ZuoTi.Pro
Question

A student performs the titration of 25.0 mL of HCI with 0.1 M NaoH. If the acid concentration is 0.1 M and 35.0 mL of base are added, the hydroxide concentration and the pH are: O a) [oH-1 1.67 x 102 M, pH 12.22 O b) [oH-1 3.5 M, pH 13.46 1.78 O d) [oH-1- 2.58 x 10 M, pH 13.51 Save Question 15 (5 points) The pH at the equivalence point when a o.20 M weak base (Ka 9.1 x 10 is titrated with a 0.20 M strong add is:
science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

2 ㄣ

0 0
Add a comment
Know the answer?
Add Answer to:
A student performs the titration of 25.0 mL of HCI with 0.1 M NaOH. If the...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • In the titration of 25.0 mL of 0.1 M CH3COOH with 0.1 M NaOH, how is...

    In the titration of 25.0 mL of 0.1 M CH3COOH with 0.1 M NaOH, how is the pH calculated before the titrant is added? The pH is calculated by determining the concentration of excess hydroxide ions in the solution, subtracting pOH from 14, and taking the negative log of the result. The pH is 14. The pH is 7. The pH is calculated using the H-H equation for a buffer solution, using the ratio of the concentrations of the base...

  • 1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution....

    1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution. What volume of NaOH is required to reach the equivalence point in the titration? a. 25.0 mL b. 50.0 mL c. 1.00 × 10^2 mL d. 1.50 × 10^2 mL 2. Consider the following acid–base titrations: I) 50 mL of 0.1 M HCl is titrated with 0.2 M KOH. II) 50 mL of 0.1 M CH3COOH is titrated with 0.2 M KOH. Which statement...

  • A student performs a titration of 25.0 mL of 0.100 M lactic acid (HC3H5O3), using 0.050...

    A student performs a titration of 25.0 mL of 0.100 M lactic acid (HC3H5O3), using 0.050 M sodium hydroxide (NaOH). The Ka for lactic acid is 1.4 x 10-4. a) (10 points) What is the pH of the solution after the addition of 23.5 mL of sodium hydroxide solution? b) (4 points) How many milliliters of NaOH are required to reach the equivalence point? c) (4 points) Write the chemical reaction that will determine the pH of the solution at...

  • A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate...

    A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate the pH of the solution during the titration if the weak acid concentration is 0.10 M and its Ka = 1.8 x 10-5 and 10.0 mL of base has been added. (Hint: use Henderson-Hasselbach equation). Question options: a) pH= 7.00 b) pH= 5.28 c) pH = 4.56 d) pH= 4.74

  • A student performs a titration in the laboratory. A 20.0 mL sample of 0.080 M HCl...

    A student performs a titration in the laboratory. A 20.0 mL sample of 0.080 M HCl is titrated with 0.10 M NaOH. What would be the pH of the solution after 25.0 mL of the base has been added? __ 13.05 __ 9.80     __ 10.00 __ 12.30

  • 16.36 Consider the titration of 40.0 mL of 0.100 M NaOH with 0.100 M HCI. a)...

    16.36 Consider the titration of 40.0 mL of 0.100 M NaOH with 0.100 M HCI. a) b) c) What is the pH after adding 35.0 mL of acid? What is the pH at the equivalence point? What is the pH after adding 45.0 mL of acid?

  • Consider the titration of a 25.0 -mL sample of 0.110 M HC2H3O2 with 0.120 M NaOH

     Consider the titration of a 25.0 -mL sample of 0.110 M HC2H3O2 with 0.120 M NaOH. Determine each of the following. Part A the initial pH Part B the volume of added base required to reach the equivalence point Part C the pH at 6.00 mL of added base Part D the pH at one-half of the equivalence point Part E the pH at the equivalence point

  • A student performs a titration, titrating 25.00 mL of a weak monoprotic acid, HNO2, with a...

    A student performs a titration, titrating 25.00 mL of a weak monoprotic acid, HNO2, with a 1.821 M solution of NaOH. They collect data, plot a titration curve and determine that the equivalence point was reached after the addition of 24.64 mL of the base. What is concentration of NO2 at equivalence point (in M)? (give your answer to three decimal places)

  • What is the shape of the titration curve (plot of pH vs. mL of added base)...

    What is the shape of the titration curve (plot of pH vs. mL of added base) for titration of a weak acid by a strong base? In a titration, 10 mL of 0.10 M HF was titrated with 0.20 M KOH. Calculate the pH of the resulting solution after the addition of the following volumes of base: 0 mL, 2.5 mL, 5.0 mL, and 6.0mL. What volume of base is needed to reach the equivalence point? What species is present...

  • 3) (10 points total) A 25.0-mL sample of 0.35 M HCOOH (formic acid) is titrated with...

    3) (10 points total) A 25.0-mL sample of 0.35 M HCOOH (formic acid) is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ka-1.77 x 10 a) (4 points) What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ks-1.77 x 10 C 2-l04Co1s5 b) (6 points) Calculate at least nine (9) more titration points, build a table...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT