Color of pHydrion strip: Navy Blue pH of saturated solution based on color guide: 13 Hydronium ion concentration in saturated solution, M: __________ Hydroxide ion concentration in saturated solution, M: __________ Estimated solubility product for calcium hydroxide: __________ Using the following information, how do I solve for 3,4, and 5?

Color of pHydrion strip: Navy Blue pH of saturated solution based on color guide: 13 Hydronium ion concentration in saturated solution, M: Hydroxide ion concentration in saturated solution, M: Estimated solubility product for calcium hydroxide: __ Using the following information, how do I solve for 3,4, and 5?

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter9: Complexometric And Precipitation Titrations

Section: Chapter Questions

Problem 6P

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The molar solubility of calcium carbonate in a 0.269 M calcium acetate solution is ______________ M.
This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?
Question : Write the equilibrium equations showing any hydrolysis (if any) that is happening in the solution for each of the solutions,. Discussion:Correlate the observed pH with the hydrolysis equilibria. Procedure:Part 1. Using a pH meter, measure the pH of the following 5 salt solutions (use the solutions that are labeled "Experiment 3"): 1 M NaC2H3O2 , 1 M NaCl, 1 M NH4Cl, 1 M NH4C2H3O2, 1 M Na2CO3 .Part 2. Go to the reagent shelves and find the containers of solid ammonium chloride, ammonium acetate, and ammonium carbonate. Open the containers and cautiously smell. Rank the three solids in terms of the strength of the ammonia odor. Part 3. Using a pH meter, measure the pH of 0.1 M NaH2PO4 (sodium dihydrogen phosphate) and 0.1 M Na2HPO4 (sodium monohydrogen phosphate).Part 4. Weigh out about 2 grams of solid aluminum sulfate (since this is an approximate mass, use the centigram balance, do not use the analytical balance) in a 50 mL beaker. Add about 10 mL of water and mix…
E University Librarie. E UNIVERSITY POR. Student Detail Sc. Part A The table shows respective color change when a universal indicator is added to the clear solutions. Rank the samples based on increasing order of acid strength. Solutions Color change 0.001 M lactic Light red 0.01 M phenol Light yellow 0.01 M nitrous acid Light orange 0.001 M hydrogen peroxide Light green Rank the solutions by Increasing order of their acid strength. To rank items as equivalent, overlap them. > View Available Hint(s) Reset Help 0.01 Mnitrous acid 0.001 Mlactic acid 0.001 M hydrogen peroxide 0.01 Mphenol Least acidic Most acidic P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions | Contact Us | MacBook Air 80 888 DII DD F3 F4 F5 F6 F7 F8 F9 F10 F11 $ & 3 4 7 8. 9. { R Y U 一 F J K く C V B N M + I| .. .- エト

Discussion:- 1. What the difference between primary and secondary standard substances? 2. Calculate the volume of conc. HCl required for preparing 250 ml 0.1 M? 3. Calculate the weight of NazCO, required for preparing 100 ml 0.1 M? 4. Why is sodium carbonate primary solution? 5. Why standard solution should be colorless? 6. Why is HCl not primary solution? 7. What is the titration?
How would the average calculated concentration of NaOH have been affected (Higher, Lower, No Change) if... 1. undissolved KHP was present in the bottom of the flask at the "end" of the titration. 2. you stopped the titration (and recorded the volume of NaOH added) immediately after the solution first became pink, however, the pink color disappeared almost immediately.
In Experiment 4, you used phenolphthalein HIn as indicator in titrating the acid content of samples. The indicator forms this equilibrium in an aqueous solution: HIn + H2O ↔ H3O+ + In-. During the course of the titration, the concentration of H3O+___________, shifting the equilibrium towards ___________ , until end-point is reached. a. decreases, HIn b.increases, In- c. increases, HIn d.decreases, In-
When we mix together, from separate sources, the ions of a slightly soluble ionic salt, the salt will precipitate if Qsp _____ Ksp, and will continue to precipitate until Qsp _____ Ksp.
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