Question

a 200.0 ml volume of solution contains 3.8*10^-2 M in Al^3+ and 0.29 m in NaF...

a 200.0 ml volume of solution contains 3.8*10^-2 M in Al^3+ and 0.29 m in NaF
A) writeout a chemical equation fir Al^3 ion and F ion forming AlF6^-3


B) write kf equilibrium expression for the reaction a

Homework Answers

Answer #1

A) Al3+ (aq) + 6F-(aq) --> [AlF6]3-(aq)

B) Kc = ([AlF6]3-) / [(Al3+)(F-)6]

Kc is equilibrium expression, Kf is forward reaction expression. Rate = Kf x [AlF6]3-

Kc = Kf / Kr

moles Al3+ = 200 mL x 10-3 L x 3.8 x 10-2 M = 0.0076 moles

moles F- = 200 mL x 10-3 L x 0.29 M = 0.058 moles

0.0076 moles Al3+ reacts with ( 6 x 0.0078 = 0.0468 moles) of F- and gives 0.0468 moles of [AlF6]3- only.

Kc = (0.0468) / (0.0076)(0.0468)6 = 5.86 x 108

Kc = 5.86 x 108

Thank You So Much! Please Rate this answer as you wish.

Know the answer?
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
Similar Questions
In aqueous solution the Al+3 ion forms a complex with six fluoride anions. Write the formation...
In aqueous solution the Al+3 ion forms a complex with six fluoride anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the last step in the formation of the complex.
2.) FeSCN2+ equilibrium concentration was found to be 3.20 x 10-5 M in a solution made...
2.) FeSCN2+ equilibrium concentration was found to be 3.20 x 10-5 M in a solution made by mixing 5.00 mL of 1.00 x 10-3 M Fe(NO3)3 with 5.00 mL of 1.00 x 10-3 M HSCN. The H+ concentration is maintained at 0.500 M at all times since the HSCN and Fe3+ solutions were prepared using 0.500 M HNO3 in place of distilled water. a. How many moles FeSCN2+ are present at equilibrium? b. How many moles each of Fe3+ and...
2. What is the pH and [F–]eq in a 0.100 M solution of HF?      Ans....
2. What is the pH and [F–]eq in a 0.100 M solution of HF?      Ans. pH = 2.08; [F–] = 8.2×10–3 M 3. What would happen to the equilibrium [H3O+] and the pH of the solution if we suddenly added some solid NaF? (Remember, sodium salts are completely soluble in water. How will this change affect the equilibrium system? Which direction will the reaction shift to minimize the disturbance?) If we suddenly added some solid NaF the solution will...
Given that Buffer A contains 200.0 mL 0.050 M HOCl and 400.0 mL 0.030 M NaOCl,...
Given that Buffer A contains 200.0 mL 0.050 M HOCl and 400.0 mL 0.030 M NaOCl, calculate 1. The pH of the buffer solution. 2. The pH of the solution after adding 10.0 mL 0.50 M HCl. 3. The pH of the solution after adding 20.0 mL 0.40 M NaOH
2) A 350.0 −mL buffer solution is 0.140 M in HFand 0.140 M in NaF. What...
2) A 350.0 −mL buffer solution is 0.140 M in HFand 0.140 M in NaF. What mass of NaOH could this buffer neutralize before the pH rises above 4.00? If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOHcould be handled before the pH rises above 4.00? 3) A 5.65 −g sample of a weak acid with Ka=1.3×10−4 was combined with 5.20 mL of 6.10 M NaOH and the...
You mix 5.00 mL of 1.0x10^-5 M AgNO3 with 10.00 mL of 2.00 M NH3 solution...
You mix 5.00 mL of 1.0x10^-5 M AgNO3 with 10.00 mL of 2.00 M NH3 solution resulting in the formation of diamminesiler(I) complex ion, [Ag(NH3)2]. (Assume volumes are additive). a. Write the net-ionic equilibrium equation for the formation of this complex ion. b. Calculate the concentration of the complex ion in the reaction mixture, assuming the reaction goes to completion.
What is the [NO3¯] in 200 mL of 0.350 M Al(NO3)3? What is the [NO3¯] in...
What is the [NO3¯] in 200 mL of 0.350 M Al(NO3)3? What is the [NO3¯] in the above solution after adding 200.0 mL of 0.150 M Ca(NO3)2 please show full solution
when 75.0 ml of .150 m NaCl solution and 75.0mL of a 0.250 M Pub(NO3)2 are...
when 75.0 ml of .150 m NaCl solution and 75.0mL of a 0.250 M Pub(NO3)2 are mixed, a white precipitate forms. a. Identify the precipitate in the reaction. b. write out the balanced molecular equation and net ionic equation for the reaction. c. Calculate the mass (in g) of precipitate formed. d. calculate the concentration s of the remaining ions in solution. (what is the total volume after the solutions are mixed? How many moles of each ion remain in...
A) What volume of 0.150 M HClO4 solution is needed to neutralize 59.00 mL of 8.80×10−2...
A) What volume of 0.150 M HClO4 solution is needed to neutralize 59.00 mL of 8.80×10−2 M NaOH? B) What volume of 0.130 M HCl is needed to neutralize 2.87 g of Mg(OH)2? C) If 26.4 mL of AgNO3 is needed to precipitate all the Cl− ions in a 0.755-mg sample of KCl (forming AgCl), what is the molarity of the AgNO3 solution? D) If 45.8 mL of 0.112 M HCl solution is needed to neutralize a solution of KOH,...
Consider the titration of 30.00 mL of an HCl solution with an unknown molarity. The volume...
Consider the titration of 30.00 mL of an HCl solution with an unknown molarity. The volume of 0.1200 M NaOH required to reach the equivalence point was 42.50 mL. a. Write the balanced chemical equation for the neutralization reaction. b. Calculate the molarity of the acid. c. What is the pH of the HCl solution before any NaOH is added? d. What is the pH of the analysis solution after exactly 42.25 mL of NaOH is added? e. What is...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT