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Using the following reaction

Mg(NO3)2(aq) + 2 NaOH (aq) --> Mg(OH)2 (s) + 2 NaNO3 (aq)

To 2.0 mL of 0.10 M Mg(NO3)2 in a test tube, 3.0 M NaOH is added dropwise

a) calculate the number of moles of Mg(NO3)2 in the solution

b) calculate othe volume in mL of NaOH which is needed to reat completley with the Mg(NO3)2

c) if one drop of the NaOH solution ahs a volume of 0.04 mL, how many drops of 3M NaOH are needded to react compeltely with the Mg(NO3)2?

please show all your work thanks. will upvote help

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Sixta Kovacek
Sixta KovacekLv2
29 Sep 2019
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Related questions

Part IV. 1. Zn(OH)2 (s) ⇌ Zn (aq) + 2 OH (aq) (This is the lab procedure)

2+ 2-
2. Zn (aq) + 4 OH (aq) ⇌ Zn(OH)4 (aq)

2+
3. Zn (aq) + 4 NH3 (aq) ⇌ Zn(NH3)4 (aq)

1. In a test tube add 2 mL 0.1M Zn(NO3)2. Add one drop of 6M NaOH and stir. Record your observations.

r. What is happening as NaOH is added?

2. Add more 6M NaOH dropwise until a change is observed. Record your observations.

s. What happened to the solid? What is now in the solution? Explain how the equilibrium of the complex ion reaction affected the equilibrium of the solid Zn(OH)2.
3. In a new test tube add 2 mL 0.1M Zn(NO3)2. Add one drop of 6M NH3 and stir. Record your observations. Add 2mL more 6M NH3 until a change is observed. Record your observations.

t. What happened to the solid? What is now in the solution? Explain how the equilibrium of the complex ion reaction affected the equilibrium of the solid Zn(OH)2. 4. In another new test tube add 2 mL 0.1M Zn(NO3)2. Add one drop of 6M NaOH and stir. Record your observations. Add 6M HCl dropwise until a change is observed. Record your observations.
.

5. In a test tube add 2 mL 0.1M Mg(NO3)2. Add one drop of 6M NaOH and stir. Record your observations.

u. What is happening as HCl is added? How is HCl affecting the equilibrium of Zn(OH)2?

2+ – Mg(OH)2 (s) ⇌ Mg (aq) + 2 OH (aq)

v. What is happening as NaOH is added?

6. Add 6M NaOH dropwise for 10 drops. Did a change happen? Record your observations.

w. What happened to the solid? Did magnesium (II) ion form a complex ion like Zn? How do you know? What is your evidence?

7. . In a new test tube add 2 mL 0.1M Mg(NO3)2. Add one drop of 6M NH3 and stir. Record your observations. Add 2 mL more 6M NH3. Record your observations.
x. What happened to the solid? Did magnesium (II) ion form a complex ion like Zn? How do you know? What is your evidence?

8. In another new test tube add 2 mL 0.1M Mg(NO3)2. Add one drop of 6M NaOH and stir. Record your observations. Add 6M HCl dropwise until a change is observed. Record your observations..

y. What is happening as HCl is added? How is HCl affecting the equilibrium of Mg(OH)2?

Part IV. - I need help having these questions answered.

Write the relevant (3) Zn equilibrium reaction(s) here: (0.75)

15.What happened as NaOH was added in a single drop to a Zn+2 solution? (0.25)

16. What happened to the Zn(OH)2 as excess NaOH was added? What is now in the solution? Using your observations as evidence and your understanding of LCP, explain how the equilibrium of the complex ion reaction affected the earlier equilibrium of the solid Zn(OH)2. Explain BOTH reactions equilibrium shifts. (0.75)

17. What happened as NH3 was added drop by drop to the Zn+2 solution? What happened when excess NH3 was added? What is now in the solution? Using your observations as evidence and your understanding of LCP, explain how the equilibrium of the complex ion reaction affected the earlier equilibrium of the solid Zn(OH)2. Explain BOTH reactions equilibrium shifts. (0.75)

18. What happened as HCl was added to the Zn(OH)2 equilibrium? What did the HCl react with? How did this reaction change the equilibrium position of reaction 1? (0.5)

5

Write the relevant Mg equilibrium reaction here: (0.25)
19. What happened as NaOH was added in a single drop to a Mg+2 solution? (0.25)

20. What happened to the Mg(OH)2 as more NaOH was added? Did Mg2+ form complex ion with OH-? Which way did equilibrium shift? (0.75)

21. What happened as NH3 was added by drop to the Mg+2 solution? What happened when excess NH3 was added? Did Mg2+ form complex ion with OH-? Which way did equilibrium shift? (0.75)

22. What happened as HCl was added to the Mg(OH)2 equilibrium? How did HCl affect the equilibrium of Mg(OH)2? Which way did equilibrium shift? (0.25)

NiCl2(aq)+2NaOH(aq)?Ni(OH)2(s)+2NaCl(aq)

1) How many milliliters of 0.165M NaOH are needed to react with34.5mL of 0.415M NiCl2?

2) How many grams of Ni(OH)2 are produced from the reaction of38.5mL of 1.78M NaOH?

Mg(s)+2HCl(aq)?MgCl2(aq)+H2(g)

3)How many milliliters of a 6.500M HCl solution are required toreact with 42.20g magnesium?

4) What volume of hydrogen gas, at 25.0 ?C and 689.3 torr, willform when 662mL of 4.76M HCl reacts with excess Mg?

5) How many g NO of gas can be produced from the reaction of129.0mL of 3.40M HNO3 and excess Cu?

3Cu (s) + 8HNO3 (aq) ? 3Cu(NO3)2 (aq) + 4H2O (l) + 2NO (g)

6) Calculate the final concentration of each of the followingdiluted solutions:

A) A 50.0mL sample of 8.00% (m/v) NaOH is diluted with water sothat the final volume is 200.0mL

B) A 8.00mL sample of 50.0% (m/v) acetic acid (HC2H3O2) solutionis added to water to give a final volume of 25.0mL .

This experiment involved mixing aqueous solutions of Cu(NO3)2(Copper nitrate) and KI (potassium iodide)

2 Cu(NO3)2 (aq) + 4 KI (aq) ---- > 2 CuI (s) + I2 (aq) +4KNO3 (aq)


You have two test tubes labeled A and B. Both test tubes havethe same solution in them. The solution is 2.0 mL of 0.50 MCu(NO3)2 and 5.0 mL of 0.50 M KI. After centrifuging the test tubesfor 5 minutes the preciptate (CuI) settles to the bottom. Thesupernatant is removed from each test tube and then the precipitateis dried. Once it is dry, the precipitate is weighed in each testtube. Test tube A ended up with a precipitate weighing 0.3 gramsand test tube B had a precipitate weighing 0.33 grams.

Given this information, calculate the following:

1.) average moles of product (CuI)


2.) average moles of Cu(NO3)2


3.) average moles of KI


4.) theoretical moles of product based Cu(NO3)2


5.) theoretical moles based on KI


6.) percent error in moles of CuI

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