Question

the pka of HOCL is 7.5. Calculate the pH of a 0.53 m solution of HOCL


the pka of HOCL is 7.5. Calculate the pH of a 0.53 m solution of HOCL

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

The reaction of HOCl as acid :

Acid constant Ka for reaction

Initial concentration of HOCl = 0.53 M

At equilibrium if x moles of acid are dissociating then

At equilibrium concentrations of

acid contant

Acid ionization constant vlue is very small that means a small concentration of HOCl is ionized, leaving the concentration of unionized HOCl concentration (0.53-x) can be considered unchanged. Therefore the equation can be rewrite as:

Therefore the

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
0.1 M solution of weak acid has pH=4.0. Calculate pKa. 20 mL of 0.1 M solution...
0.1 M solution of weak acid has pH=4.0. Calculate pKa. 20 mL of 0.1 M solution of weak acid was mixed with 8 mL 0.1 M solution of NaOH. Measured pH was 5.12. Calculate pKa. Calculate the pH of a 0.2M solution of ammonia. Ka=5.62×10-10. Calculate pH of 0.01 M aniline hydrochloride. Aniline pKb=9.4.
Calculate the pH of a 0.382 M solution of ethylenediamine (H2NCH2CH2NH2). The pKa values for the...
Calculate the pH of a 0.382 M solution of ethylenediamine (H2NCH2CH2NH2). The pKa values for the acidic form of ethylenediamine ( H3NCH2CH2NH3 ) are 6.848 (pKa1) and 9.928 (pKa2). pH= Calculate the concentration of each form of ethylenediamine in this solution at equilibrium. H2NCH2CH2NH2 = H2NCH2CH2NH3+ = H3+NCH2CH2NH3+ =
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....
Calculate the pH of a 0.320 M solution of ethylenediamine (H2NCH2CH2NH2). The pKa values for the...
Calculate the pH of a 0.320 M solution of ethylenediamine (H2NCH2CH2NH2). The pKa values for the acidic form of ethylenediamine ( H3NCH2CH2NH3 ) are 6.848 (pKa1) and 9.928 (pKa2). pH = Calculate the concentration of each form of ethylenediamine in this solution at equilibrium. 1. [ H2NCH2CH2NH2 ] = 2. [ H2NCH2CH2NH3+ ] = 3. [ H3+NCH2CH2NH3+ ] = please be detailed thanks.
a) The pKa of HF is 3.17. Calculate the pH of a 1.00 L solution that...
a) The pKa of HF is 3.17. Calculate the pH of a 1.00 L solution that is 1.00 M HF and 1.50 M NaF. b) What is the pH of this solution after addition of 50.0 mL of 10.0 M HCl?
The pKa of the complex [Cr(H2O)6]Cl3 is 4.2. Calculate the pH of a 0.35 M solution...
The pKa of the complex [Cr(H2O)6]Cl3 is 4.2. Calculate the pH of a 0.35 M solution of the complex ion. You MUST show all workings.
pKa of acetic acid is 4.75. Calculate the pH of a vinegar solution that is 1.5...
pKa of acetic acid is 4.75. Calculate the pH of a vinegar solution that is 1.5 M in acetic acid. SHOW ICE TABLE
What is the equilibrium pH of an initially 4.4 M solution of hypochlorous acid, HOCl, at...
What is the equilibrium pH of an initially 4.4 M solution of hypochlorous acid, HOCl, at 25°C (Ka = )? What is Ka for a weak monoprotic acid if a 0.020 M solution of the acid has a pH of 3.28 at 25°C? 15.0 mL of 0.50 M HCl is added to a 100.0-mL sample of 0.484 M HNO2 (Ka for HNO2 = 4.0 × 10–4). What is the equilibrium concentration of NO2– ions?
6. Calculate the final Equilibrium pH of a buffer that initially contains 6.60*10-4 M HOCl and...
6. Calculate the final Equilibrium pH of a buffer that initially contains 6.60*10-4 M HOCl and 7.50*10-4 M NaOCl. Ka of HOCl= 3.0*10-5
Part B Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2. Express your...
Part B Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2. Express your answer numerically using two decimal places. ph= Part C Calculate the pH of a 0.10 M solution of NaOH. Express your answer numerically using two decimal places. ph= Part D Calculate the pH of a 0.10 M solution of hydrazine, N2H4. Kb for hydrazine is 1.3×10−6. Express your answer numerically using two decimal places. ph= Part E Calculate the pH of a 0.10 M...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT