when the ionic solute MgCl2 is dissolved in water, what can you say about the number of chloride ions present in the solution compared to the number of magnesium ions in the solution?

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opn04125Lv3

14 Feb 2023

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Nestor RutherfordLv2

26 Mar 2019

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Dibasic calcium phosphate (CaHPO4) has limited solubility in water with solubility product of Ksp= 7.23*10^-7. Taking into account ionic interactions, what will be the concentration of Ca2+ ions in the solution saturated with CaHPO4 after 2.5*10^-3 m magnesium chloride (MgCl2) is dissolved in the same solution.

There are 2 beakers, one with MgCl2 dissolved in water and onewith NaCl dissolved in water. There is 1.0 L solutions of 1.0 MNaCl(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 youarrive at this answer?

What is the concentration of chloride ions in each beaker?

e. Explain how it is that the concentrations of chloride ions inthese beakers are different even though the concentrations of eachsubstance(compound) are the same.

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

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

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

c. Explain why the concentration of MgCl2 (aq) would change,whereas the number of moles of MgCl2 would change when solution wasremoved from the beaker.As part of your answer, you are encouragedto 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 withthe addition of water, whereas the number of moles does notchange.you are encouraged to use pictures to help answer thequestion.

Please explain how you came up with the answers.