Advertisements
Advertisements
Question
The value of [H3O+] in mol lit–1 of 0.001 M acetic acid solution (Ka = 1.8 × 10–5) is ______.
Options
1.34 × 10–1
1.34 × 10–2
1.34 × 10–3
1.34 × 10–4
Advertisements
Solution
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
RELATED QUESTIONS
0.05 M NaOH solution offered a resistance of 31.6 Ω in a conductivity cell at 298 K. If the cell constant of the cell is 0.367 cm-1, calculate the molar conductivity of NaOH solution.
The molar conductivity of 0.05 M BaCl2 solution at 25° C is 223Ω-1 cm2 mol-1. What is its conductivity?
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 ______.
Answer the following:
What is Kohlrausch law of independent migration of ions? How is it useful in obtaining molar conductivity at zero concentration of a weak electrolyte? Explain with an example.
Write three important steps required to determine molar conductivity.
If resistivity of 0.8 M KCI solution is 2.5 × 10-3 Ω cm. Calculate molar conductivity of solution?
The CORRECT unit of molar conductivity is ____________.
For the reaction \[\ce{A -> B}\], the rate increases by a factor of 2.25 when the concentration of A is increased by 1.5. What is the order of the reaction?
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?
The molar conductances at infinite dilution `(∧_0)` for electrolytes B+A− and C+A− are 140 and 120 S cm2 mol−1. The molar conductance at infinite dilution for B+X− is 198 S cm2 mol−1. The `∧_0` (in S cm2 mol−1) of C+X− 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?
Conductivity of KCI solution is 0.0027 Ω−1 m−1 at 25°C. The resistance of the solution is 82.4 Ω. The cell constant is ____________ m−1.
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 ____________.
The SI unit of resistivity and molar conductivity are respectively ____________.
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 ______.
The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is 1500 Ω. What is the cell constant if conductivity of 0.001 M KCI solution at 298 K is 0.146 × 10−3 S cm−1?
What is the common unit of conductivity if the dimensions are expressed in centimeter?
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?
What is the unit of electrical conductance?
If the resistivity of 0.1 M KCI solution is 50 Ω cm, what is it's molar conductivity?
What is the SI unit of conductivity?
Which of the following has least conductivity in aqueous solution?
Define the term cell constant.
Write the relation between molar conductivity and molar ionic conductivities for the electrolytes:
- Na2SO4
- AlCl3
