University College - Chemistry Chem 112A Lecture Notes - Lecture 13: Sodium Chloride, Lead

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limehorse889

15 Feb 2017

School

WUSTL

Department

University College - Chemistry

Course

University College - Chemistry Chem 112A

Professor

D' Arcy

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Document Summary

0. 1m ki -> k+, i- in 1l of solution. Ksp = 1. 4 x 10-8 = s(0. 1 + 2s)2. I- is present in solution initially, which pushes the reaction left and there is less dissolution of. The presence of a common ion will result in a decrease of the solubility of the salt. But ag2cro4 is not soluble so first k2cro4 must be dissolved. Then agno3 is added creates ag2cro4 precipitate. Nacl added, so there is an excess of cl- ions. Original reaction pushed to the right, disrupting the equilibrium, and pulling the. Ag+ ions out of solution with cl- ions. The less soluble species is pulled out of solution, and forces the slightly non soluble species to dissolve. 0. 015m agno2 + 0. 005m pbno2 + nacl -> agcl + pbcl2. Agcl is insoluble (ksp = 1. 6 x 10-10) Pbcl2 is slightly soluble (ksp = 1. 6 x 10-5) If q = [pb2+][cl-]2 > ksp = 1. 6 x 10-5.

Related Questions

For questions 13-14, use the information provided below from the experiment Identification of an Unknown. The molecular masses and reactions are provided for you.

NaHCO₃ KHCO₃ Na₂CO₃ K₂CO₃ NaCl KCl

84.01 g/mol 100.12 g/mol 105.99 g/mol 138.21 g/mol 58.44 g/mol 74.55g/mol

2 NaHCO₃ (s) Ã Na₂CO₃ (s) + H₂O (g) + CO₂ (g) (Reaction 1)

Na₂CO₃ (s) +2HCl (aq) Ã 2NaCl (s) + H₂O (l) + CO₂ (g) (Reaction 2)

13. Brad starts with 0.652 g of unknown. How much mass should he have after the first heating step if his unknown
was NaHCO₃?

A. 0.411 g Na₂CO₃

B. 0.326 g Na₂CO₃

C. 0.822 g Na₂CO₃

D. 0.00402 g Na₂CO₃

14. If Brad has a final mass of 0.270 g at the end of the experiment (after the 2^nd heating), what is his percent yield
of the final salt? (Assuming he starts with 0.652 g of NaHCO₃).

A. 40%

B. 60%

C. 80%

D. 86%

15. What is the concentration of chloride ions in 50.0 mL of a 5.25 M solution of barium chloride?

A. 0.525 M Cl^-

B. 1.05 M Cl^-

C. 5.25 M Cl^-

D. 10.5 M Cl^-

Aqueous Solutions

16. Which of the following represents a correct precipitation reaction between sodium iodide and lead(IV) sulfate?

A. PbSO₄ (aq) + NaI(aq) Ã PbI (aq) + NaSO₄ (aq)

B. PbSO₄ (aq) + NaI(aq) Ã PbI (s) + NaSO₄ (aq)

C. Pb(SO₄)₂(aq) + NaI (aq) Ã PbI₂ (s) + Na₂SO₄ (aq)

D. Pb(SO₄)₂(aq) + NaI (aq) Ã PbI₂ (aq) + Na₂SO₄ (aq)

17. How many of the following salts would not form a precipitate in an aqueous solution?

A. one

B. two

C. three

D. four

18. What type of reaction is the following? CaCO₃ + heat Ã CaO + CO₂

A. Combination

B. Decomposition

C. Single Replacement

D. Combustion

19. Calculate the amount of copper recovered from an 85% yield if the theoretical yield is 0.25 g

A. 21 g

B. 3.4 g

C. 0.21 g

D. 0.34 g

20. Which of the following chemical species is the oxidizing agent in the reaction below?

Cu (s) + 4 HNO₃ (aq) â Cu(NO₃)₂ (aq) + 2 NO₂ (g) + 2 H₂O (l)

A. Cu (s)

B. HNO₃ (aq)

C. Cu(NO₃)₂ (aq)

D. NO₂ (g)

CHE 169 Exp. # 4 Le Chatelier's Principle and Chemical Equilibrium Run each of the following reactions in test tubes. For each reaction record your observa write a net ionic equation. Interpret your observations in terms of chemical equilibrium. and 1. Label a test tube #1, and add a few mL of NaOH to it. 2. Add CaClh drop wise until a noticeable precipitate of Ca(OH)2 is present. 3. N Ca(OH)2 in it "4 Add 6M HCI (NOT 12M!!) drop wise to the first test tube (#1) with the Ca(OH)2 until a change is observed. Record your results. 5 Prepare a stock solution b cylinder adding H20 to bring the volume to 100 mL. Save this stock solution for the rest of the class 6. Take 5mL of the stock solution and note the color. Add about 1mL of 0.1M FeCla solution and observe the result. ow add a few drops of the phenolphthalein indicator to the test tube #1 with the y mixing 2mL of 0.1M FeCly and 0.1M KSCN in a 100 mL graduated 7. Take 5mL of the stock solution and note the color. Add about 1mL of 0.1M KSCN solution and observe the result. 8. Take 5mL of the stock solution and note the color. Add 0.1M AgNO, solution dropwise until n into two test tubes including the precipitate. 9. Add 2mL of 0.1M KSCN dropwise to one tube and observe the result. 10. Add 2mL of 0.1M FeCla dropwise to the second tube and observe the result 11. Add 2 drops of 6M HNO, to roughly 3mL of 0.1M K2 result. .12. Add 10% NaOH solution dropwise to the solution from step 11 until the original color is restored 11. Add 2 drops of 6M HNO, to roughly 3mL of 0. 1M K,CrO, solution and observe the 13. Add 2 drops of 6M H2SO, to roughly 3mL of 0.1M K Cro, solution and observe the result *14. Add 10% NaOH solution dropwise to the solution from step 13 until the original color is restored ed, 10% NaOH 15. Add 3 mL of conc. HCI dropwise to 2mL (no more) of 0.1M CoCl2 and observe the result. 16. Add water dropwise to the solution from step 15 until the reverse reaction is evident. 17. Take the test tube from step 16 and place it in a water bath on a Bunsen burner and heat. .18. Label a test tube #3, and then add a few mL of the Cua solution to it. 19. Add 6 M NaOH drop wise until a precipitate of Cu(OH)2 is observed. 20. Add 6M NH3 drop wise (Use Caution!! Are those goggles still on!) until a change is observed. You will probably need to stir or shake your test tube. Record your observations 21. Add 6M HCI dropwise until a change is observed. Stir or shake as you add the HCI Record all observations. Revision 1.00 17 Jan 2012

Iodine is sparingly soluble in pure water. However, it dissolvesin solutions containing excess iodide ion:

I- (aq) + I2 (aq) <--> I-3 (aq) K=710 @ 25 degreesCelcius

What is the concentration of I2 at equilibrium if 0.10 mol of I2is added to 1.0 L of 0.20 M KI Solution?

goldswan130

University College - Chemistry Chem 112A Lecture Notes - Lecture 13: Sodium Chloride, Lead

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