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I need you to do these chemistry questions there are 6 pages, but not difficult I upload them in the file

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Hydrolysis & Buffers Lab Report Sheet eed Name: Abdul Partner: Save Alrashi sa char 1. What are the ions in each of these salts? a. NaC2H302 b. NH4Cl 09 C. Na2CO3 MH dil d. K3PO4 2. For each of the salts, write the chemical formula for the acid and the base from which it is derived and identify whether the acid and the base are strong or weak. Example Naci NaOH strong base HCI strong acid a. NaC2H302 HO b. NHACI C. Na2CO3 d. K3PO4 3. Identify the ion in each salt that will undergo hydrolysis and write the hydrolysis equation for this ion. Remember that ions hydrolyze with one water molecule at a time. a. NaC2H302 b. NHACI C. Na2CO3 d. K3PO4 1 4. Predict whether aqueous solutions of these salts should be acidic, basic or neutral. a. NaC2H302 b. NHACI C. Na2CO3 d. K3PO4 pH Measurement Data 5. Calibrate the Vernier pH probe with a 2 point calibration using two different buffer solutions. 6. After calibrating the pH probe, measure the pH of 25 mL of 0.10M sodium acetate solution and 25 mL of 0.10M ammonium chloride solution (separate 50 ml beakers). 7. From your pH measurements complete all of the following: 1. Sodium acetate solution pH 8.44 pОН [H30+) (OH) a. Using your experimental data, construct an ICE table, then calculate the equilibrium constant and the pk for the ion undergoing hydrolysis. Identify the equilibrium constant as either Ka or Kb. . bns zelo Experimental K pk 2 b. Calculate the actual value of the equilibrium constant using Kw and the Ka reference value for acetic acid: Ka = 1.8 x 10-5 Reference K рк. C. Calculate the % error using the pk values. sultantul od solid sod for your buffer 0.0 ml volume 2. Ammonium Chloride Solution pH 5.44 Celio pОН [H3O+] (OH) Ho a. Using your experimental data, construct an ICE table, then calculate the equilibrium constant and the pk for the ion undergoing hydrolysis. Identify the equilibrium constant as either Ka or Kb. nad OHNE CH i sad imaju dor Experimental K pk 3 b. Calculate the actual value of the equilibrium constant using Kw and the Kb reference value for ammonia: Kb = 1.76 x 10-5 Reference K pk C. Calculate the % error using the pk values. 1. Buffers Acid Addition 1. Set up four 50 mL beakers. Place approximately 30 mL of each of the following in a separate beaker: distilled water, pH 4 buffer, pH 7 buffer, pH 10 buffer. Measure pH. Before addition: H20_8.12 pH 4 405 pH 7_6.99 pH10_10.02 2. To each of the beakers add 2 drops of 6M HCl, then measure the pH: After addition: H20 2.10 pH 4 3,20 pH 7_6.44 pH10_9.69 2. Base Addition 1. Set up four 50 ml beakers. Place approximately 30 mL of each of the following in a separate beaker: distilled water, pH 4 buffer, pH 7 buffer, pH 10 buffer. 2. To each of the beakers add 2 drops of 6M NaOH, then measure the pH: After addition: H₂O 11.39 pH 4_4.86 pH 77.68 PH10 10.43 4 3. Explain the results. Discuss the change in pH in the water and contrast it to the change in pH of the buffer systems. No Halo Acid Addition Base Addition 4. Prepare your own buffer solution. You will be assigned a pH value for your buffer. You will have available 0.30M acetic acid, solid sodium acetate and a 50.0 mL volumetric flask. Your assigned Buffer pH is_ 5.20 a. Calculate the amount of sodium acetate required to make the buffer. Show all your work. bns bolo og below 5
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1
Running Head: CHEMISTRY ASSIGNMENT

Chemistry Assignment
Student’s Name
Institutional Affiliation

Q1.
a. Sodium ions, acetate ions
b. Ammonium ions, chloride ions
c. Sodium ions, carbonate ions
d. Potassium ions, phosphate ions
Q2.
a. NaOH strong base, CH3COOH weak acid
b. NH4OH weak base, HCl is strong acid
c. NaOH strong base, H2CO3 weak acid
d. KOH strong base, H3PO4 weak acid.

2
Running Head: CHEMISTRY ASSIGNMENT

Q3.
a. NaC2H3O2 + H2O → NaOH + CH3COOH
b. NH4CL + H20 → NH3 +H30 + Cl
c. NA2CO3 + H20 → NaOH +H20 +C02
d. K3PO4 + H20 →KOH + K2HPO4
Q4.
a. Acidic
b. Acidic
c. Basic
d. Basic
Q5.
So...


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