Question

Calculate the molarity of S2O32− if 3.0 mL 0.10 M K2S2O8, 2.0 mL 0.10 M K2SO4,...

Calculate the molarity of S2O32− if 3.0 mL 0.10 M K2S2O8, 2.0 mL 0.10 M K2SO4, 1.0 mL 2% starch, 2.0 mL 0.010 M Na2S2O3, and 5.0 mL 0.20 M KI are mixed. (Include units in your answer)

Homework Answers

Answer #1

The S2O32- ONLY can come from the Na2S2O3 since nothing else has it (in other problems, the material you are asked to find the concentration may come from more than 1 of the compounds).

Equation 1: 2 I - (aq) + S2O82- (aq) --> I2 (aq) + 2 SO42- (aq)

Equations 2: (very fast) I2(aq) + 2 S2O32- (aq) --> 2I - (aq) + S4O62- (aq)


1 mL = 0.001 L
2 mL = 0.002 L
0.010 M Na2S2O3 = 0.010 mole/L Na2S2O3

0.010 mole/L * 0.002 L = 2*10-5 mole Na2S2O3

2*10-5 mole of Na2S2O8 contains mole 2*10-5 mole of S2O32− from the chemical formula.

Total volume =  3 mL + 2 mL + 1 mL + 2 mL + 5 mL = 13 mL = 0.013 L


Concentration of S2O32− = 2*10-5mole / 0.013 L = 0.0015 M

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
3. (a) Calculate the volume of 0.5 M BaCl2, required for complete precipitation of 2.0 mL...
3. (a) Calculate the volume of 0.5 M BaCl2, required for complete precipitation of 2.0 mL of the unknown solution (K2SO4) if its concentration is 0.10 M. (b) Calculate the volume of reagent required for complete precipitation of 2.0 mL of the unknown solution (K2SO4) if its concentration is 1.0 M. (c) If it turns out that about 1.5 mL of precipitating reagent is required for complete precipitation of 2.0 mL of unknown solution (K2SO4), what is its approximate concentration?...
A solution is made by combining 50 mL 1.0 M carbonic acid, 2.0 mL 5.0 M...
A solution is made by combining 50 mL 1.0 M carbonic acid, 2.0 mL 5.0 M KOH and 448 mL pure water (assume the total volume is 500 mL). The pKa of carbonic acid is 6.35. Calculate the pH of the resulting solution.
1.Calculate the rate of reaction for the solution to turn from colorless to blue-black after each...
1.Calculate the rate of reaction for the solution to turn from colorless to blue-black after each addition. Volume Added to Solution 1 Reaction time (s) Total Volume (L) Rate (mol/L·s) 25 mL (NH4)2S2O8 69 .100 .032 1 mL Na2S2O3 105 .101 9.96X10^-4 1 mL Na2S2O3 80 .102 .0013 1 mL Na2S2O3 75 .103 .0014 2.What is the average rate of the reaction for Solution 1 (include units)?                   .009 mol/L*s               3.What is the concentration of KI and (NH4)2S2O8...
Calculate the molarity of each of the following solutions. Part A 0.43 mol of LiNO3 in...
Calculate the molarity of each of the following solutions. Part A 0.43 mol of LiNO3 in 6.44 L of solution Express your answer using two significant figures. molarity = M   Part B 11.45 mg KI in 114.8 mL of solution Express your answer using four significant figures. molarity =   M  
1. Which of the following balanced molecular equations represent reactions for which the rate law expression...
1. 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. 3 SrCl2 (aq) + 2 Li3PO4 (aq) ---> Sr3(PO4)2 (s) + 6 LiCl (aq) b. 2 HBr (aq) + Ca(OH)2 (aq) ---> 2 H2O (l) + CaBr2 (aq) c. FeS (s) + HCl (aq) ---> FeCl2 (aq) + H2S (g) d. 2 NO (g) + 5 H2 (g) ---> 2...
  20. Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of...
  20. Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00    [A] 1.0 ⋅ 10-9 [B] 1.0 ⋅ 10-5 [C] 9.0 ⋅ 10-14 [D] 9.00 [E] 5.0 ⋅10-14       21. What is the pOH of an aqueous solution at 25.0 °C that contains 3.98 ⋅ 10-9 M hydronium ion?    [A] 9.000 [B] 5.600 [C] 3.980 [D] 7.000 [E] 8.400 22. Which solution will be the most basic? [A] 0.20 M Sr(OH)2...
Calculate the pH at the equivalence point when 10.0 mL of 0.10 M HC9H7O2 (Ka =...
Calculate the pH at the equivalence point when 10.0 mL of 0.10 M HC9H7O2 (Ka = 3.6 × 10–5) is titrated against 0.20 M sodium hydroxide
Calculate the volume (mL) of 1.0 M metal nitrate solution required to prepare 3.0 g of...
Calculate the volume (mL) of 1.0 M metal nitrate solution required to prepare 3.0 g of CaCO3. Again, using the balanced chemical equation you should be able to relate the moles of pigment to the moles of metal nitrate and from that calculate the volume of 1.0 M metal nitrate solution required. Balanced equation: Ca(NO3)2 (aq) + K2CO3 (aq) ↔ CaCO3 (s) + 2KNO3 (aq)
40.0 mL of 2.0 M Fe(NO3)3 is mixed with 2 mL of 5 M Fe(NO3) and...
40.0 mL of 2.0 M Fe(NO3)3 is mixed with 2 mL of 5 M Fe(NO3) and 48 mL of water. What is the final molar concentration of Fe(NO3)? Answer is 1M but how do we get this solution? Please help.
Solution Volume of 0.20 M Fe3+ Volume of 0.002 M SCN- Volume of H2O A-1 25.0...
Solution Volume of 0.20 M Fe3+ Volume of 0.002 M SCN- Volume of H2O A-1 25.0 mL 0.0 mL 75.0 mL A-2 25.0 mL 5.0 mL 70 mL A-3 25.0 mL 7.0 mL 68.0 mL A-4 25.0 mL 9.0 mL 66.0 mL A-5 25.0 mL 11.0 mL 64.0 mL Solution Volume of 0.002 M Fe3+ Volume of 0.002 M SCN- Volume of H2O B-1 5.0 mL 1.0 mL 5.0 mL B-2 5.0 mL 2.0 mL 4.0 mL B-3 5.0 mL...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT