Question

a student titrates a 25.00mL aliquot of HCl (concentration unknown) with 33.10mL of 0.1500M NaOH. What...

a student titrates a 25.00mL aliquot of HCl (concentration unknown) with 33.10mL of 0.1500M NaOH. What is the concentration of HCl?

Homework Answers

Answer #1

molarity of NaOH = number of moles of NaOH / volume of solution in L

0.1500 M = number of moles of NaOH / 0.0331 L

number of moles of NaOH = 0.1500 *0.0331 = 0.004965 mole

Balanced equation is

NaOH + HCl -----> NaCl + H2O

from the balanced equation we can say that

1 mole of NaOH requires 1 mole of HCl so

0.004965 mole of NaOH will require 0.004965 mole of HCl

molarity of HCl = number of moles of HCl / volume of solution in L

molarity of HCl = 0.004965 / 0.025 L = 0.199 M

Therefore, the concentration of HCl = 0.199 M

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
Suppose a student titrates a 10.00-mL aliquot of saturated Ca(OH)2 solution to the equivalence point with...
Suppose a student titrates a 10.00-mL aliquot of saturated Ca(OH)2 solution to the equivalence point with 13.70 mL of 0.0234 M HCl. What was the initial [OH − ]?
If 25.62 mL of 1.0 NaOH was needed to titration 30.00 mL HCl at unknown concentration,...
If 25.62 mL of 1.0 NaOH was needed to titration 30.00 mL HCl at unknown concentration, what was the HCl concentration?
A 25 mL aliquot of an HCl solution is titrated with 0.100 M NaOH. The equivalence...
A 25 mL aliquot of an HCl solution is titrated with 0.100 M NaOH. The equivalence point is reached after 21.27 mL of the base were added. Calculate the concentration of the acid in the original solution, the pH of the original HCl solution and the original NaOH solution
Find the Total Alkalinty and Bicarbonate content from these numbers: I pipetted a 25.0mL aliquot of...
Find the Total Alkalinty and Bicarbonate content from these numbers: I pipetted a 25.0mL aliquot of our unknown into a flask, then titrated with standarized HCl which was 0.1011M. We reached a end point and found the total volume dispensed was 5.39mL. I then pipetted a 25.00ml aliquot of the unknown and added 50.00mL of 0.1010M NaOH to it. We titrated the excess NaOH with my standarized 0.1011M HCl solution to the endpoint. I dispensed 50.17mL of HCl to reach...
15.00 of a hydrochloric acid of unknown concentration are mixed with 25.00ml of 0.100M hydrochloric acid....
15.00 of a hydrochloric acid of unknown concentration are mixed with 25.00ml of 0.100M hydrochloric acid. The resulting solution is completely neutralized by 0.254 g of solid strontium hydroxide. What was the concentration of the unknown hydrochloric acid solution. Please show work and explanation. Thank You Appreciate it!
What volume of 0.5 M NaOH is needed to perform the titration of 30 mL of...
What volume of 0.5 M NaOH is needed to perform the titration of 30 mL of 0.1 M H3PO4? Question options: a) V = 12 mL b) V = 6 mL c) V = 18 mL d) V = 30 mL he pH at the equivalence point when a 0.20 M weak base (Ka = 9.1 x 10-7) is titrated with a 0.20 M strong acid is: Question options: a) pH = 2.9 b) pH = 1.7 c) pH =...
Suppose a student adds 25.00 mL of 1.041 M HCl to a 1.50 g antacid tablet....
Suppose a student adds 25.00 mL of 1.041 M HCl to a 1.50 g antacid tablet. The student boils and then titrates the resulting solution to the endpoint with 0.4989 M NaOH. The titration requires 21.1 mL NaOH to reach the endpoint. How many moles of HCl were neutralized by the NaOH?How many moles of HCl were neutralized by the tablet?
Concentration of NaOH = 1.1M Volume of NaOH = 45mL Concentration of HCL = 1.2M volume...
Concentration of NaOH = 1.1M Volume of NaOH = 45mL Concentration of HCL = 1.2M volume of HCL = 45mL final temperature of mixture = 29.1 degrees celsius initial temperature (HCL and NaOH) = 21.9 degrees celsius mass of final mixture (assume density of mizture is 1.00g/mol) = 90.0g specific heat capacity for H20 = 4.18J/g/degree celsius 1) calculate qwater, qcalorimeter and qreaction 2) calculate the number of mols reacted of the limiting reagent
An analytical chemist weighs out 0.223g of an unknown triprotic acid into a 250mL volumetric flask...
An analytical chemist weighs out 0.223g of an unknown triprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1500M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 45.5mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.
1.) A student titrated 25.0mL of a buffer with 0.126 M HCL. What is the concentration...
1.) A student titrated 25.0mL of a buffer with 0.126 M HCL. What is the concentration of the weak base in the buffer? Document your logic(do not use M1V1=M2V2) http://i1190.photobucket.com/albums/z451/chemistrypictures/chart1.jpg 2.) The student then titrated 25.0 mL of the same buffer with 0.115M NaOH. The observed titration curve is shown below. What is the concentration of the weak acid in the buffer? http://s1190.photobucket.com/user/chemistrypictures/media/graph1.jpg.html 3.) What is the buffer strength? 4.) If the pH of the buffe (before it is titrated)...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT