I need to write a lab plan based on preparing a standard solution-- Standardization of NaOH (aq)

Experiment 8: Preparing a Standard Solution—Standardization of NaOH(aq) Learning Objectives » to understand the meaning of the term primary standard » to learn how to determine the precise concentration of a solution » to learn how to properly prepare, use and read a buret » to practice titration techniques and calculations » to learn how to weighing by difference Read and complete the Prelab Assignment for Experiment 8 (Chemistry 121 Lab Moodle site). Note that these assignments are always due the Sunday the week of lab, by 5 PM. Safety: 3.0 M sodium hydroxide is hazardous and will attack skin and clothing rapidly. Don't wear expensive clothes to lab. Flood any spills with water and ask your instructor or assistant for help. Wear goggles! If solutions are splashed on your face, call for help and use the eyewash. Materials 3 M NaOH, solid KHP (potassium hydrogen phthalate) dried, in weighing bottles, phenolphthalein indicator solution, one buret, four 250-mL Erlenmeyer flasks. Disposal The solutions of KHP and dilute NaOH should be neutralized (5 < pH < 9) and only then may be poured down the drain with lots of water. This is a skill-building experiment, where you will have to work carefully and use equipment skillfully in order to achieve good results. Learning good titration techniques will be helpful in subsequent labs, not only as specific skills, but they illustrate the excellent results that can be achieved if sound technique is employed. Students can work individually or in pairs on this experiment. Remember, it's up to you to make sure that you take part in all lab activities!

A beaker with 1.10×10^2 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 mol L−1. A student adds 7.00 mL of a 0.490 mol L−1 HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.760.

Please show where all numbers comes from.

10) Aluminum doesn’t readily corrode because:

a) its standard reduction potential is more positive than oxygen

b) its standard reduction potential is more negative than oxygen

c) it forms a dense coating of alumina, Al₂O₃, that slows oxidation.

d) It is already oxidized.

.

11) What best describes a glass?

a) A transparent, crystalline insulator.

b) A viscous liquid

c) An amorphous solid

d) The thermodynamic (lowest energy) state for a material

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For the following reaction answer questions 13 & 14):

                       Fe(s) + Cu²⁺(aq)            Fe²⁺(aq) + Cu(s)

13) What is being oxidized (oxidant)?

a) Fe²⁺

b) Cu²⁺

c) Cu

d) Fe

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14) What is being reduced (reductant)?

a) Fe²⁺

b) Cu²⁺

c) Cu

d) Fe

Please answer all of them without guessing!!! Thanks

Use the following thermodynamic data to calculate ∆S° (universe) for the formation of HBr(g) from its elements at 298K in J/K.   HINT: write the formation reaction for HBr(g)

Species        ∆H_f° (kJ/mol)        S° (J/Kmol)                  Species      ∆H_f° (kJ/mol)      S° (J/Kmol)

HBr(g)           -36.3                   198.59                               Br₂(g)          30.91                245.38

Br₂(l)                  0                   152.23                              H₂(g)              0                     130.6

Arrange the following 0.10 M

solutions in order of increasing acidity: (i) NH4NO3, (ii) NaNO3, (iii) CH3COONH4, (iv) NaF, (v) CH3COONa.

There are several classifications of chemical reactions. Please research a reaction and provide its particular classification and characterization(s).

Balance the following aqueous reactions:

a. CrI₃ + Cl₂ -----> CrO₄^2- + IO₄^1- + Cl^1- (basic solution)

b. Cr(NCS)₆^4- + Ce⁴⁺ ----> Cr³⁺ + Ce³⁺ + NO₃^1- + CO₂ + SO₄^2- (acidic solution)

12. Calculate the pH of a buffer solution made from 0.30 M hydrofluoric acid and 0.70 M sodium fluoride after the addition of 0.08 mol of NaOH to 1.0 L of this solution.  Assume no change in volume.  The Ka for HF is 3.5 • 10-4.

Can someone guide me through this question? The answer is below but I can figure out how they got this answer.

Answer: pH = 4.01

To a 100.0mL volumetric flask are added 1.00 mL volumes of three solutions: 0.0100 M AgNO3, 0.190 M NaBr, and 0.100 M NaCN. The mixture is diluted with deionized water to the mark and shaken vigorously. What mass of AgBr would precipitate from this mixture? (Hint: The Ksp of AgBr is 5.4x10-13 and the Kf of Ag(CN)2- is 1.0x1021)

A 300mL buffer is prepared in which [HCO3-] = 0.2M and [CO3^2-]=0.075M.

a) What is the pH of this buffer (Ka HCO3-=4.7x10^-11)?

b) What is the pH of the buffer if 0.0100 moles of HCl are added?

c) What is the pH of the buffer if 0.0200 moles of NaOH are added?

Balance the following, in basic solution, by the method of half reactions.

C₂H₅OH +MnO₄^- -->C₂H₃O₂^- +MnO_2,

What is the coefficient on water (H₂O) in the product of the balanced equation?

Why can a heavy-water moderated reactor use a lower enrichment uranium fuel than a light water moderated reactor?

Structural data evolves with time, even for simple molecules. Consider the compounds E(CF₃)₃, i.e, the tris(trifluoromethyl) derivatives of P, As, and Sb. C-E-C bond angles were determined by gas-phase electron diffraction in the mid-20^th century and given as: E=P, 99.6°; E=As, 100.1°; E=Sb, 100.0°.          

a) Does this trend seem reasonable, and explain your answer.                    

b) A more rigorous recent similar experiment gave a C-As-C bond angle of 95.4°, compared to a calculated value of 95.9°. In view of this which of the other two C-E-C bond angles seems most suspect, and why?