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12 Nov 2019

___1. Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC₂H₃O₂. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was present?

(A) 1.60 M
(B) 0.800 M
(C) 0.600 M
(D) 0.450 M
(E) 0.200 M

_2. HSO₄^- + H₂O <===> H₃O⁺ + SO₄^2-

In the equilibrium represented above, the species that act as bases include which of the following?

I. HSO₄^-

II. H₂O

III. SO₄^2-

(A) II only
(B) III only
(C) I and II
(D) I and III
(E) II and III

_3. Which of the following has the lowest pH?

(A) 0.1 M CuSO₄
(B) 0.1 M KOH
(C) 0.1 M BaCl₂
(D) 0.1 M HF
(E) 0.1 M HNO₃

___4. What volume of 0.150-molar HCl is required to neutralize 25.0 millilters of 0.120-molar Ba(OH)₂?

(A) 20.0 mL
(B) 30 0 mL
(C) 40.0 mL
(D) 60.0 mL
(E) 80.0 mL

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Titration of Acetic Acid in Vinegar :

A) Determine the concentration of acetic acid if it is between 5% (wt/wt) in Mole/L(M). Assume a density of 1.0056 g/mL for the vinegar.

B) Will the acetic acid solution of the vinegar be too concentrated to perform this titration with a NaOH solution of 0.1 M? If you donât know by just looking at the numbers, this can be determined by pretending you are doing a titration and calculating the end point. Pick a volume of acetic acid (conc from #6) you would like to titrate. Then calculate the volume of NaOH you will need (the endpoint).

C) Based on your results, determine if you need to dilute the vinegar or not. If no, go to question 11. If yes, decide how much you will dilute the vinegar. Describe the glassware and procedure below. Remember that you want to do this in a quantitative fashion, so you need to pick the correct glassware.

D) Calculate the approximate concentration of the acetic acid of the diluted vinegar.

E) Again pick a volume of diluted vinegar you want to titrate (conc. of acetic acid was determined in #9). Calculate the expected end point (volume of NaOH needed).

i need help graphing this information based on data 1 and data 2 based on information below provided

Activity 1: Buffer Solution Preparation

The following eight solutions are prepared in the eight plastic cups labeled with the solution names.

1. Based on the Preparation calculations, prepared 50 mL of a 0.10 M solution of sodium acetate in the cup labeled sodium acetate. 0.050L x 0.10M= 0.005 x 82.03= .41g CH₃COONa

2. 100 mL of pure water was added to the cup labeled water

3. 50 mL of a 0.1 M acetic acid solution was added to the cup labeled acetic acid.

4. 10 mL of a 0.1 M NaOH solution (0.10M)(10mL)=(1M)(V₂)V₂=1mL NaOH

5. 10 mL of a 0.1M HCl solution (.10M)(10mL)=(1M)(V₂)V₂=1mL HCl

6. 10 mL of a pH 3.7 buffer (9.1 mL of 0.1 M acetic acid and 0.9 mL of sodium acetate)

7. 10 mL of a pH 4.7 buffer (5.0 mL of 0.1 M acetic acid and 5.0 mL of sodium acetate)

8. 10 mL of a pH 5.7 buffer (0.9 mL of 0.1 M acetic acid and 9.1 mL of sodium acetate)

The following amount of Bogenâs Universal Indicator was added to each solution: 10 drops to the acetic acid and the sodium acetate solutions, 20 drops to the 100 mL water, and 2 drops to the NaOH and the HCl solutions.

The 24-well plate was placed on to a sheet of plain white paper as shown below, and one drop of universal indicator was added to each well. The following amount of solutions was transferred the appropriate pipets to each well.

a. 1 mL of 0.1 M acetic acid to all four wells in the first row of the 24-well plate.

b. 1 mL of water to all four wells in the second row of the plate

c. 1 mL of 0.1 M sodium acetate solution to all four wells in the third row

d. 1 mL of the 3.7 pH buffer to all four wells in the fourth row

e. 1 mL of the 4.7 pH buffer to all four wells in the fifth row

f. 1 mL of the 5.7 pH buffers to all four wells in the sixth row

The color of the solution for each row was recorded, and a photo of the plate was taken.

The approximate pH of the solution was determined based on the indicator color chart.

One drop of 0.1 M HCl was added to the second well of each row, 1 drop of 0.1 M NaOH was added to the third well of each row, and 10 drops of 0.1 M NaOH was added to the fourth well of each row.

The color and corresponding pH was recorded.

A photo of the plate showing the colors in each well was taken.

	0.1M Acetic Acid	water	0.1M Sodium Acetate	pH 3.7 Buffer	pH 4.7 Buffer		pH 5.7 Buffer
Initial Color		yellow	green	pink		orange		yellow
Initial pH	4	6	7	4		5		6
Color after 1 drop HCl	Pink	Pink
pH after 1 drop HCl	4	4	7	4		5		6
Color after 1 drop NaOH	Pink	blue	blue					blue
pH after 1 drop NaOH	4	8	8	4		5		8
Color after 10 drops NaOH	Pink	purple	purple					purple
pH after 10 drops NaOH	4	10	10	4		5		10

Activity 2: Buffering Capacity of a Solution

The 24-well plate was placed on to a sheet of plain white paper at 90Â°so that it is four rows by six columns

20 mL of pH 4.7 buffer was prepared by doubling the volumes calculate in from activity 1 in the appropriate cup, and 2 mL of the solution was added into all 6 wells in the first row.

5 mL of the pH 4.7 buffer solution was diluted with 15 mL of purified water containing the indicator and poured into a clean cup. 2 mL of this first dilution was added to all the wells in the second row.

5 mL of the first dilution was diluted with 15 mL of purified water containing the indicator and poured into a clean cup. 2 mL of this second dilution was added to all the wells in the third row.

5 mL of the second dilution was diluted with 15 mL of purified water containing the indicator and poured into a clean cup. 2 mL of this third dilution was added to all the wells in the fourth row.

An additional drop of indicator was added to each well to make the color more visible. The color of the first well of each row was recorded.

One drop of 0.1 M NaOH solution was added to the second well in each row, two drops of 0.1 M NaOH solution was added to the third well of each row, three drops to the fourth well, four drops to the fifth well, and five drops to the sixth well. The color and corresponding pH of each well was recorded, and a photo of the plate showing the colors in each well was taken. The sodium acetate molar concentration of each dilution was calculated.

	pH 4.7 Buffer	First Dilution	Second Dilution	Third Dilution
Initial Color	orange	orange	orange	orange
Initial pH	5	5	5	5
Color after 1 drop NaOH	orange	orange	Blue	purple
pH after 1 drop NaOH	5	5	8	10
Color after 2 drops NaOH	orange	yellow	Blue	purple
pH after 2 drops NaOH	5	6	8	10
Color after 3 drops NaOH	orange	green	purple	purple
pH after 3 drops NaOH	5	7	9	10
Color after 4 drops NaOH	orange	purple	purple	purple
pH after 4 drops NaOH	5	9	9	10
Color after 5 drops NaOH	orange	purple	purple	purple
pH after 5 drops NaOH	5	9	9	10
Concentration of sodium acetate	0.1 M	2.5x10^-2 M	6.3x10^ -3 M	1.6x10^-3 M

Please help me solve this questions for solution concentratrions. I don't really know how to get to the answer.

1) Calculate the molarity of a solution made by dissolving 123.4 g of sodium sulfate (Na₂SO₄) in enough water to form 525.0mL of solution.

2) What is the molarity of a solution that is made by dissolving 13.68g of sucrose (C₁₂H₂₂O₁₁) in sufficient water to form 225.0mL of solution?

3) Calculate the molarity of a solution made by dissolving 15.00 g of glucose (C₆H₁₂O₆) in sufficient water to form exactly 200mL of solution.

4) What is the molar concentration of each ion present in a 0.225 M aqueous solution of calcium nitrate?

5) What is the ratio of the concentration of potassium ions to the concentration of carbonate ions in a 0.1275 M solution of Aluminium carbonate?

6) What is the molar concentration of K⁺ ions in a 0.0175 M solution of potassium Phosphate?

7) How many grams of Na₂SO₄ are required to make 1.250 L of 0.800 M Na₂SO₄?

8) What is the concentration of ammonia in a solution made by dissolving 13.75 g of ammonia in 8.0 L of water?

9) (a) How many grams of Na₂SO₄ are there in 250 mL of 0.50M Na₂SO₄? (b) How many milliliters of 0.50 M Na₂SO₄ solution are needed to provide 0.038 mol of this salt? (c)How many milliliters of 2.5M H₂SO₄ are needed to make 450mL of 0.20M H₂SO₄?

10) What volume of 1.00M stock solution of glucose must be used to make 200.0mL of a 2.75x10^â2M glucose solution in water?

11) (a) What volume of 2.80 M lead(II) nitrate solution contains 0.550 mol of Pb²⁺? (b) How many milliliters of 5.0 M K₂Cr₂O₇ solution must be diluted to prepare 550 mL of 0.20 M solution? (c) If 20.0 mL of a 10.0 M stock solution of NaOH is diluted to 250 mL, what is the concentration of the resulting stock solution?

12) Glacial acetic acid with density 1.049 g/ml â Calculate the molarity if 20.00 ml of glacial acetic acid dissolved in enough water to produce 250.00 ml of the solution.

13) Glycerol, C₃H₈O₃, with density of 1.2656 g/ml. Calculate the molarity of a solution of glycerol, when 50.00 ml of glycerol dissolved in enough water to make 500.00 ml of the solution.

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