Each response gives a pair of solutions. Which pair of solutions should conduct electrical current equally well?
1. 0.10 M NH3 and 0.10 M NH4Cl
2. 0.10 M NaNO3 and 0.10 M HNO2
3. 0.10 M HBr and 0.10 M HF
4. 0.10 M NaCl and 0.10 M NaClO4
Please help...
I would also would like to know how to solve. Thank You...
Conducting electricity EQUALLY well means both not very well, both not at all, both very well.
So look to see if the pair are non-electrolytes, strong electrolytes, weak electrolytes.
NH3 and NH4Cl. NH3 is a weak base; NH4Cl a salt that ionizes completely so NH3 will conduct weakly and NH4Cl strongly. Not #1.
NaNO3 is ionizes 100% so strong conductor; HNO2 is a weak acid so weak conductor. Not #2.
HBr a strong acid and HF weak acid; therefore not #3
4. NaCl strong electrolyte; NaClO4 strong electrolyte so both will conduct electricity very well. I would pick #4 as the choice.
Well, to determine which pair of solutions conducts electrical current equally well, we need to analyze the nature of the ions in each solution.
1. 0.10 M NH3 and 0.10 M NH4Cl: NH3 is a weak base and NH4Cl is a salt of the weak base NH3 and a strong acid HCl. Since NH4Cl dissociates into NH4+ and Cl- ions, the presence of ions makes it a good conductor.
2. 0.10 M NaNO3 and 0.10 M HNO2: NaNO3 and HNO2 are both salts, but NaNO3 is a strong electrolyte that completely dissociates into Na+ and NO3- ions, while HNO2 is a weak acid that partially dissociates into H+ and NO2- ions. So, NaNO3 would conduct current better due to its higher ion concentration.
3. 0.10 M HBr and 0.10 M HF: HBr is a strong acid and HF is a weak acid. Strong acids completely dissociate into ions, while weak acids partially dissociate. Therefore, HBr would conduct current better.
4. 0.10 M NaCl and 0.10 M NaClO4: Both NaCl and NaClO4 are strong electrolytes that completely dissociate into Na+ and Cl- ions, so both solutions would conduct electricity well.
Based on this analysis, the pair of solutions that would conduct electrical current equally well is 0.10 M NaCl and 0.10 M NaClO4.
To determine which pair of solutions conducts electrical current equally well, we need to consider the strength of the electrolytes present in each solution. The stronger the electrolyte, the higher the conductivity.
The strength of an electrolyte can be determined by looking at the ions it produces when dissolved in water. Generally, strong electrolytes dissociate completely into ions, while weak electrolytes only partially dissociate.
Now let's analyze each pair of solutions and determine their relative conductivity:
1. 0.10 M NH3 (weak base) and 0.10 M NH4Cl (strong acid): NH4Cl dissociates completely into NH4+ and Cl- ions, making it a strong electrolyte. NH3, on the other hand, is a weak base and only partially dissociates. Therefore, this pair of solutions will not conduct electrical current equally well.
2. 0.10 M NaNO3 (strong base) and 0.10 M HNO2 (weak acid): Both NaNO3 and HNO2 are strong electrolytes, as they dissociate completely into their respective ions. Hence, this pair of solutions will conduct electrical current equally well.
3. 0.10 M HBr (strong acid) and 0.10 M HF (weak acid): HBr is a strong acid and will fully dissociate, while HF is a weak acid and will only partially dissociate. So, this pair of solutions will not conduct electrical current equally well.
4. 0.10 M NaCl (strong electrolyte) and 0.10 M NaClO4 (strong electrolyte): Both NaCl and NaClO4 are strong electrolytes that dissociate completely into ions. Therefore, this pair of solutions will conduct electrical current equally well.
In conclusion, the pair of solutions that will conduct electrical current equally well is 0.10 M NaNO3 and 0.10 M HNO2 (option 2).