Second, you should be able to calculate the amount of solute in (or needed to make) a certain volume of solution. Fourth, you might need to calculate the concentration of a solution made by the dilution of another solution.
In either of the first two cases, the amount of solute might be in moles or grams and the amount of solution might be in liters or milliliters.
There are times when you need to deal with the concentration of chemical species in solution rather than the concentration of a chemical compound.
With weak electrolytes, this issue is complicated by the fact that some of the chemical remains undissociated.
When dealing with the concentrations of chemical species, it is customary to use brackets around the formula of the chemical specie as a symbol for the concentration of that specie.
If we add H2 gas to the container, equilibrium shifts to the right and system decrease the concentration of H2. In an endothermic reaction; increasing temperature shift equilibrium to the right and equilibrium constant increases. In an endothermic reaction; increasing temperature shift equilibrium to the left and equilibrium constant decreases.
To talk about affect of pressure on equilibrium, at least one of the matters must be in gas phase.
If one of the matters in container  under constant temperature and pressure is removed or added, pressure of the system changes.

In gas reactions, if there is no change in number of moles, then pressure do not effect equilibrium. If volumes of them decreased from point I to II, find in which container equilibrium shifts to the right. Sucrose isn't charged, so you don't have to worryabout it messing with your reversal potentials, etc. Please note that with molarity we are concerned with how much solute there is and with how much solution there is, but not with how much solvent there is.
You may want to look through the workbook examples on your own and if they make perfect sense to you, test your understanding by doing exercise 4. So the answer is that you would make the solution by dissolving 28.1 g NaCl in enough water to make 400 ml of solution. If you like the algebraic approach, you would write down the general equation shown in part a, substitute in the known values, solve for moles of NaCl, and then change that into grams. Once you are familiar with how those are done then you should try answering the following questions (exercise 4 in your workbook). For example when HF dissolves in water HF(aq), H+(aq) and F(aq) are all formed and present in the solution. In other words, in a reaction consisting of liquid, aqueous, or solid there is no affect of pressure on equilibrium of this system.
In this situation even if pressure changes, we consider changes in the temperature while finding equilibrium constant.

In this case what you need to find out is how much NaCl would have to be dissolved in 400 ml to give the concentration that is specified. Depending on the conditions under which the solution is formed, the concentration of each of those chemical species might be different. If heat is given to system, according to Le Chatelier's principle system wants to decrease this temperature and equilibrium shift to the left or right. This amount is going to have to be in grams because we don't have any balances that weigh in moles.
I other words, in first situation equilibrium shifts to the right and in second situation equilibrium shifts to the left. It is simply a matter of specifying that the concentration refers to a particular chemical specie rather than a chemical compound.
This could also have been done using algebra by writing down the general equation relating molarity, moles and liters, substituting the known values, and then solving the equation for moles.

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