Question

Gravimetrics Lab Question You have 20 mL of 0.0825 M Cl-. You are titrating 0.1 M...

Gravimetrics Lab Question

You have 20 mL of 0.0825 M Cl-. You are titrating 0.1 M AgNO3 into the solution. What is the pAg when you add 10 mL of AgNO3 solution?

What is the pAg at the equivalence point given that Qip=Ksp and Ksp is 1.8 x 10-10?

0 0
Add a comment Improve this question Transcribed image text
Answer #1

13S xUsS

Add a comment
Know the answer?
Add Answer to:
Gravimetrics Lab Question You have 20 mL of 0.0825 M Cl-. You are titrating 0.1 M...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • A) Assume that you are titrating 60.0 mL of 0.0500 M ammonia (Kb = 1.8 ×...

    A) Assume that you are titrating 60.0 mL of 0.0500 M ammonia (Kb = 1.8 × 10–5) with 0.100 M hydrochloric acid.    How much HCl (in mL) is required to reach a titration equivalence point? B) Assume that you are titrating 60.0 mL of 0.0500 M ammonia (Kb = 1.8 × 10–5) with 0.100 M hydrochloric acid. Setting up I.C.E charts for NH3 before the titration, and when the titration reaches the equivalence point.  Based on the I.C.E. Chart and find...

  • If you titrated 30.0 mL of 0.1 M HCl with 0.1 M NaOH, indicate the approximate...

    If you titrated 30.0 mL of 0.1 M HCl with 0.1 M NaOH, indicate the approximate pH (a) at the start of the titration and (b) at the equivalence point. (c) What is the total volume of the solution at the equivalence point? Add this curve to your sketch in question 2.   [a. 1.0; b. 7.0; c. 60 mL

  • Consider the titration of 25.00 mL of 0.082 M KI with 0.051 M AgNO3.             Ksp...

    Consider the titration of 25.00 mL of 0.082 M KI with 0.051 M AgNO3.             Ksp for AgI is 8.3 X 10−17 Write the chemical reaction occurring in the beaker during the titration. Calculate the equivalence point volume. (about 40 mL, calculate to 4 significant figures) Calculate the pAg a) Before AgNO3 is added (Boom, Why?)             b) At the volume half way to the equivalence point (14.4)             c) At the equivalence point (8.04)             d) 5 mL after...

  • Perform the calculations needed to generate a titration curve for 50.00 ml of a 0.0500 M...

    Perform the calculations needed to generate a titration curve for 50.00 ml of a 0.0500 M NaCl solution titrated with 0.1000 M AgNO3 . Note for AgCl the Ksp = 1.82×10-10 . (i) Calculate pAg when 10.00 ml of AgNO3 is added. (ii) Calculate pAg when 25.00 ml of AgNO3 is added. (iii) Calculate pAg when 26.00 ml of AgNO3 is added. Given the solubility products above, show (by calculation) which of the two compounds concerned has the greater solubility...

  • Assume that you are titrating 60.0mL of 0.05 M Ammonia (Kb = 1.8x10^-5) with 0.1 M...

    Assume that you are titrating 60.0mL of 0.05 M Ammonia (Kb = 1.8x10^-5) with 0.1 M Hydrochloric Acid. Fill in the following table and explain your answers with calculation. (I really need a thorough table and calculations here, I understand almost nothing of this, please help.) This is all the info I have for the whole question Volume(mL) of HCl added Total volume(mL) [NH3] [NH4+] {H3O+](Fill this in only after equivalence point is reached) pOH pH 0 mL 15 mL...

  • You are titrating 50.0 mL of a 2.64 M benzoic acid solution with a 0.445 M...

    You are titrating 50.0 mL of a 2.64 M benzoic acid solution with a 0.445 M potassium hydroxide solution. What is the pH of the benzoic acid solution before you begin titrating? What is the pH after 20.0 mL of the potassium hydroxide solution has been added? What volume of potassium hydroxide is needed to reach the equivalence point? What is the pH at the equivalence point? What is the pH after 332.0 mL of potassium hydroxide has been added?

  • QUESTION 2 Suppose you have 20 mL of 0.1 M HCl. What will the pH of...

    QUESTION 2 Suppose you have 20 mL of 0.1 M HCl. What will the pH of the solution be after 10 mL of 0.1 M NaOH is added? Report your answer to 2 significant figures (i.e., 2 decimal places). Suppose you have 20 mL of 0.1 M HCl. What will the pH of the solution be after 30 mL of 0.1 M NaOH is added? Report your answer to 2 significant figures (i.e., 2 decimal places).

  • 1. You are titrating a 100.0 mL  solution of 0.050 M HBrwith a 0.150 M solution of...

    1. You are titrating a 100.0 mL  solution of 0.050 M HBrwith a 0.150 M solution of KOH.  What will be the pH after the addition of 25.0 mL KOH? 2. You titrate 250 mL of 0.250 M acetic acid (Ka= 1.8 x 10-5) with 50.0 mL of 0.350 M NaOH.  What is the pH of this solution? 3. For the titration in question 2, what would be the Kaof an ideal indicator.

  • A chemist titrates 25.0 mL of 0.00100 M I- solution with 0.000500 M Ag+ . It...

    A chemist titrates 25.0 mL of 0.00100 M I- solution with 0.000500 M Ag+ . It takes 50.0 mL of titrant to reach the equivalence point. The Ksp= 8.3 x 10-17 for AgI solid.   a) What is the [I-] value when the added titrant volume is 48.0 mL? b) What is the pAg+ value when the added titrant volume is 48.0 mL?

  • How many mL of 0.1 M NaOH would you have to add to 30 mL of...

    How many mL of 0.1 M NaOH would you have to add to 30 mL of 0.35 M HCl to reach the equivalence point?

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