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23 Nov 2019

Here is another solutions problem. Please privide step bystepdescriptions of how to solve this problem.

Mixing 40 mL of a 4.00 M sodium chloride solution with 20 mL ofa5.00 M calcium cloride solution results in a solution withachloride ion concentration of:

(the answer is 6 M, I just have no idea how to work withsolutionsbased on our professor's description).

Thank you!

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Jarrod RobelLv2

8 Aug 2019

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If volumes are additive and 80.0 mL of .40 M sodium chloride ismixed with 120 mL of a calcium chloride solution to give a newsolution in which [Cl^-1] is .52 M, what is the concentration ofthe calcium chloride used to make the new solution?

I know the answer is .30 M, but I don't know how to get to thatanswer. Please explain, thanks! :)

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B. Solid potassium fluoride is slowly added to 50.0 mL of a 0.0386M calcium nitrate solution. The concentration of fluoride ionrequired to just initiate precipitation is...

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Please work out both problems of parts A and B. I don't have atextbook and I really need to see examples.

1) If 8.07 g of CuNO3 is dissolved in water to make a 0.760 M solution, what is the volume of the solution?

2) Which of the following aqueous solutions will have a chloride concentration different from the others? 3.0 M NaCl 0.15 M BaCl2 0.30 M KCl 0.10 M FeCl3 0.20 M MgCl2

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4) Write the balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous NaI. Include phases. What mass of precipitate will form if 1.50 L of highly concentrated Pb(ClO3)2 is mixed with 0.300 L of 0.110 M NaI? Assume the reaction goes to completion.

5) Write the balanced neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional. 0.450 L of 0.440 M H2SO4 is mixed with 0.400 L of 0.200 M KOH. What concentration of sulfuric acid remains after neutralization?

6) A 150.0 mL solution of 3.353 M strontium nitrate is mixed with 210.0 mL of a 3.569 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a zero for the concentration.

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