Question

If you try to prepare a solution containing 0.02 moles/L of benzoic acid (weak acid, pKa...

If you try to prepare a solution containing 0.02 moles/L of benzoic acid (weak acid, pKa 4.2; Mol Wt=122.12) at pH 3 will this solution be clear or turbid. The So of benzoic acid is 0.028 M

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Let us answer this question based on the dissociation of a weak acid like benzoic acid in Acidic pH range. A weak acid means it will not dissociate completely to ions, here it is H+ and COO- ions. If it dissociated incompletely, it will not dissolve completely. So some benzoic acid parts will be formed as turbid (not clear) in the solution. But do some calculations on the given data

number of moles = given mass/ molecular mass

therefore mass of benzoic acid = no of moles x M.M = 0.02 x 122.12 =2.4424 g in 1 litter of the solution.

The amount of dissolved substance is very low compared to the total volume of solution. So it is less chance to form a turbid solution than a clear one

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
In a solution that contains benzoic acid (pKa = 4.2), 16% of the total benzoic acid...
In a solution that contains benzoic acid (pKa = 4.2), 16% of the total benzoic acid occurs as the benzoate anion. What is the pH of this solution? Consider a solution that contains both acetic and benzoic acid. Using the information above, what is the pH of the solution if 95% of the benzoic acid is dissociated? How much acetic acid is dissociated (e.g., is in the form of acetate) at this pH?
1. A 0.0450 M solution of benzoic acid has a pH of 2.71. Calculate pKa for...
1. A 0.0450 M solution of benzoic acid has a pH of 2.71. Calculate pKa for this acid. 2. A 0.0460 M solution of HA is 0.80% dissociated. Calculate pKa for this acid. 3. Consider a reaction mixture containing 100.0 mL of 0.112 M borate buffer at pH = pKa = 9.24. At pH = pKa, we know that [H3BO3] = [H2BO3−] = 0.0560 M. Suppose that a chemical reaction whose pH we wish to control will be generating acid....
a) Calculate the pH and pOH of a solution containing 10-4 mol/L sulfuric acid at 25...
a) Calculate the pH and pOH of a solution containing 10-4 mol/L sulfuric acid at 25 degrees C (Kw = 10-14). b) The pKa of a weak acid, carboxylic acid (CH3COOH), is 4.75. Do you expect the pH of a solution containing 10-4 mol/L carboxylic acid less or greater than 4?
a) A solution was prepared by dissolving 0.02 moles of acetic acid (HOAc; pKa = 4.8)...
a) A solution was prepared by dissolving 0.02 moles of acetic acid (HOAc; pKa = 4.8) in water to give 1 liter of solution. What is the pH? b) To this solution was then added 0.008 moles of concentrated sodium hydroxide (NaOH). What is the new pH? (In this problem, you may ignore changes in volume due to the addition of NaOH). c) An additional 0.012 moles of NaOH is then added. What is the pH?
You need to prepare 100 ml of a ph=4 buffer solution using .100M benzoic acid (pka=4.20)...
You need to prepare 100 ml of a ph=4 buffer solution using .100M benzoic acid (pka=4.20) and .240M sodium benzoate. How much of each solution should be mixed to prepare this buffer? Find ml of benzoic acid and ml of sodium benzoate
A 0.28 −mol sample of a weak acid with an unknown pKa was combined with 12.0...
A 0.28 −mol sample of a weak acid with an unknown pKa was combined with 12.0 mL of 3.00 M KOH and the resulting solution was diluted to 1.500 L. The measured pH of the solution was 3.85. What is the pKa of the weak acid?
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.120 M sodium benzoate. How much of each solution should be mixed to prepare this buffer? ___ ml benzoic acid ___ ml sodium benzoate
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.240 M sodium benzoate. How much Benzoic Acid and Sodium Benzoate should be added in mL?
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.180 M sodium benzoate. How much of each solutionshould be mixed to prepare this buffer? ____ mL of benzoic acid ____ mL sodium benzoate
A buffer contains equal molar concentrations of a weak acid (pKa=4.76) and the salt of the...
A buffer contains equal molar concentrations of a weak acid (pKa=4.76) and the salt of the weak acid and a strong base (Mol Wt= 112.5). The buffer capacity of this solution is 0.33. Calculate the grams/L if the salt in this solution.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT