Question

33. Calculate the pH of a solution that is 1.00 M HF, 2.00 M HCl, and...

33. Calculate the pH of a solution that is 1.00 M HF, 2.00 M HCl, and 1.439 MNaF. (Ka = 7.2 10–4)

3.14

3.30

2.48

2.98

0.25

34. If the solid CuF2 has a solubility of 0.0020 mol/L, what is the value of Ksp?

1.8 x 10-7

4.0 x 10-6

3.2 x 10-8

8.0 x 10-9

none of the above

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

33)

Molarity of HF = 1 M

Molarity of HCl = 2 M

Molarity of NaF = 1.439 M

Ka = 7.2 x 10-4

[F-] = 1.439 -1 = 0.439 M

We have,

pH = -logKa + log[F-]/[HCl] = -log(7.2 x 10-4) + log[0.439]/[2]

= 3.143 – 0.659 = 2.48

34)

CuF2           Cu2+    +    2F-

     x                           x                2x

Ksp = [Cu2+][F-]2 = 4x3 = 4 x (0.0020)3 = 3.2 x 10-8

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
1. What is the pH after 20 ml of 0.1 M KOH is added to 10...
1. What is the pH after 20 ml of 0.1 M KOH is added to 10 ml of 0.2 M HClO? (Ka for HClO = 3.0 x 10-8)? A. 10.2            B. 3.8 C. 13.0            D. 4.3 E. 9.7 32. Calculate the pH of a solution that is 1.00 M HF, 1.00 M HCl, and 1.439 MNaF. (Ka = 7.2 10–4) 3.14 3.30 2.48 2.98 0.25
A 1.00 L buffer solution is composed of 0.250 M HF and 0.250 M NaF. Calculate...
A 1.00 L buffer solution is composed of 0.250 M HF and 0.250 M NaF. Calculate the 13)______ pH of the solution after the addition of 0.150 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4.
What volumes of 0.47 M HF and 0.47 M NaF must be mixed to prepare 1.00...
What volumes of 0.47 M HF and 0.47 M NaF must be mixed to prepare 1.00 L of a solution buffered at pH = 3.28? ka= 7.2 x 10^-4 for HF
33. Use the following standard-state free energy of formation data to calculate the acid-dissociation equilibrium constant...
33. Use the following standard-state free energy of formation data to calculate the acid-dissociation equilibrium constant (Ka) at 25oC: Compound Delta Gf (kJ/mol) HCO2 (aq) -372.3 H+ (aq) 0.00 HCO2- (aq) -351.0 a.   6.3 x 10-5                                                   d.   8.0 x 10-3 b.   3.4 x 10-5                                                   e.   4.0 x 10-5 c.   1.8 x 10-4 34. Use the Ka Table to identify the acid in question #33 at 25oC: Ka Name a 7.2 x 10-4 Nitrous Acid b 6.6 x 10-4 Hydroflouric Acid...
A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate...
A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5x10^-4. Please show how to work out this problem.
a. Calculate the pH of a 0.538 M aqueous solution of hydrofluoric acid (HF, Ka =...
a. Calculate the pH of a 0.538 M aqueous solution of hydrofluoric acid (HF, Ka = 7.2×10-4). b. Calculate the pH of a 0.0242 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).
Calculate the pH of a 1 L solution that contains 1.0 M HCl and 1.5 M...
Calculate the pH of a 1 L solution that contains 1.0 M HCl and 1.5 M CH3COOK. The Ka for CH3COOH is 1.8 x 10-5
A)Calculate the pH of 0.100 L of a buffer solution that is 0.27 M in HF...
A)Calculate the pH of 0.100 L of a buffer solution that is 0.27 M in HF (Ka = 3.5 x 10-4 ) and 0.51 M in NaF?B)What is the pH after adding 0.004 mol of HNO3 to the buffer described in Part A? C)What is the pH after adding 0.004 mol of KOH to the buffer described in Part A?
Find the pH for the following solutions: a) A solution that is 0.115 M in HBr...
Find the pH for the following solutions: a) A solution that is 0.115 M in HBr and 0.130 M in HCHO2 b) A 0.25 M CH3NH3I solution? (Kb = 4.4 x 10-4 M for CH3NH2) c) A 0.0180 M solution of HClO2? (Ka = 1.1 x 10-2 M) d) A 0.0180 M solution of Sr(OH)2 e) A 0.170 M solution of KOCl? (For HOCl, Ka = 3.5 x 10-8 M) f) A solution that is 3.00×10−2M in HI and 9.00×10−3M...
Calculate the pH of a 1 L solution that contains 1.0 M HCl and 1.5 M...
Calculate the pH of a 1 L solution that contains 1.0 M HCl and 1.5 M CH3COOK. The Ka for CH3COOH is 1.8 x 10-5. 9.56                             b) 4.74                         c) 4.44                        d) 0.30                         e) 7.45
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT