Question

In: Chemistry

0.1 M HCl is a stong-conductor and 0.1 M HC2H3O2 is a weak-conductor. Explain the difference...

0.1 M HCl is a stong-conductor and 0.1 M HC2H3O2 is a weak-conductor. Explain the difference in conductivity between 0.1 M HCl and 0.1 M HC2H3O2. Relate the difference to the terms strong acid and weak acid.

Solutions

Expert Solution

HCl is a strong acid whereas CH3COOH (HC2H3O2) is a weak acid.
All strong acids are strong electrolytes which means they completely dissociate to corresponding ions at all dilutions or concentrations. Weak acids are weak electrolytes which means they do not dissociate completely and form a dynamic equilibrium between undissociated molecules and dissociated ions.

We know the conductance of solution depends directly on number of ions in the solution and velocity of the ions. Since strong electrolytes (HCl) produce more ions than weak electrolytes (CH3COOH), Conductance of 0.1M HCl would be superior to 0.1M CH3COOH.

Do let me know if you have any doubts.  


Related Solutions

What difference in the properties of 0.1 M HCl and 0.1 M acetic acid caused the...
What difference in the properties of 0.1 M HCl and 0.1 M acetic acid caused the pH's of equal volumes of each to differ?
Calculate the pH of 5 mL 0.10 M HC2H3O2 + 5 mL 0.1 M HCl Can...
Calculate the pH of 5 mL 0.10 M HC2H3O2 + 5 mL 0.1 M HCl Can someone please help me with this I have no clue how to work this (step by step) This is due tomorrow please help me tonight, I appreciate the help and will rate!
Which of these has the lower concentration of hydrogen ions: 0.1 M H2SO4, 0.1 M HCl,...
Which of these has the lower concentration of hydrogen ions: 0.1 M H2SO4, 0.1 M HCl, CaCO3, or pure water?
Weak acid with strong base: 25 mL of 0.1 M HCOOH with 0.1 M NaOH (pka...
Weak acid with strong base: 25 mL of 0.1 M HCOOH with 0.1 M NaOH (pka = 3.74) pH after adding following amounts of NaOH 18) 0 mL of NaOH 19) at half equivalence point 20) after adding 25 mL NaOH
what is the new PH of a solution if 10ml of 0.1 M Hcl is added...
what is the new PH of a solution if 10ml of 0.1 M Hcl is added to 150ml of a buffer system that is 0.1M Benzoic acid and 0.1M sodium benzoate ( the Ka of benzoic acid is 6.3X10^-5). Thanks
Add 10 mL of 0.1 M HCl to one liter of a 0.10 M sodium acetate...
Add 10 mL of 0.1 M HCl to one liter of a 0.10 M sodium acetate buffer, pH 6.76 (pKa = 4.76 for acetic acid). Does the pH of the solution change? Determine the effect of the addition of 20.0 mL of 0.100 M HCl?
Consider the titration of 0.100 M HCl, a strong acid, with 0.100 M NH3, a weak...
Consider the titration of 0.100 M HCl, a strong acid, with 0.100 M NH3, a weak base: HCL(aq)+NH3(aq)---NH4+(aq)+H2O(l) Calculate the pH at the following points in the titration when 25.0 mL of 0.0100 M NH3 is titrated with 0.100 M HCL. A. 0.0 mL of HCl added B. 10.0 mL of HCl added C. At equivalence point D. 35.0 mL of HCL added
What is the pH of solution if 40 mL 0.1 M HCl is mixed with 60...
What is the pH of solution if 40 mL 0.1 M HCl is mixed with 60 mL 0.2 M HAc?
A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate...
A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate the pH of the solution during the titration if the weak acid concentration is 0.10 M and its Ka = 1.8 x 10-5 and 10.0 mL of base has been added. (Hint: use Henderson-Hasselbach equation). a) pH = 4.56 b) pH= 5.28 c) pH= 4.74
Carbonic acid, H2CO3, is a weak diprotic acid. In a 0.1 M solution of the acid,...
Carbonic acid, H2CO3, is a weak diprotic acid. In a 0.1 M solution of the acid, which of the following species is present in the largest amount? H2CO3. H3O+ HCO3
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT