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13 Dec 2019

1)When 1.50 mole of CaCl2 dissolved in water, how many moles of ions are produced? (Show work)

2)Which of the following aqueous solutions would be the best conductor of electricity? (Pick one) Explain why..

Na3PO4 KCL C6H1206 MgCl2 AgNo3

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Beverley Smith
Beverley SmithLv2
17 Dec 2019

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Related questions

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. 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.Please explain how you came up with the answers.

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.

Please Explain All answers :)

1: What is the concentration of magnesium ions in a 0.250 M MgSO4 solution?

2: Which of the following aqueous solutions will have the highest concentration of chloride ions?

a. 0.10 M NaCl (aq)

b. 0.10 M MgCl2 (aq)

c. 0.10 M AlCl3 (aq)

d. 0.05 M CaCl2 (aq)

e. All of these solutions have the same

concentration of chloride ions.

3: How many grams of potassium permanganate (KMnO4) are needed to prepare 500 mL solution that is 0.2500 molar?

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