Advertisements
Advertisements
प्रश्न
Choose the most correct option.
Two solutions have the ratio of their concentrations 0.4 and ratio of their conductivities 0.216. The ratio of their molar conductivities will be ______.
विकल्प
0.54
11.574
0.0864
1.852
Advertisements
उत्तर
Two solutions have the ratio of their concentrations 0.4 and ratio of their conductivities 0.216. The ratio of their molar conductivities will be 0.54.
Explanation:
Given: `K_1/K_2` = 0.216, `C_1/C_2` = 0.4
As we know
∧m = `K/C xx 100`
`∧_(m_1)/∧_(m_2) = (K_1/C_1 xx 100)/(K_2/C_2 xx 100)`
⇒ `∧_(m_1)/∧_(m_2) = (K_1/K_2)/(C_1/C_2) = 0.216/0.4`
= 0.54
APPEARS IN
संबंधित प्रश्न
What is a cell constant? What are its units? How is it determined experimentally?
Kohlrausch law is applicable for the solution _______.
SI unit of conductivity is _______.
In case of weak electrolyte the graph Λ vs `sqrt"c"` is _______.
Write three important steps required to determine molar conductivity.
Calculate molar conductivities at zero concentration for CaCl2 and NaCl.
Given: molar ionic conductivities of Ca2+, Cl–, Na+ ions are respectively, 104, 76.4, 50.1 Ω–1 cm–2 mol–1
Write relation between electrolytic conductivity and molar conductivity.
Molar conductance of BaCl2, H2SO4 and HCl at infinite dilution are X1, X2 and X3 respectively. Molar conductance of BaSO4 at infinite dilution is ____________.
The conductivity of 0.02 M solution of NaCl is 2.6 × 10−2 S cm−1. What is its molar conductivity?
Which among the following solution has the highest conductivity (k) value?
The molar conductivities at infinite dilution for sodium acetate, HCI and NaCl are 91 S cm2 mol-1, 425.9 S cm2 mol-1 and 126.4 S cm2 mol-1 respectively. The molar conductivity of acetic acid at infinite dilution is ______.
In 2 hours, a certain current liberates 0.504 g hydrogen. How many grams of copper can be deposited by the same current flowing for the same time in a CuSO4 solution?
(Molar mass of Cu = 63.5 g mol−1, H2 = 2.0 g mol−1)
What is the cell constant of `"N"/10 "KCl"` solution at 25°C, if conductivity and resistance of a solution is 0.0112 Ω−1 cm−1 and 55.0 Ω respectively?
The distance between electrodes of a conductivity cell is 0.98 cm and area of cross section is 1.96 cm2. What is the cell constant?
Conductivity of a conductor is ____________.
A conductivity cell dipped in 0.01 M AgNO3 solution gives a resistance of 3160 ohms. If cell constant is 0.47 cm−1, what is the conductivity of AgNO3 solution?
What will be the concentration of NaCl solution, if the molar conductivity and conductivity of NaCl solution is 124.3 Ω-1 cm2 mol-1 and 1.243 × 10-4 Ω-1 cm2 respectively?
What is the conductivity of 0.01 M NaCl solution if resistance and cell constant of NaCl solution are 375 ohms and 0.5 cm-1 respectively at 298 K?
If the resistivity of 0.1 M KCI solution is 50 Ω cm, what is it's molar conductivity?
Specific conductance of 0.1 M sodium chloride solution is 1.06 × 10−2 ohm−1 cm−1. Its molar conductance in ohm−1 cm2 mol−1 is ______.
What is the SI unit of conductivity?
Calculate molar conductivity for 0.5 M BaCl2 if its conductivity at 298K is 0.01 Ω–1 cm–1.
Molar conductivities at infinite dilution of Mg2+ and Br- are 105.8 Ω-1 cm2 mol-1 and 78.2 Ω-1 cm2 mol-1 respectively. Calculate molar conductivity at zero concentration of MgBr2.
Explain the determination of molar conductivity of a weak electrolyte at infinite dilution or zero concentration using Kohlrausch's law.
Define the term cell constant.
Write the relation between molar conductivity and molar ionic conductivities for the electrolytes:
- Na2SO4
- AlCl3
