Determine the speciation of manganese when 2 x 10-6 M TOT Mn (II) added to water at pH 6 and at pH 9. Assume that the manganese does not participate in any redox reactions but remains wholly as MnII. Use data in table 9.3 below. Is Mn (II) more likely to complex with hydroxide at pH 6 or pH 9? Feel free to check your answer with Visual Minteq.
2. Based on these results, to what oxidation states did the Mnchange in each test tube?
Mn
a
Test tube 3
+6
b
Test tube 4
+4
c
Test tube 5
+2
3. Write the net ionic equations for the redox reactions in eachtest tube: Referring to the table in the background of the lab manual may behelpful.
a
Test tube 3
b
Test tube 4
c
Test tube 5
Need help with #3
Here is the rough procedure
First we obtained 5 test tube, We filled the first test tubewith 5Ml of water, the second with 5mL of 0.02M PotassiumPermanganate , and the third, fourth, and fifth with 9mL of thepotassium Permanganate.
Next we added 1mL of 2m sodium hydroxide to test tube 3 and 1mLof 3m sulfuric acid to test tube 5. We then recorded the pH of allthe test tubes
1: 7
2: 7
3: 14
4: 7
5: 1.27
Next, we aquired a beaker and a dropper and added 20mL of 0.1Msodium bisulfite to the beaker
Two drops of Sodium bisulfite at a time added to test tube 3
The test tube3, turned green as compated to the first test tube...oxidation state +6
In Test tube 4, The color changed to clear as water and a blacksolid formation occured .. oxidation state +4
In test tube 5, the solution turned a pale pink indicating anoxidation state of +2
Which of the following balanced molecular equations represent reactions for which the rate law expression could likely be determined via time to turbidity determinations? Select all that apply.
a.
2 KI (aq) + Pb(NO3)2 (aq) ---> PbI2 (s) + 2 KNO3 (aq)
When working in the laboratory a small amount of 0.30 M sodium thiosulfate accidentally splashes on your exposed forearm. What should you do? Select all that apply.
a.
Inform your lab instructor.
b.
Proceed immediately to the sink in the laboratory and flush the area with copious amounts of water. Then wash the area with mild hand soap.
c.
Leave the laboratory immediately. All lab work is over for you today.
d.
Do nothing.
e.
Stop, drop, and roll.
QUESTION 4
volume of 1.0 M HCl
volume of water
volume of 0.3 M Na2S2O3
well 1
2.0 mL
0
3.0 mL
well 2
2.0 mL
1.5 mL
1.5 mL
well 3
2.0 mL
2.0 mL
1.0 mL
The above table summarizes the amounts and concentrations of the reactants that will be used in each trial in Parts II. Use the dilution equation, M1V1 = M2V2, to calculate the concentration Mf (molarityfinal) of Na2S2O3 in each well after mixing but before any reaction occurs. The [HCl] has been worked for you as an example.
M1(HCl)V1 = M2(HCl)V2 where V2 = final total volume Vf
(1.0 M)(2.0 mL) = M2(HCl)(5.0 mL)
M2(HCl) = 0.40 M = Mf(HCl)
- a. b. c. d. e. f.
well 1 Mf
- a. b. c. d. e. f.
well 2 Mf
- a. b. c. d. e. f.
well 3 M
a.
0.090 M
b.
0.18 M
c.
0.60 M
d.
0.20 M
e.
0.060
f.
0.30 M
QUESTION 1 10.00000 points Save Answer The following data were collected at 20 °C for the reaction of bromophenol blue (HBPB2) and hydroxide ions (OH-) HBPB (a)+ OH (a)BaH20( The times required to form a constBPB at varying initial concentrations of reactants were determined and tabulated. From the rate data, determine the rate law for the reaction rialHBPB2 reaction time (sec) rate (1/sec) 6 .6 .6 75 290 152 11.00 7.22 x 10 2 0.25 7.22 x 10 3 1.00 3.63 x 10" atekHBPB2120H] rate k[HBPB rate kHBPB20H] rate = k[HBPB2-110H72 QUESTION 2 20.00000 points Save Answer Which of the following balanced molecular equations represent reactions for which the rate law expression could likely be determined via time to turbidity determinations? Select all that apply a. 2 Kl (ag) + Pb(NO3)2 (a)Pbl2 (s) + 2 KNO3 (ag)
