Question

Q1:  You have 21.7 mL of a 0.9 M solution of A. How many moles of A...

Q1:  You have 21.7 mL of a 0.9 M solution of A. How many moles of A do you have?

Q2: In a titration experiment, 9.3 mL of an aqueous HCl solution was titrated with 0.4 M NaOH solution. The equivalence point in the titration was reached when 9.5 mL of the NaOH solution was added. What is the molarity of the HCl solution?

Q3: In the titration of HCl with NaOH, the equivalence point is determined
a. from the point where the pink phenolphthalein turns colorless and then remains colorless on swirling.
b. from the point where the phenolphthalein turns pink and then remains pink on swirling.
c. from the point where the pink phenolphthalein first turns colorless and then the pink reappears on swirling.
d. from the point where the colorless phenolphthalein first turns pink and then disappears on swirling

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
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
1. 20.00 mL of 0.510 M NaOH is titrated with 0.740 M H2SO4. ______ 1 mL...
1. 20.00 mL of 0.510 M NaOH is titrated with 0.740 M H2SO4. ______ 1 mL of H2SO4 are needed to reach the end point. 2.  If 35.00 mL of 0.0200 M aqueous HCl is required to titrate 30.00 mL of an aqueous solution of NaOH to the equivalence point, the molarity of the NaOH solution is ________ 1 M.
You determine the concentration of a solution of HCl by titration with NaOH. The titration reaction...
You determine the concentration of a solution of HCl by titration with NaOH. The titration reaction is: HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq) Using a volumetric pipet, you transfer 10.00 mL of the HCl solution into an Erlenmeyer flask, then dilute it with ~50 mL of water and add 3 drops of phenolphthalein. The endpoint is reached after you have added 44.00 mL of 0.1250 M NaOH solution from a buret. Calculate the molarity of the original HCl solution....
Bob Cat is attempting to determine the molarity of an unknown solution of acetic acid. He...
Bob Cat is attempting to determine the molarity of an unknown solution of acetic acid. He began by mixing an aqueous NaOH solution and standardizing it by titration of KHP with phenolphthalein indicator. He then titrated the acetic acid solution with his standardized NaOH. The data from one of Bob’s trials is below, but he still needs to complete his calculations. The molar mass of KHP is 204.2 g. Titration of KHP Titration of Acetic Acid mass of KHP (g)...
Consider the titration of 30.00 mL of an HCl solution with an unknown molarity. The volume...
Consider the titration of 30.00 mL of an HCl solution with an unknown molarity. The volume of 0.1200 M NaOH required to reach the equivalence point was 42.50 mL. a. Write the balanced chemical equation for the neutralization reaction. b. Calculate the molarity of the acid. c. What is the pH of the HCl solution before any NaOH is added? d. What is the pH of the analysis solution after exactly 42.25 mL of NaOH is added? e. What is...
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq) 4.00 mL of an unknown...
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq) 4.00 mL of an unknown acid solution containing HCl was added to flask containing 30.00 mL of deionized water and two drops of an indicator. The solution was mixed and then titrated with NaOH until the end point was reached. Use the following titration data to determine the mass percent of HCl in the acid solution. Mass of flask: 125.59 g Mass of flask + acid solution: 129.50 g...
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?
A student dissolves 0.326 g of a powdered antacid in 32.36 mL of 0.1034 M HCl....
A student dissolves 0.326 g of a powdered antacid in 32.36 mL of 0.1034 M HCl. The student boils the mixture and then allows it to cool. Lastly, the student adds phenolphthalein indicator to the mixture. Suppose 11.72 mL of 0.1506 M NaOH is required to turn the solution from colorless to pale pink. Calculate the total moles of OH- added.
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 =
A 44.9 mL sample of a 0.350 M solution of NaCN is titrated by 0.260 M...
A 44.9 mL sample of a 0.350 M solution of NaCN is titrated by 0.260 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 48.4 mL of 0.260 M HCl pH = (c) at the equivalence point pH = (d) after the addition of 76.2 mL of 0.260 M HCl. pH =
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT