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crimsonsheep797Lv1

28 Sep 2019

The acid-dissociation constant for hypochlorous acid (HClO) is3.0x10^-8

A)Calculate the concentration of H30+at equilibrium if the initialconcentration of HClO is 7.8Ã10-3 .

B)Calculate the concentration of ClO- at equilibrium if the initialconcentration of HClO is 7.8Ã10-3 .

C)Calculate the concentration of HClO at equilibrium if the initialconcentration of HClO is 7.8Ã10-3 .

If someone could please show me how to perform these equations, Iwould appreciate it!

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Sixta KovacekLv2

28 Sep 2019

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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

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a. 50 mL

b. 34 mL

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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

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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

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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

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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

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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

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1. consider a 0.45 M solution of hypochlorous (H0CL) in water (at 298K). a) write the equilibrium expression for the dissociation of this weak acid. b) what are the concentrations of all species at equilibrium if Ka(HOCL) = 3.5 X 10^-8? c) why is it ok to use this approximation (o.45-x~0.45) d) Now use your result from b to find the pH of 0.45 M solution of hypoclorous acid. e) what is the hydronium ion concentration of a HOCL solution at pH 3.33?

Please help