Question

50.0mL of 0.10M HNO2 (nitrous acid, Ka= 4.5x10^-4) is titrated with a 0.10M KOH solution. After...

50.0mL of 0.10M HNO2 (nitrous acid, Ka= 4.5x10^-4) is titrated with a 0.10M KOH solution. After 25.00mL of the KOH solution is added, the pH in the titration flask will be

Homework Answers

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
An analytical chemist is titrating 150.0 mL of a 0.5800 M solution of nitrous acid HNO2...
An analytical chemist is titrating 150.0 mL of a 0.5800 M solution of nitrous acid HNO2 with a 0.2800 M solution of KOH. The pKa of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 320.0 mL of the 0.2800 M KOH solution to it.
Calculate the pH of a 0.375 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4)...
Calculate the pH of a 0.375 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH =    [HNO2 ]equilibrium =    M [NO2- ]equilibrium =    M
For the nitrous acid, HNO2, Ka= 4.0 x 10^-4. Calculate the ph of 0.27 M HNO2
For the nitrous acid, HNO2, Ka= 4.0 x 10^-4. Calculate the ph of 0.27 M HNO2
To a 1.00 L buffer solution made of 1.65 M nitrous acid (HNO2) and 1.01M potassium...
To a 1.00 L buffer solution made of 1.65 M nitrous acid (HNO2) and 1.01M potassium nitrite (KNO2) was added 0.625 moles of NaOH (assume no volume change to the solution). What is the final pH of this buffer assuming Ka nitrous acid = 4.00e-4
What is the pH of a 0.0520 M solution of nitrous acid (HNO2)? (Ka = 4.5...
What is the pH of a 0.0520 M solution of nitrous acid (HNO2)? (Ka = 4.5 x 10-4) (Hint: use ICE and solve the quadratic equation) OR something A LOT simple PLEASE Question options: a) pH = 2.34 b) pH = 2.32 c) pH = 2.30 d) pH = 2.36     
Cyanic acid (HOCN) is a weak acid and has Ka = 3.5 × 10–4. The titration...
Cyanic acid (HOCN) is a weak acid and has Ka = 3.5 × 10–4. The titration is begun with 0.0400 moles of HOCN in 1.00 L of solution in an Erlenmeyer flask below a burette holding KOH. Gradually 0.005 M KOH in the burette is added to the acid to titrate it.                                        a) What is the pH after 80 mL of KOH have been added to the solution?                                     b) What is the pH after 100 mL of...
2. The Ka of nitrous acid is 4.5 x 10-4. In a titration 50.0 mL of...
2. The Ka of nitrous acid is 4.5 x 10-4. In a titration 50.0 mL of a 1.00 M solution is titrated with 0.750 M NaOH. Calculate the pH of the solution: a. Before the titration begins. b. When sufficient NaOH has been added to neutralize half of the nitrous acid originally present. c. At the equivalence point. d. When 0.05 mL of NaOH less than that required to reach the equivalence point has been added. e. When 0.05 mL...
1)consider a 1.50 M solution of nitrous acid,HNO2 (ka=6.0*10^-4) what is molarity of H^+? what is...
1)consider a 1.50 M solution of nitrous acid,HNO2 (ka=6.0*10^-4) what is molarity of H^+? what is the PH? 2) indiacte speices if its an acid or base? NH3 +h20 ...> <.... NH4+ +OH C7H502H +c6h5nh2 C75O2^- +C6H5NH3^+
A 100.0 mL sample of 0.20 M HF is titrated with 0.10M KOH. Determine the pH...
A 100.0 mL sample of 0.20 M HF is titrated with 0.10M KOH. Determine the pH of the solution before teh addition of any KOH. The Ka of HF is 3.5x10^-4
Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO2) and 0.178...
Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO2) and 0.178 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT