Question

if 38.03 ml of 0.08289 M hydrochloric acid requires 21.33 ml of the NaOH solution to...

if 38.03 ml of 0.08289 M hydrochloric acid requires 21.33 ml of the NaOH solution to reach the endpoint, what is the molarity of the NaOH solution?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Balanced acid base neutrilisation reaction is

HCl + NaOH    NaCl + H2O

no. of mole = molarity X volume of solution in liter

28.03 ml = 0.02803 liter

no. of mole of HCl = 0.08289 X 0.02803 = 0.0023234 mole

According to balanced reaction 1 mole HCl required 1 mole of NaOH therefore to neutrilize 0.0023234 mole of HCl required NaOH = 0.0023234 mole of NaOH

molarity = no. of mole/volume of solution in liter

21.33 ml = 0.02133 liter

molarity of NaOH = 0.0023234/0.02133 = 0.1089 M

Molarity of NaOH = 0.1089 M

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
if 9.76 mL of an acetic Acid solution required 9.80 mL of 1.0962 M NaOH to...
if 9.76 mL of an acetic Acid solution required 9.80 mL of 1.0962 M NaOH to reach the endpoint, whats the concentration of the Acetic Avid Solution?
if 10.57 mL of an acetic Acid solution required 10.54 mL 0.9607 M NaOH to reach...
if 10.57 mL of an acetic Acid solution required 10.54 mL 0.9607 M NaOH to reach the endpoint, whats the concentration?
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH....
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH. To reach the endpoint of the titration, 30.00 mL of NaOH solution is required. Ka = 1.8 x 10-4 What is the concentration of formic acid in the original solution? What is the pH of the formic acid solution before the titration begins (before the addition of any NaOH)?
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH....
A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH. To reach the endpoint of the titration, 30.00 mL of NaOH solution is required. Ka = 1.8 x 10-4 What is the pH of the solution after the addition of 10.00 mL of NaOH solution? What is the pH at the midpoint of the titration? What is the pH at the equivalence point?
59.2 mL of 1.98 M hydrochloric acid is added to 38.2 mL of barium hydroxide, and...
59.2 mL of 1.98 M hydrochloric acid is added to 38.2 mL of barium hydroxide, and the resulting solution is found to be acidic. 16.5 mL of 5.53 M potassium hydroxide is required to reach neutrality. What is the molarity of the original barium hydroxide solution?
10.00mL of a sample of concentrated hydrochloric acid is diluted to 100.00mL. If a 20.00 mL...
10.00mL of a sample of concentrated hydrochloric acid is diluted to 100.00mL. If a 20.00 mL portion of this diluted acid required 15.23mL of 1.5 M NaOH to reach the endpoint, what is the concentration of the original, undiluted HCl?
A NaOH solution is standardized using KHP and the molarity of the NaOH solution is determined...
A NaOH solution is standardized using KHP and the molarity of the NaOH solution is determined to be 0.4150 M. Since the acid in vinegar is the monoprotic acid, acetic acid, the concentration of the acetic acid can easily be determined by titration. If 90.72 mL of this solution is required to titrate 10.32 mL of vinegar to the Phenolphthalein endpoint, what is the concentration of acetic acid in the vinegar? _______________ M 95.71 mL of NaOH solution is required...
A 25.0 mL aliquot of concentated hydrochloric acid (11.7 M) is added to 175.00 mL of...
A 25.0 mL aliquot of concentated hydrochloric acid (11.7 M) is added to 175.00 mL of 3.25 M hydrochloric acid. (a) Is this a dilution? (b)Determine the number of moles of hydrochloric acid from the 175.00 mL of 3.25 M hydrochloric acid. (c) Determine the number of moles of hydrochlocic acid in the solution after the addition of the concentrated hydrochloric acid. Asume the volumes are additive. (d) Detemine the molarity of the solution after the addition of the concentrated...
Consider the titration of H3C6H5O7 with NaOH. If it requires 0.00343 mol of NaOH to reach...
Consider the titration of H3C6H5O7 with NaOH. If it requires 0.00343 mol of NaOH to reach the endpoint, and if we had originally placed 16.41 mL of H3C6H5O7 in the Erlenmeyer flask to be analyzed, what is the molarity of the original H3C6H5O7 solution?
titration of a 12mL solution of HCl requires 22.4 mL of .12 M NaOH? what is...
titration of a 12mL solution of HCl requires 22.4 mL of .12 M NaOH? what is the molarity of the HCl solution?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT