Advertisements
Advertisements
प्रश्न
The value of [H3O+] in mol lit–1 of 0.001 M acetic acid solution (Ka = 1.8 × 10–5) is ______.
विकल्प
1.34 × 10–1
1.34 × 10–2
1.34 × 10–3
1.34 × 10–4
उत्तर
The value of [H3O+] in mol lit–1 of 0.001 M acetic acid solution (Ka = 1.8 × 10–5) is 1.34 × 10–4.
Explanation:
[H+] or [H3O+] = αc
c = 0.001 M
= 10–3 M
α = `sqrt(K_a/c)` ......[∵ Ka = α2c]
= `sqrt((1.8 xx 10^-5)/10^-3)`
= 1.34 × 10–1
Now [H3O+] = α × c
= 1.34 × 10–1 × 10–3
= 1.34 × 10–4
APPEARS IN
संबंधित प्रश्न
The molar conductivity of 0.05 M BaCl2 solution at 25° C is 223Ω-1 cm2 mol-1. What is its conductivity?
Answer the following in one or two sentences.
Write the relationship between conductivity and molar conductivity and hence unit of molar conductivity.
Answer the following in brief.
Explain the effect of dilution of the solution on conductivity.
Kohlrausch law is applicable for the solution _______.
In case of weak electrolyte the graph Λ vs `sqrt"c"` is _______.
Give SI unit of resistivity.
Write an equation that shows the relationship between molar conductivity and degree of dissociation of weak electrolyte.
Write applications of Kohlrausch’s Law.
Write three important steps required to determine 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 ____________.
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?
A conductivity cell having cell constant 8.76 cm−1, placed in 0.01 M solution of an electrolyte offered a resistance of 1000 ohms. What is the specific conductance of electrolytes?
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 zero concentration for Ca2+ and CaCl2 are 104 and 256.8 Ω−1 cm2 mol−1 respectively. The molar conductivity at zero concentration for Cl− 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)
Which of the following graph represents the variation of `∧` with `sqrt"c"` for acetic acid solution?
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 is the unit of electrical conductance?
A conductivity cell dipped in 0.5 M KCl gives a resistance of 250 ohms. If the conductivity of KC I solution is 6.68 × 10-3 S cm-1, what is the cell constant?
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.
A conductivity cell filled with 0.02 M AgNO3 gives at 25°C resistance of 947 ohms. If the cell constant is 2.3 cm-1, what is the molar conductivity of 0.02 M AgNO3 at 25°C?
What is the SI unit of molar conductivity?
Define cell constant. Give its units.
