Question

1)A 40.0 mL sample of 0.045 M ammonia is titrated with 25.00 mL of 0.080 M...

1)A 40.0 mL sample of 0.045 M ammonia is titrated with 25.00 mL of 0.080 M HCl. If pK_bb​ = 4.76 for ammonia, what is the solution pH?

2)

The single equivalence point in a titration occurs at pH = 5.65. What kind of titration is this?

A

Strong acid titrated with a strong base

B

Weak acid titrated with a strong base

C

Weak base titrated with a strong acid

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
An 80.0 mL sample of 0.200 M ammonia is titrated with 0.100M hydrochloric acid. Kb for...
An 80.0 mL sample of 0.200 M ammonia is titrated with 0.100M hydrochloric acid. Kb for ammonia is 1.8 x 10-5. Calculate the pH of the solution at each of the following points of the titration: a. before the addition of any HCl. ______________ b. halfway to the equivalence point.______________ c. at the equivalence point._________________ d. after the addition of 175 mL of 0.100M HCl.____________
A  25.00-mL  sample of propionic acid,  HC3H5O2,  of unknown concentration A  25.00-mL  sample of propionic acid,  HC3H5O2,  of unknown concentration  was titrated w
A  25.00-mL  sample of propionic acid,  HC3H5O2,  of unknown concentration A  25.00-mL  sample of propionic acid,  HC3H5O2,  of unknown concentration  was titrated with  0.151  M  KOH. The equivalence point was reached when was titrated with  0.151  M  KOH. The equivalence point was reached when  41.28  mL  of base had been added. What is the pH at the equivalence point?    41.28  mL  of base had been added. What is the pH at the equivalence point?     Ka   for propionic acid is    1.3×10–5   at  25°C.Ka   for propionic acid is    1.3×10–5   at  25°C. Select one: a. 8.93 b. 7.65 c. 9.47 d. 5.98 e. 9.11
1. When 50.00 mL of 0.100 M NaOH reacts with 25.00 mL of 0.300 M HX,...
1. When 50.00 mL of 0.100 M NaOH reacts with 25.00 mL of 0.300 M HX, a weak monoprotic acid, the pH of the resulting solution is 3.74. Calculate the Ka of the acid. 2. Will the equivalence point of ammonia plus HCl be higher, lower, or equal to 7? Explain.
In the titration of a 25.00 mL of 0.245 M weak base (Kb= 1.0 *10^-4) being...
In the titration of a 25.00 mL of 0.245 M weak base (Kb= 1.0 *10^-4) being titrated by 0.365 M HCl determine the pH at equivalence point and the pH after 22.4 mL of HCl has been reached. Please explain! I'm having a hard time with these type of questions.
1) If 25.2 mL of 0.109 M acid with a pKa of 5.55 is titrated with...
1) If 25.2 mL of 0.109 M acid with a pKa of 5.55 is titrated with 0.102 M NaOH solution, what is the pH of the titration mixture after 13.7 mL of base solution is added? 2) If 28.8 mL of 0.108 M acid with a pKa 4.15 is titrated with 0.108 M NaOH solution, what is the pH of the acid solution before any base solution is added? 3)If 27.9 mL of 0.107 M acid with a pKa of...
A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the...
A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the pH after the addition of the following volumes of acid. a) 0.0 mL b) 15.0 mL c) At the equivalence point d) 40.0 mL
A student titrated a 25.00 mL sample of a solution containing an unknown weak, diprotic acid...
A student titrated a 25.00 mL sample of a solution containing an unknown weak, diprotic acid (H2A) with NaOH. If the titration required 17.73 mL of .1036 M NaOH to completely neutralize the acid, calculate the concentration (in M) of the weak acid in the sample.
When 0.100 M NaOH is titrated with 25.00 mL 0.0500 M HBr, which of the following...
When 0.100 M NaOH is titrated with 25.00 mL 0.0500 M HBr, which of the following is correct for this titration? A. Initially the pH will be less than 1.00. B. The pH at the equivalence point will be 7.00. C. It will require 12.50 mL of NaOH to reach the equivalence point. When 0.100 M NaOH is titrated with 25.00 mL 0.0500 M HBr, which of the following is correct for this titration? A. Initially the pH will be...
1) A 16.8 mL sample of a 0.489 M aqueous acetic acid solution is titrated with...
1) A 16.8 mL sample of a 0.489 M aqueous acetic acid solution is titrated with a 0.376 M aqueous sodium hydroxide solution. What is the pH at the start of the titration, before any sodium hydroxide has been added? pH - ___ 2) What is the pH at the equivalence point in the titration of of a 29.5 mL sample of a 0.460 M aqueous hydroflouric acid solution with a 0.358 M aqueous sodium hydroxide solution? pH - ___
A 46.3 mL sample of a 0.380 M solution of NaCN is titrated by 0.350 M...
A 46.3 mL sample of a 0.380 M solution of NaCN is titrated by 0.350 M HCl. Kb for CN- is 2.0×10-5. Calculate the pH of the solution: (a) prior to the start of the titration pH = (b) after the addition of 25.1 mL of 0.350 M HCl pH = (c) at the equivalence point pH = (d) after the addition of 71.9 mL of 0.350 M HCl. pH =
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT