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?
Gravimetrics Lab Question You have 20 mL of 0.0825 M Cl-. You are titrating 0.1 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 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 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 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 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 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 0.35 M HCl to reach the equivalence point?
Question 6 (1 point) In your pre-lab, you were asked to determine the concentration for a 25.00 mL sample of acetic acid, CH3COOH (K= 1.8 x 10-5) of unknown concentration. Suppose you now repeat that same titration, using another 25.00 mL sample of that same unknown acetic acid and the same concentration of NaOH as a titrant. However, before you start titrating, you add an additional 100 mL of water to the flask containing our sample of acid. Everything else...
If you titrated 30.0 mL of 0.1 M HCl with 0.1 M NaOH indicate the approximate pH at... a.) the start of the titration b.) at the equivalence point c.) What is the total volume of the solution at the equivalence point?
you have three flasks with 0.03 M Cl- , Br- I- if you have titrated each solution with Cu+ what order with the equivalence points appear in the titration curves? Ksp for CuI=1*10-12 Ksp for CuCl=1.9*10-7 Ksp for CuBr = 5 * 10-9 A. pCu+ (I-) < pCu+(Br-)<pCu+(Cl-) B.pCu+ (Cl-) < pCu+(Br-)<pCu+(I-) C.pCu+ (Br-) < pCu+(I-)<pCu+(Cl-)