There are 2 beakers, one with MgCl2 dissolved in water and one with NaCl dissolved in water. There is 1.0 L solutions of 1.0 M NaCl(aq) and 1.0 M MgCl2(aq).

c. How many moles of NaCl and MgCl2 are in each beaker?

d. How many moles of chloride ions in each beaker? How did you arrive at this answer?

What is the concentration of chloride ions in each beaker?

e. Explain how it is that the concentrations of chloride ions in these beakers are different even though the concentrations of each substance(compound) are the same.

Say you were to dump out half of the MgCl2 solution from one beaker.

a. What would be the concentration of the MgCl2(aq) ion and of the chloride ions in the remaining solution?

b. How many moles of the MgCl2 of the chloride ions would remain in the beaker?

c. Explain why the concentration of MgCl2 (aq) would change, whereas the number of moles of MgCl2 would change when solution was removed from the beaker.As part of your answer, you are encouraged to use pictures.

Consider the beaker containing 2.3 L of the 2.1 M NaCl(aq) solution. You now add 1.0 L of water of this beaker.

a. What is the concentration of this NaCl(aq) solution?

b. How many moles of NaCl are present in the 1.0 L of NaCl(aq) solution?

c. Explain why the concentration of NaCl(aq) does change with the addition of water, whereas the number of moles does not change.you are encouraged to use pictures to help answer the question.