Question

Sodium fluoride(0.977M) is added dropwise to a solution that contains 0.020M calcium chloride and 0.020M magnesium...

Sodium fluoride(0.977M) is added dropwise to a solution that contains 0.020M calcium chloride and 0.020M magnesium chloride.
a) which compound precipitates first
b) calculate the percentages of the first cation remanining after first precipitation.
c) can calcium and magnesium ions be separated by selective precipitation of their fluoride salts? (Explain)
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Ans (a) Mg-compound will be precipitated first.

Ans (c). MgF and CaF will be formed which further be classified based on its stability. MgF is more stable due to more ionic character and Size similarity. They can be separated by selective precipitation.As both have same concentration, stability factor will come into role. They can be treated in selective solvent to test its stability .Hence, it can be separated.

Ans (b) 0.977-0.5(0.02) = 0.967. As MgCl2 precipitates first,

NaF reacts with half mole of MgCl2. Therefore,

% change after 1st precipitation = 0.967*100/0.997 = 96.99%

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A solution of NaSCN is added dropwise to a solution that is 0.0821 M in Hg22+...
A solution of NaSCN is added dropwise to a solution that is 0.0821 M in Hg22+ and 0.0142 M in Cu+. The Ksp of Hg2(SCN)2 is 3.2e-20. The Ksp of CuSCN is 1.77e-13. (a) What concentration of SCN- is necessary to begin precipitation? (Neglect volume changes.) (b) Which cation precipitates first? Hg2 2+ or Cu+ (c) What is the concentration of SCN- when the second cation begins to precipitate?
A solution of NaF is added dropwise to a solution that is 0.0532 M in Mg2+...
A solution of NaF is added dropwise to a solution that is 0.0532 M in Mg2+ and 1.43e-05 M in Y3+. The Ksp of MgF2 is 5.16e-11. The Ksp of YF3 is 8.62e-21. (a) What concentration of F- is necessary to begin precipitation? (Neglect volume changes.) [F-] =  M. (b) Which cation precipitates first? Mg2+Y3+      (c) What is the concentration of F- when the second cation begins to precipitate? [F-] =  M.
A solution of Na3PO4 is added dropwise to a solution that is 0.0219 M in Ca2+...
A solution of Na3PO4 is added dropwise to a solution that is 0.0219 M in Ca2+ and 7.03e-06 M in Al3+. The Ksp of Ca3(PO4)2 is 2.07e-33. The Ksp of AlPO4 is 9.84e-21. (a) What concentration of PO43- is necessary to begin precipitation? (Neglect volume changes.) [PO43-] = ___________ M. (b) Which cation precipitates first? Ca2+ Al3+     (c) What is the concentration of PO43- when the second cation begins to precipitate? [PO43-] = _____________ M.
A solution contains 5.84×10-3 M potassium fluoride and 5.84×10-3 M ammonium carbonate. Solid magnesium nitrate is...
A solution contains 5.84×10-3 M potassium fluoride and 5.84×10-3 M ammonium carbonate. Solid magnesium nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of magnesium ion when this precipitation first begins? [Mg2+] =  M
An aqueous solution of sodium fluoride is slowly added to a water sample that contains barium...
An aqueous solution of sodium fluoride is slowly added to a water sample that contains barium ion (4.15×10-2 M ) and calcium ion (3.55×10-2 M ). The Ksp of barium fluoride is 1.00x10–6. The Ksp of calcium fluoride is 3.90x10–11. What is the remaining concentration of the first ion to precipitate when the second ion begins to precipitate?
Barium and Calcium ions in aqueous solutions can be separated by the differences in their solubilizes...
Barium and Calcium ions in aqueous solutions can be separated by the differences in their solubilizes as fluoride salts( Baf2, Ksp=1.8E-7 and CaF2, ksp=5.3E-11. a) which salt precipitates first when slowly adding fluoride ion to a solution that is .1 M In both Ba and Ca? Explain. b) wat concentration of fluoride ion will precipitate the maximum amount of the first salt from the solution described in "part a" while not precipitating the second? Explain.
A solution contains 1.22×10-2 M barium nitrate and 9.39×10-3 M calcium acetate. Solid sodium sulfite is...
A solution contains 1.22×10-2 M barium nitrate and 9.39×10-3 M calcium acetate. Solid sodium sulfite is added slowly to this mixture.What is the formula of the substance that precipitates first?What is the concentration of sulfite ion when this precipitation first begins?
An aqueous solution of barium nitrate is added dropwise to a solution containing 0.10 M sulfate...
An aqueous solution of barium nitrate is added dropwise to a solution containing 0.10 M sulfate ions and 0.10 M fluoride ions. The Ksp value for barium sulfate = 1.1 x 10-10 and the Ksp value for barium fluoride = 1.7 x 10-6 a.) Which salt will precipitate from solution first? b.) What is the minimum [Ba2+] concentration necessary to precipitate the first salt? c.) What is the minimum [Ba2+] concentration necessary to precipitate the second salt? c.) What is...
Hard water often contains dissolved Ca2+ and Mg2+ ions. One way to soften water is to...
Hard water often contains dissolved Ca2+ and Mg2+ ions. One way to soften water is to add phosphates. The phosphate ion forms insoluble precipitates with calcium and magnesium ions, removing them from solution. Suppose that a solution is 0.054 M in calcium chloride and 0.076 M in magnesium nitrate. What mass of sodium phosphate would have to be added to 1.8 L of this solution to completely eliminate the hard water ions? Assume complete reaction.
2. Sodium chloride, potassium chloride, and calcium chloride are all used to de-ice streets. given equal...
2. Sodium chloride, potassium chloride, and calcium chloride are all used to de-ice streets. given equal concentrations of each, which de-ices streets best? Explain why. 3. The freezing point of water decreases as salt is added until it reaches the limit of sodium chloride solubility at -21.0 C. What is the molality of the solution at this temperature?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT