Question

In: Chemistry

You have 100. mL of aqueous 0.40 M CuSO4 mixed with 100. mL of aqueous 0.20...

You have 100. mL of aqueous 0.40 M CuSO4 mixed with 100. mL of aqueous 0.20 M Na2S.

1. What kind of reaction could potentially take place? (a) Bronsted-Lowry acid base (b) redox (c) precipitation (d) no reaction

2. Which of the following is/are the spectator ions in this reaction? (a) SO42-   (b) Na+ (c) S2- (d) Cu2+

3. After the solutions are mixed, what will be the concentration of Na+ ? (a) 0.10M (b) 0.80M (c) 0.20M (d) 0.40M (e) something else

4. After the solutions are mixed, what will be the concentration of  SO42- ? (a) 0.40M (b) 0.20M (c) 0.80M (d) 0.10

5. Which reactant will limit the amount of product that can form? (a) Cu2+ (b) S2- (c) something else

6. This mixture will establish equilibrium in mere fractions of a second. After it does, what will be the concentration of Cu2+? (a) something much smaller than 0.10M (b)0.40 M (c)0.10 M (d) 0.20M (e)zero M

7. This mixture will establish equilibrium in mere fractions of a second. After it does, what will be the concentration of S2-?

Answers and explanations to any of the questions above would be very helpful.

Solutions

Expert Solution

You have 100. mL of aqueous 0.40 M CuSO4 mixed with 100. mL of aqueous 0.20 M Na2S.

1. What kind of reaction could potentially take place?

ions present:

Cu2+; SO4-2; Na+ + S-2

note that cu2+ and S-2 are not souble they form CuS

(a) Bronsted-Lowry acid base (b) redox (c) precipitation (d) no reaction

2. Which of the following is/are the spectator ions in this reaction? (a) SO42-   (b) Na+   (c) S2-   (d) Cu2+

spectator ions --> must not react , they remain in solution, so

SO4-2 and Na+ are not reacting, those are spectator ions

(a) SO42-   (b) Na+   (c) S2-   (d) Cu2+

3. After the solutions are mixed, what will be the concentration of Na+ ?

Vtotal = 100+100 = 200 mL

[Na+] = 0.2*2 = 0.4 M initially after 50% dilution -_> 0.2 M

(a) 0.10M (b) 0.80M (c) 0.20M (d) 0.40M (e) something else

4. After the solutions are mixed, what will be the concentration of  SO42- ?

SO4-2 iniailly --> 0.40

when halved --> 0.20 M

(a) 0.40M (b) 0.20M (c) 0.80M (d) 0.10

5. Which reactant will limit the amount of product that can form?

the limiting reactant --> Na2S, since 0.2 M and th eother species is 04 M

(a) Cu2+  (b) S2-  (c) something else


Related Solutions

400. mL of 0.5875 M aqueous silver nitrate are mixed with 500. mL of 0.290 M...
400. mL of 0.5875 M aqueous silver nitrate are mixed with 500. mL of 0.290 M sodium chromate. a) What is the mass of the precipitate? b) What is the concentration of each of the ions remaining in solution? Indicate any assumptions or approximations.
100 mL of .220 M copper ll chloride is mixed with 100 mL of .750 M...
100 mL of .220 M copper ll chloride is mixed with 100 mL of .750 M sodium hydroxide according to the following equation: CuCl2 + 2NaOH -->Cu(OH)2 + 2NaCl 1. What is the mass of solid product formed? 2. Calculate the concentration of Cu2+ remaining in solution. 3. Calculate the concentration of OH- remaining in solution. 4. Calculate the concentration of Cl- remaining in solution 5. Calculate the concentration of Na+ remaining in solution.
A 100. ml sample of 0.10 M HCl is mixed with 50. ml of 0.10 M...
A 100. ml sample of 0.10 M HCl is mixed with 50. ml of 0.10 M NH3. What is the resulting pH? Thank you!
When 200. mL of 0.40 M hydrochloric acid solution is mixed with 3.76 g of aluminum...
When 200. mL of 0.40 M hydrochloric acid solution is mixed with 3.76 g of aluminum metal, how many moles of hydrogen gas would be produced? 6HCl(aq) + 2Al(s) → 2AlCl3(aq) + 3H2(g)
A 100 mL solution of .400 M Sodium Acetate (NaOAc) mixed with 100 ml of .400 M HCl.
Determine the [H3O+] and [OH-] for the following: A 100 mL solution of .400 M Sodium Acetate (NaOAc) mixed with 100 ml of .400 M HCl.
1. You need 100 mL of 10% (W/V) CuSO4 (FW 160), but only CuSO4 * H2O...
1. You need 100 mL of 10% (W/V) CuSO4 (FW 160), but only CuSO4 * H2O is available. 2. A procedure requires the use of a 10% (W/V) sodium carbonate (FW 106). Prepare 200 mL using the monohydrate form. 3. Prepare 1 mmol/L Lithium standard from lithium carbonate (Li2CO3). Give the quantity in mg/L.
You have 500.0 mL of a buffer solution containing 0.20 M acetic acid and 0.30 M...
You have 500.0 mL of a buffer solution containing 0.20 M acetic acid and 0.30 M sodium acetate. What will the pH of the solution be after the addition of 20.0 mL of 1.00 M NaOH solution. Ka (CH3COOH) = 1.8x105 Please answer the question using ICE tables, I am unsure of whether to use 1 ICE table or 2 ICE Tables. Thank you.
375 mL of a .150 M aqueous solution of silver (1) nitrate is mixed with 125...
375 mL of a .150 M aqueous solution of silver (1) nitrate is mixed with 125 mL of .125 M aqueous solution of sodium phosphate. Calculate the mass of precipitate that forms and the final concentration of each ion in the mixed solution. Volumes are additive and the precipitation reaction goes to completion.
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100...
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100 M HCl. Determine the pH after addition of: 0 ml of HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, and 250 mL of HCl.
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100...
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100 M HCl. Determine the pH after addition of: 0 ml of HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, and 250 mL of HCl.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT