Answer:
The most concentrated one, 6.0 M.
Explanation:
A simple and reliable way to produce a solution of HCl (or anything else, for that matter) is to use a more concentrated solution and dilute it.
In this case the chemist could take a portion of the 6.0 M solution and dilute it by adding water, until the concentration is 3.4 M.
Such a process would not be possible with the 2.0 N (which is the same as 2.0 M for HCl) solution.
Answer:
See below
Step-by-step explanation:
An exothermic reaction tends to occur spontaneously because the products are more stable than the reactants.
Nature tries to get to the lowest energy state.
Answer:

Explanation:
In order to answer this question, we need to be familiar with the law of freezing point depression. The law generally states that mixing our solvent with some particular solute would decrease the freezing point of the solvent.
This may be expressed by the following relationship:

Here:
is the change in the freezing point of the solvent given its initial and final freezing point temperature values;
is the van 't Hoff factor (i = 1 for non-electrolyte solutes and i depends on the number of moles of ions released per mole of ionic salt);
is the freezing point depression constant for the solvent;
is molality of the solute, defined as a ratio between the moles of solute and the mass of solvent (in kilograms).
We're assuming that you meant 1.7-molal solution, then:

Given ethylene glycol, an organic non-electrolyte solute:

The freezing point depression constant:

Initial freezing point of pure water:

Rearrange the equation for the final freezing point and substitute the variables:

Answer:
electric balance, goggles, beaker
Explanation:
I did it and got it right