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Experiment 4- Properties of Systems in
1. Define Le Chatlier’s Principle.
2. 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
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- . 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?(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 10-5Che. 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…
- 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 ?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) ]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]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
- 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(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.The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. 1. what is the pH when the volume of base added equals half the volume of the equivalence point? 2. what is the pH of the titration when 20.00 mL of base have been added? 3. what is the pH of the titration when 30.00 mL of base have been added?