How will Le Chatlier’s Principle be used to? a. Cause a color change for an indicator in Part A b. Cause an insoluble salt to become more soluble A. Acid-Base IndicatorsThere is a large group of chemical substances, called acid-base indicators, which changecolor in solution when [H] changes. A typlcal substance indicator like this is calledmethyl violet, which we will give the formula HMV. In solution HMV dissociates asfollows:HMV(aq)yellowH(aq) + MV (aq)violet(5)HMV has an intense yellow color, while the anion MV is violet. The color of theindicator in solution depends very strongly on [H"].1. Add about 5 mL of distilled water to a regular (18 x 150 mm) test tube. Add 3-5 drops.of methyl violet indicator. Record the color of the solution in your notebook.2. How could you force the equilibrium system to go to the other form (color)? Select areagent (something that adds H or removes H") that should do this and add it to thesolution, drop by drop, until the color change is complete. Record your observations inyour notebook. If there is no color change, try another until reagent you find one thatdoes. Work with 6 M reagents if they are available..3. Equilibrium systems are reversible. That is, the reaction can be driven to the left andright by changing the conditions in the system. How can you force the system in Step 2 torevert to its original color? Select a reagent that should do this and add it drop by dropuntil the color has become the original one. Again, if your first choice was incorrect, tryanother reagent. Record everything in your notebook.4. Answer all the questions for Part A in the data section before going on to Part B.

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Answered: How will Le Chatlier’s Principle be…

How will Le Chatlier’s Principle be used to? a. Cause a color change for an indicator in Part A b. Cause an insoluble salt to become more soluble

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 82E: The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they...

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The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
Methyl violet belongs to a large class of chemicals called acid-base indicators. These substances change color in solution when the hydrogen ion concentration changes. The actual formula for methyl violet is quite complicated, so we'll use the abbreviation HMV. This notation suggests that methyl violet is itself a weak organic acid. In solution, methyl violet dissociates as follows: HMV(ag)-yellow + H*(ag) + MV(ag)-violet (2) According to the video : (a) What are the colors of methyl violet in an acidic medium , and in a neutral environment ? (b) What was the acidic pH_ What was the neutral pH_ (c) Predict what will happen to the color if HCl solution is added to the reaction system ? (d) What will happen if NaOH is added ?
Che. 065: Acid -Base Titration: Part I: Standardization of NaOH(aq): Molarity of NaOH(aq) is determined by using the stoichiometry reaction with a strong acid such as HCl(aq). Part II: Molarity and mass % of acetic acid CH3COOH(aq) in a vinegar solution are determined by the reaction with NaOH(aq). Part I: Standardization of NaOH(aq): Use a 50.00 mL. Buret : wash it with tap H2O twice, with deionized H2O twice and twice with 0.100 M HCl (aq). Fill the buret with 0.100 M HCl(aq), remove the air bubble and adjust the initial buret reading to 0.00 mL. Get two 125 mL. Erlenmeyer. To each Erlenmeyer flask add 20.00 mL. HCl(aq) from the buret. Burette Holder 3P Burette Flask Support Stand Trail 2 Trial 1 Initial buret reading of HCl(aq): 0.00 mL. Final buret reading of HCl(aq): 20.00 mL. Volume of HCl(aq) : Initial buret reading of HCl(aq): 20.00 mL. Final buret reading of HCl(aq): 40.00 mL. Volume of HCl(aq) Add 3 drops of phenolphethaleine to each Erlenmeyer flask, the color of solution is…
(92) What is [OH-] in a solution of 1.25 M NH3 and 0.78 M NH4NO3? NH3 (ag) + H2 O(1) NH4 +(ag) + OH-(ag)_ Kb = 1.8 x 10-5
5. What concentration of acetate ion (CH3CO2') in 0.500 M CH3CO2H produces a buffer solution with pH = 5.00? (Ka = 1.8 x 10-5) CH;CO2H (aq) H20 (I) CH;CO, (aq) H30* (aq) + 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH;CO2H) to 1.00LH,0. What is the pH of the solution at equilibrium? (K, 1.8 x 10°)
Methyl orange is an indicator used for detecting the pH of acidic solutions. The red, protonated form of the indicator (HIn) dissociates into a yellow, deprotonated form (In¯) as shown in the reaction. The pKa for methyl orange is 3.4. HIn(aq) = H*(aq) + In¯(aq) yellow red Identify the color of a solution containing methyl orange Identify the color of a solution containing methyl orange indicator at pH 2. indicator at pH 3.4. orange yellow yellow orange red red Identify the color of a solution containing methyl orange indicator at pH 6. orange yellow red
(5e) Which two of the following compounds would you make a buffer of pH = 12.5. H3PO4 (MM=98.00 g/mol), NaH2PO4 (MM=119.98 g/mol), NazHPO4 (MM=141.96 g/mol), and Na3PO4 (MM = 163.94 g/mol)? [For H3PO4: pK; = 2.148; pKz=7.199; pK3=12.15]
Complete the changes in concentrations for each of the following reactions:(a) AgI(s) ⟶ Ag+(aq) + I−(aq) x _____(b) CaCO3(s) ⟶ Ca2+(aq) + CO3 2−(aq) ____ x(c) Mg(OH)2(s) ⟶ Mg2+(aq) + 2OH−(aq) x _____(d) Mg3(PO4 )2(s) ⟶ 3Mg2+(aq) + 2PO43−(aq) x_____(e) Ca5(PO4 )3OH(s) ⟶ 5Ca2+(aq) + 3PO4 3−(aq) + OH−(aq) _____ _____ x
Consider the titration of the weak acid, benzoic acid, HC7H5O2. Its acid dissociation reaction is: HC7H5O2 (aq) + H2O (l) ↔ C7H5O2- (aq) + H3O+ (aq) A 25.00 mL sample of a solution of benzoic acid, concentration unknown, is titrated with 0.0500M NaOH solution. A plot of the titration is shown below. 1. what is the pKa (approximately) of benzoic acid? Its Ka? 2. on the plot, indicate the buffering region of the titration 3. From the pH at the equivalence point, estimate the pKb of benzoate ion (conjugate base to benzoic acid)______________[Remember, at the equivalence point, C7H5O2- (aq) + H2O (l) ↔ HC7H5O2 (aq) + OH- (aq) ]
Ammonia (NH3) is a weak base with a Kp = 1.8 x 10-5. A certain solution of ammonia has a %3D pH = 9.05. What was the molar concentration of ammonia in the starting solution? %3D NH3(aq) + (H20(1) NH,*(aq) + OH (aq) And pH = JUL CC
(2) When ammonium sulfate dissolves, both the anion and cation have acid-base reaction: (NH4)2SO4(s)< 2NH4* + SO4²- NH4* + NH3(aq) + H* SO42- + H2O → HSO4 + OH- Ksp = 276 Ka = 5.70 ×10-10 Кь 3 9.80 х 10-13 (a) (b) (c) (Show your Calculation) Write a charge balance for this system. Write a mass balance for this system. Find the concentration of NH3(aq) if the pH is fixed at 9.25.