please help I hope this is enough info to complete the proce

please help I hope this is enough info to complete the process the data from my lab is there I just need assistance answering the data under processing data. Thank you very much

DATA TABLE Solution A - CaCl A- AlCls A NaCI B - HC2Ha02 B- HCI B- HaP04 B HaB03 Conductivity (pS/cm) 250A0 I132 C - CH:OH (methanol) PROCESSING THE DATA Based on your conductivity values, do the Group A compounds appear to be molecular, ionic, or mo dissociate, or not dissociate at all? 1. lecular acids? Would you expect them to partially dissociate, completely 2. Why do the Group A compounds, each with the same concentration (0.05 M), have such large differences in conductivity values? Hint: Write an equation for the dissociation of each. Explain NaCI AlCl3 CaCl2 y no tricit

Solution

1. Group A are all ionic with high conductivities

2. Group A compounds give different numer of ions in solution which are responsible for conductivity, like NaCl (Na+ and Cl-), CaCl2 (Ca2+ and 2Cl-), AlCl3 (Al3+ and 3Cl-) ions. So they all have different values for conductivities.

3. The compounds of Group B appears to be ionic.

Group B order of conductivity (decreasing order) : HCl > H3PO4 > HC2H3O2 > H3BO3

HCl : strong electrolyte

H3PO4, HC2H3O2, H3BO3 : weak electrolyte

4. HCl --> H+ + Cl-

H3PO4 <==> H+ + HPO42-

HC2H3O2 <==> H+ + C2H3O2-

H3BO3 <==> H+ + HBO3-

5. The H3PO4 and H3BO3 are both weak electrolytes, therefore 3 for H in these do not result in greater number of ions.

6. Group C compund H2O appears to be ionic, rest all are molecular

A small extent of dissociation would be seen in this case.

7. tap water has other ions present in it, which increases conductivity of water, whereas, distilled water is devoid of any such ions and thus are having lower conductivity.