Question

17. Calculate the solubility of calcium fluoride in a 0.035 M sodium fluoride solution. Some important...

17. Calculate the solubility of calcium fluoride in a 0.035 M sodium fluoride solution. Some important information is given below: ▪ NaF will ionize completely, and the reaction is: NaF (aq) → Na+ (aq) + F− (aq) ▪ The calcium fluoride equilibrium reaction is: CaF2 (s) → Ca+2 (aq) + 2F−1 (aq) ▪ For CaF2 (s), Ksp is 4.0 × 10−11 ▪ Na+ (aq) is a spectator ion; The F− (aq) is the common ion.

0 0
Add a comment Improve this question Transcribed image text
Answer #1

son: war +:0 0.035 m tatea o not to 0 0 0.035 0.035 [ 100%. Imig a Hon] Now, Cafy (s) = +20 de (pure solid active mass = 1) c

Add a comment
Know the answer?
Add Answer to:
17. Calculate the solubility of calcium fluoride in a 0.035 M sodium fluoride solution. Some important...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • 2. The equilibrium constant for the following reaction is called the "solubility product" of calcium fluoride:...

    2. The equilibrium constant for the following reaction is called the "solubility product" of calcium fluoride: CaF2(s) - Cal(aq) + 2F-(ay) K = Kp = 3.2 x 10-11 (a) Write an expression for the equilibrium constant of this reaction in terms of concentrations. Why do you suppose we call this a solubility product instead of a solubility quotient or ratio? (b) Calculate the equilibrium concentrations of Ca2+ and F if excess solid CaF is placed in water. (c) in which...

  • Calcium fluoride, the main component of the mineral fluorite, dissolves to a slight extent in water....

    Calcium fluoride, the main component of the mineral fluorite, dissolves to a slight extent in water. CaF2 (s) ⇄ Ca2+ (aq) + 2F-(aq) Ksp = [Ca2+][F-]2 Calculate the Ksp value for CaF2 if the calcium ion concentration has been found to be 2.3×10-4 M.

  • 1. Solid calcium fluoride (CaF2) establishes the following equilibrium in solution: CaF2(s) = Ca2+(aq) + 2F-(aq)...

    1. Solid calcium fluoride (CaF2) establishes the following equilibrium in solution: CaF2(s) = Ca2+(aq) + 2F-(aq) Ke = 1.5 x 10-10 A solution initially contains 2.45 g of CaF2. a. In which direction will the reaction move to reach equilibrium? Explain your reasoning b. Calculate the equilibrium concentrations of Ca2+ and F. How much CaF2 (in mg) dissolves in solution? c. Another solution initially contains 2.45 g of CaF2 and 0.0025 M NaF. What are the equilibrium concentrations of Ca2+...

  • Calcium fluoride, CaF2, is an insoluble salt (Ksp = 1.46 x 10-10) that can be formed...

    Calcium fluoride, CaF2, is an insoluble salt (Ksp = 1.46 x 10-10) that can be formed by precipitation by mixing solutions of calcium nitrate and sodium fluoride. Suppose 200.0 mL of a 0.600 M Ca(NO3)2(aq) solution are mixed with 400.0 mL of a 0.0600 M NaF(aq) solution. Will a precipitate form? How much calcium fluoride could form?

  • I need all the help possible on this....thank you so much. I attached two pics...its the...

    I need all the help possible on this....thank you so much. I attached two pics...its the same question. The first picture gives background on the actual questions 2. A geologist found a large deposit of the mineral Fluorite, CaF2, within a pond of stagnant water that is undisturbed by biological activities. This mineral had been leached into the water and had established equilibrium at 25°C for a considerable length of time. The equation for the solvation of Fluorite in water...

  • Learning Goal: To learn how to calculate the solubility from Kspand vice versa. Consider the following equilibrium be...

    Learning Goal: To learn how to calculate the solubility from Kspand vice versa. Consider the following equilibrium between a solid salt and its dissolved form (ions) in a saturated solution: CaF2(s)⇌Ca2+(aq)+2F−(aq) At equilibrium, the ion concentrations remain constant because the rate of dissolution of solid CaF2 equals the rate of the ion crystallization. The equilibrium constant for the dissolution reaction is Ksp=[Ca2+][F−]2 Ksp is called the solubility product and can be determined experimentally by measuring thesolubility, which is the amount...

  • Help please! Show work xercise 14.16 thodynamic 2. The equilibrium constant for the following reaction is called the...

    Help please! Show work xercise 14.16 thodynamic 2. The equilibrium constant for the following reaction is called the fluoride: constant for the following reaction is called the "solubility product of calcium CaF2(s) - Ca2+(aq) + 2F (aq) K = K = 3.2 x 10-11 a write an expression for the equilibrium constant of this reaction in terms of concentrations. why do you suppose we call this a solubility product instead of a solubility quotient or ratio (b) Calculate the equilibrium...

  • < Question 3 of 17 ) Strontium chloride and sodium fluoride react to form strontium fluoride...

    < Question 3 of 17 ) Strontium chloride and sodium fluoride react to form strontium fluoride and sodium chloride, according to the reaction shown. SECI, (aq) + 2 NaF(aq) SF (s) + 2 NaCl(aq) What volume of a 0.310 M NaF solution is required to react completely with 317 mL of a 0.620 M SCI, solution? volume How many moles of SrF, are formed from this reaction? moles of SrF, mol

  • 10 L of a saturated solution of calcium fluoride, CaF2, was evaporated and found to contain...

    10 L of a saturated solution of calcium fluoride, CaF2, was evaporated and found to contain 4.28 millimoles (mmol) fluoride. What is the value of Ksp? CaF2(s) -> <- ca2+ (aq) +2 F- (aq) How did Ksp= [Ca2+] [F-]2 become Ksp= [s] [2s]2= 4s3 Cause I thought it was only Ksp= [s] [s]2 = s3 and why 4.28x10-3 have to devide by 10 and why the [F-] = 4.28 x 10-4 have to eqautes to 2 to have s= 2.14x10-4...

  • A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility...

    A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility of calcium iodate in mol/L? (b) What are the concentrations of Ca2+ and IO3 – ion, respectively, in the saturated solution? (c) Calculate the Ksp value for Ca(IO3)2. Part b ) Silver ion, Ag+ , readily forms complex ion, Ag(S2O3)2 3– , with thiosulfate, S2O3 2– , according to the following equation: Ag+ (aq) + 2S2O3 2– (aq) ⇌ Ag(S2O3)2 3– (aq); Kf =...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT