at a given concentration. 44 g mol , to convert from moles to grams of NaCl : The conductance of a solution depends on 1) the concentration of the ions it contains, 2) on the number of charges carried by each ion, and 3) on the mobilities of these ions. This type of conductance is known as ionic conductance. View in Scopus Google Scholar. (i) 1 l R A (ii) * G R (iii) Λm (iv) l A 26. The ionic transport and the mechanical properties in solids are intimately related. In ionic solutions, however, there are significant electrostatic interactions between solute-solvent as well as solute-solute molecules. Hint:Molar conductivity is defined as the property of solution which contains 1 mole of electrolyte or it is considered as the function of the ionic strength of the solution or the concentration of the salt. 2. Ionic conductivity and transference number. The quantity 1/κ 1 / κ is a measure for the size of this cloud and κ κ is the Debye-length. Text Solution. Surface area of electrodes The correct choice among the given is - 1. It has been found that decrease in kon dilution of a solution is more than compensated by increase in its volume. Concentration of the solution – Molar conductance varies with concentration of the electrolyte. where α is a constant between zero and unity, V m is the molar volumes, ρ is the density, and M is the molar mass. (c, d) 4. Suggest Corrections. Measure the conductivity of the solution. 2) (1. 2 Generalized Langevin Equation in Electrolytic Solution. Molar Conductivity of Selected Ions Ion Molar Conductivity (S L. 2. Define resistance, resistivity, conductance, and conductivity. distance between electrodes. It can also be defined as the ionic strength of a solution or the concentration of salt. Research into the electrical conductivity (σ) of non-aqueous liquids began largely around the turn of the 20th century, following on from studies of ionic conduction in aqueous solutions. 23 atm at 27° C. Surface area of electrodes. Choose the correct answer from the options given below: Specific conductivity passes through a maximum with an increase in the concentration of electrolyte in aqueous solutions (Figure 10 a) and in non-aqueous solutions of ionic liquids (Figure 12 a). 2012) for calculating conductivity of a mixed electrolyte solution from its chemical composition: (3) where is the ionic molar conductivity and mis the speciated molality of the ith ion. The complete set of equations for the calculation of the. The conductivity of an electrolyte solution is related to the strength of the electrolyte. temperature. b) Its conductance decreases with dilution. S. 3 M solution of KCI at 298 K is 3. 9. 4, Fig. Semiconductors: band structure determines the number of charge carriers. B. Ionic conductivity (σ) was measured using a CRISON GLP31 conductivity meter, which employs an ac voltage of 500 Hz and 0. 51 mol −1/2 dm 3/2 and B = 3. 1 M NaCl (b) 0. 6. >. You need to add the limiting ionic conductivities for HX+ H X + and OHX− O H X − together to get the limiting ionic conductivity for all the ions in solution ( Λ0 Λ 0, which will replace Λ0m Λ m 0 in your equation). Solutions prepared from potassium chloride in 30 %This will make the solution conductive in its own manner. 2) and to some ex-The specific electrical conductivity of SrCl 2, CaF 2, SrF 2, and BaF 2 in the crystalline and molten states is shown in Fig. This feature is associated with the mass transition caused by the viscosity and conductivity of the solvent, which depends on temperature. The molar conductivity of cation and anion of salt B A are 1 8 0 and 2 2 0. 1 EC = 1 µS/cm = 1 x 10 – 6 S/m. Solution For Molar conductivity of ionic solution depends on: On increasing the temperature, molar conductivity increases whereas molar conductivity decreases on increasing the concentration. Molar Conductivity of Selected Ions -Ion Molar Conductivity (S L. ionic species to water increases its ability to conduct considerably. 20M. the molar conductivity of the solution will be asked Dec 5, 2019 in Chemistry by Riteshsingh ( 90. temperature. This value of A depends on the charges on both cation and anion obtained on the dissociation of an electrolyte in a solution. Given: Molarity (M) = 0. Molar conductivity of ionic solution depends on: (i) temperature. Variation of Molar Conductivity with Concentration. The second equation has a "special name",. This feature is associated with the mass transition caused by the viscosity and conductivity of the solvent, which depends on temperature. molar conductivity is a valuable quantity to construct linear relationship with the transport properties. Molar conductivity is a feature of an electrolyte solution that is primarily used to determine an electrolyte's efficiency in conducting. 16. The specific conductance of a solution containing one electrolyte depends on the concentration of the electrolyte. The increase. 08 and 23. 05 M NaCl (c) 0. 5 ohm. Hard. The conductivity of electrolytic (ionic) solutions depends on: i) the nature of the electrolyte added ii) size of the ions produced and their solvation iii) the nature of the solvent and its viscosity iv) concentration of the. To study the Ds. Ionic contributions of ions can be evaluated from the limiting molar conductivities of strong electrolytes containing the same ions. More From Chapter. Solution: The molar conductivity can be calculated by for mula, c 7. 23 atm at 27° C. It is because k is the conducting power of all the ions present per cm 3 of the solution. (ii) Copper will dissolve at anode.