Question

A volume of 30.2 mL of a 2.66 M KMnO4 solution is mixed with 14.7 mL...

A volume of 30.2 mL of a 2.66 M KMnO4 solution is mixed with 14.7 mL of a 0.392 M KMnO4 solution. Calculate the concentration of the final solution.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 180.0 mL solution of 2.172 M strontium nitrate is mixed with 220.0 mL of a...
A 180.0 mL solution of 2.172 M strontium nitrate is mixed with 220.0 mL of a 2.634 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. and then Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a zero for the concentration.
A solution of 116 mL of 0.170 M KOH is mixed with a solution of 300...
A solution of 116 mL of 0.170 M KOH is mixed with a solution of 300 mL of 0.200 M NiSO4. What is the concentration of Ni2+ that remains in solution? What is the concentration of SO2−4 that remains in solution? What is the concentration of K+ that remains in solution?
Using 0.200 ml H2O2 10 mL H2SO4 (aq) 1 M Solution titrated with KMnO4(aq) 0.20M In...
Using 0.200 ml H2O2 10 mL H2SO4 (aq) 1 M Solution titrated with KMnO4(aq) 0.20M In the reaction of the redox pairs MnO4- | Mn2+ and H2O2 | O2. Show reaction scheme and calculate the formal concentration c(H2O2)
Using 0.200 ml H2O2 10 mL H2SO4 (aq) 1 M Solution titrated with KMnO4(aq) 0.20M In...
Using 0.200 ml H2O2 10 mL H2SO4 (aq) 1 M Solution titrated with KMnO4(aq) 0.20M In the reaction of the redox pairs MnO4- | Mn2+ and H2O2 | O2. Show reaction scheme and calculate the formal concentration c(H2O2) 35% h2o2 and density=1.126 g/ml
73.0 mL of a 1.60 M solution is diluted to a total volume of 288 mL....
73.0 mL of a 1.60 M solution is diluted to a total volume of 288 mL. A 144 mL portion of that solution is diluted by adding 129 mL of water. What is the final concentration? Assume the volumes are additive. Determine the concentration of each of the individual ions in a 0.350 M K2SO4 solution. A 0.110 L sample of an unknown HNO3 solution required 51.1 mL of 0.200 M Ba(OH)2 for complete neutralization. What was the concentration of...
62.0 mL of a 1.80 M solution is diluted to a total volume of 278 mL....
62.0 mL of a 1.80 M solution is diluted to a total volume of 278 mL. A 139-mL portion of that solution is diluted by adding 177 mL of water. What is the final concentration? Assume the volumes are additive.
52.0 mL of a 1.70 M solution is diluted to a total volume of 258 mL....
52.0 mL of a 1.70 M solution is diluted to a total volume of 258 mL. A 129-mL portion of that solution is diluted by adding 109 mL of water. What is the final concentration? Assume the volumes are additive.
61.0 mL of a 1.80 M solution is diluted to a total volume of 238 ML....
61.0 mL of a 1.80 M solution is diluted to a total volume of 238 ML. A 119 mL portion of that solution is diluted by adding 111 mL of water. What is the final concentration? Assume the volumes are additive.
62.0 mL of a 1.50 M solution is diluted to a total volume of 258 mL....
62.0 mL of a 1.50 M solution is diluted to a total volume of 258 mL. A 129-mL portion of that solution is diluted by adding 187 mL of water. What is the final concentration? Assume the volumes are additive.
A 430. mL solution of 0.230 M HBr(aq) is mixed with a solution of 225 mL...
A 430. mL solution of 0.230 M HBr(aq) is mixed with a solution of 225 mL of 0.350 M HClO4(aq). How many moles of H+(aq) are present in the final solution?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT