Question

question 1: For a strong acid with an initial solution concentration of 0.065 M, what do...

question 1: For a strong acid with an initial solution concentration of 0.065 M, what do you think will be the approximate concentration of acid molecules, the hydronium ions, and the conjugate base ions?

Question 2: For a weak acid, why is it not possible to make the same assumptions about the final product and reactant concentrations of a strong acid?

Homework Answers

Answer #1

1]

Strong acid fully dissociates in water

So

HA ---> H+ + A-

0.065 0 0

0 0.065 0.065

Concetration of acid molecules will be zero as the acid exists in ionic form

COncentration of hydronium ions = initial concentration of acid = 0.065 M

Concentration of Conjugate base also equal to concentration of initial acid = 0.065 M

2]

Weak acid doesnt dissociate completely in water

So we cant say how much percent it dissociates in water ..

HA -----------> H+ + A-

0.065 0 0

0.065-x x x

So here dissociation depends on the how much the acid is stronger

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
QUESTION 1 Consider a solution prepared by mixing 10.0 mL of 0.200 M formic acid (HCHO2,...
QUESTION 1 Consider a solution prepared by mixing 10.0 mL of 0.200 M formic acid (HCHO2, pKa = 3.75) and 5.0 mL of 0.100 M NaOH. What is the value of Ka for formic acid? Ka = ___ M QUESTION 2 Before any reaction occurs, what is present in the solution? a) Strong acid + strong base b) Strong acid + weak base c) Weak acid + strong base d) Weak acid + weak base QUESTION 3 Before considering any...
Question: Consider a .045 M solution of benzoic acid (C6H5CO2H) whose Ka value is 6.5 x...
Question: Consider a .045 M solution of benzoic acid (C6H5CO2H) whose Ka value is 6.5 x 10-5. A). write the acid-base reaction equation for this acid with water: B). write the equilibrium expression (Ka) for this reaction: C). Calculate the concentration of benzoic acid, benzoate ion (the conjugate base), and hydronium ion for this solution. D). Calculate the pH of this solution. E). Calculate the concentration of hydroxide ions in this solution.
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...
1. Which solutions are the best conductors of electricity? Why do you think this is? Consider...
1. Which solutions are the best conductors of electricity? Why do you think this is? Consider the concentrations of undissociated acid (HA) or base (MOH or B) molecules versus ions. my answer: The best solutions are Strong Acid and Strong base because when dissolved in water, they separate into ions. Ions are ideal for conduction electricity 2. Again, consider the concentrations of undissociated molecules versus ions for each of your acids and bases. How does this compare to what you...
Classify the solution properties of 1.0 M sulfuric acid. a. Strong electrolyte b. Weak electrolyte c....
Classify the solution properties of 1.0 M sulfuric acid. a. Strong electrolyte b. Weak electrolyte c. Non-electrolyte d. Pure liquid Classify the solution properties of 1.0 M potassium hydroxide. a. Strong electrolyte b. Weak electrolyte c. Non-electrolyte d. Pure liquid Classify the solution properties of 1.0 M ammonia. a. Strong electrolyte b. Weak electrolyte c. Non-electrolyte d. Pure liquid Classify the acid-base properties of 1.0 M acetic acid. a. Strong acid b. Weak acid c. Strong base d. Weak base...
Strong base is dissolved in 645 mL of 0.400 M weak acid (Ka = 4.91 ×...
Strong base is dissolved in 645 mL of 0.400 M weak acid (Ka = 4.91 × 10-5) to make a buffer with a pH of 4.11. Assume that the volume remains constant when the base is added. Calculate the pKa value of the acid and determine the number of moles of acid initially present. When the reaction is complete, what is the concentration ratio of conjugate base to acid? How many moles of strong base were initially added?
Strong base is dissolved in 545 mL of 0.200 M weak acid (Ka = 4.02 ×...
Strong base is dissolved in 545 mL of 0.200 M weak acid (Ka = 4.02 × 10-5) to make a buffer with a pH of 4.11. Assume that the volume remains constant when the base is added. a) Calculate the pKa value of the acid and determine the number of moles of acid initially present. b) When the reaction is complete, what is the concentration ratio of conjugate base to acid? c) How many moles of strong base were initially...
The hydronium ion concentration of an aqueous solution of 0.45 M phenol (a weak acid), C6H5OH,...
The hydronium ion concentration of an aqueous solution of 0.45 M phenol (a weak acid), C6H5OH, is [H3O+] =  M
The common-ion effect and buffer systems A buffer is a mixed solution of a weak acid...
The common-ion effect and buffer systems A buffer is a mixed solution of a weak acid or base, combined with its conjugate. Note that this can be understood essentially as a common-ion problem: The conjugate is a common ion added to an equilibrium system of a weak acid or base. The addition of the conjugate shifts the equilibrium of the system to relieve the stress of the added concentration of the common ion. In a solution consisting of a weak...
A buffer is a mixed solution of a weak acid or base, combined with its conjugate....
A buffer is a mixed solution of a weak acid or base, combined with its conjugate. Note that this can be understood essentially as a common-ion problem: The conjugate is a common ion added to an equilibrium system of a weak acid or base. The addition of the conjugate shifts the equilibrium of the system to relieve the stress of the added concentration of the common ion. In a solution consisting of a weak acid or base, the equilibrium shift...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT