CHEM 1AA3 Study Guide - Midterm Guide: Bromophenol Blue, Titration Curve, Buffer Solution

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Enter your version number in the correct column on your scan sheet (see p. 2 for details: the ph of a 0. 01 m aqueous solution of a strong base is: At ph 6. 5, the ratio of mes, a weak base, to irs conjugate acid, mesh+, is [mes]/[mesh+] = 2. 19. Ka(ch3cooh) = 1. 8 x 10-5: 1. 66 x 10-3, 1. 34 x 10-3, 3. 22 x 10-3, 4. 24 x 10-3, 7. 18 x 10-3, a buffer is made using only tris (weak base) and trishcl (weak acid). Ka(hno2) = 7. 2 x 10-4: 3. 53, 4. 65, 6. 04, 2. 30, 3. 14, bromophenol blue is an acid-base indicator with a pka of 4. 0. The acidic form is yellow and the basic form is blue-violet. A few drops of this indicator are added to the titration of benzoic acid (beaker, pka = 4. 20) with naoh(aq) (buret). Weak acid ka: glycine 4. 6 x 10-3, lactic acid 1. 4 x 10-4, h2po4. 6. 3 x 10-8: h2co3 4. 5 x 10-7, nh4.

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I would really appreciate it if someone showed me how to solve each of these problems instead of just giving the answers. I bolded the correct answer. Thank you

1. How many milliliters of a 5.0 x 10^-2 stock solution would you need to add to a final volume of 10 liters to obtain a solution with a pH of 3.60?

a. 50 mL

b. 34 mL

c. 13 mL

2. A 0.25 M solution of a hypothetical weak acid, HX has a pH of 3.42. What is the Ka value for this acid?

a. 8.8 x 10^ -6

b. 1.6 x 10^ -7

c. 5.8 x 10^ -7

3. What is the pH of a 0.30 M solution of magnesium hypochlorite(Mg(ClO)2)? For HClO Ka= 3.0 x10^ -8

a. 9.06

b. 3.06

c. 10.65

4. The pH= 2.84 for a 0.35 M pyridine hydrochoride, C5H5NHCl, solution. Based on this information, determine the Kb value of pyridine (C5H5N)

a. 9.4 x10^-8

b. 1.7x 10^ -9

c. 5.3 x 10^ -7

5. If you wanted to prepare a buffer composed of hypochlorous acid (HClO0 and potassium hypochlorite (KClO), how may moles of KClO would be added to 2 liters of a 1.0 M HClO solution to get a buffer with a final pH of 7.70? For HClO, Ka= 3.0 x 10^-8

a. 3.0 mol KClO

b. 1.2 mol KClO

c. 2.2 mol KClO

6. The pH of a solution by mixing 300 mL of 0.050 M HClO4 and 40.0 mL of 0.10 M Ba(OH)2 is?

a. 1.69

b. 1.77

c. 1.85

7. A 150 mL sample of 0.20 M HF solution is titrated with a strong base. What is the pH after adding 40 mL of 0.80 M NaOH? For HF, Ka= 6.8 x 10^-4

a. 13.11

b. 12.02

c. 10.37

8. A solution of Pb(NO3)2 is mixed with a solution of NaCl. A precipitate forms and analysis of the supernatant reveals the following concentrations of ions.

[Pb^2+] = 0.0062 M [NO3-]= 0.25 M [Na+]= 0.40 M [Cl-]= 0.054 M

Based on these data, what is the Ksp value for PbCl2(s)?

a. 7.2 x 10^-6

b. 5.6 x 10^-8

c. 1.8 x10^ -5

9. At an elevated temperature, Ksp= 7.5x 10^ -5 for Ca(OH)2. What is the pH of a saturated solution of a calcium hydroxide?

a. 13.06

b. 9.51

c. 12.73

d. You a buffer with 4.00 M NH3 and 0.600 M NH4Cl

i. What is the pH of this buffer solution? Kb = 1.8 Ã 10-5 (2 Marks)

ii. To 100.0 mL of this buffer solution is added 25.0 mL of 0.300 M HCl, what is the pH of the resulting solution (4 Marks)

iii. To 200.0 mL of this buffer solution is added 40.0 mL of 0.300 M NaOH, what is the pH of the resulting solution (4 Marks)

2)2.50 g of HClO was dissolved in 250 mL of water
a) Calculate the pH
b) Calculate pOH

15.6 mL of 4.0 M HCl are diluted with water to make 1.5 L of solution. What should be the pH of the final solution?

Which of these statements are true?

1. A Bronsted base accepts a proton from an acid.

2. OH^- is the conjugate acid of O^2-.

3. H₃O⁺ is the conjugate acid of OH^-.

4. An Arrhenius acid is a substance that produces H⁺ ions.

5. The stronger the acid, the smaller the K_a

_{Answer choices below:}

	a.	I, IV, V
	b.	I, II, IV
	c.	II, III
	d.	I, III, IV
	e.	III, V

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CHEM 1AA3 Study Guide - Midterm Guide: Bromophenol Blue, Titration Curve, Buffer Solution

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