HomeworkLib
Question

DeneutralizationofMPOawithKOHisenden 3H20()-K3 PO,(aq) +173.2 -K,Polaq)+173u H,PO,(aq) +3KOH(aq) kJ 60.0 mL of 0.200 M H3P04 is mixed with 60.0 mL of 0.600 M KOH initially at 23.91 ?. Predict the final temperature of the solution if its density is 1.13 g/mL and its specific heat is 3.78 Jfg?) Assume that the total volume is the sum of the individual volumes. Number final

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

reteased 10 12 23-3」 r C

0 0
Add a comment
Know the answer?
Add Answer to:
DeneutralizationofMPOawithKOHisenden 3H20()-K3 PO,(aq) +173.2 -K,Polaq)+173u H,PO,(aq) +3KOH(aq) kJ 60.0 mL of 0.200 M H3P04 is mixed...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • The neutralization of H3PO4 with KOH is exothermic. H3PO4(aq)+3KOH(aq)⟶3H2O(l)+K3PO4(aq)+173.2 kJ If 55.0 mL of 0.207 M...

    The neutralization of H3PO4 with KOH is exothermic. H3PO4(aq)+3KOH(aq)⟶3H2O(l)+K3PO4(aq)+173.2 kJ If 55.0 mL of 0.207 M H3PO4 is mixed with 55.0 mL of 0.620 M KOH initially at 23.29 °C, predict the final temperature of the solution, assuming its density is 1.13 g/mL and its specific heat is 3.78 J/(g·°C). Assume that the total volume is the sum of the individual volumes. ?final= °C

  • The neutralization of HPO with KOH is exothermic 4 Н, РО, (аq) + 3 КОНаq) 3 H2O(l) + K3PO4 (aq) 173.2 kJ If 65.0 mL of...

    The neutralization of HPO with KOH is exothermic 4 Н, РО, (аq) + 3 КОНаq) 3 H2O(l) + K3PO4 (aq) 173.2 kJ If 65.0 mL of 0.220 M H PO4 is mixed with 65.0 mL of 0.660 M KOH initially at 21.49 °C, predict the final temperature of the solution, assuming its density is 1.13 g/mL and its specific heat is 3.78 J/(g.°C). Assume that the total volume is the sum of the individual volumes 333.4 °C Trinal

  • A solution of 0.200 M KOH (17.6 mL) is mixed with 45.9 mL of 0.143 M...

    A solution of 0.200 M KOH (17.6 mL) is mixed with 45.9 mL of 0.143 M HCl. Assuming that the final volume is the sum of the initial volumes, calculate: (a) the molarity of the K+ cation (b) the molarity of the Cl- anion (c) the pH of the final solution (d) the pOH of the final solution

  • In a constant-pressure calorimeter, 60.0 mL of 0.300 M Ba(OH)2 was added to 60.0 mL of...

    In a constant-pressure calorimeter, 60.0 mL of 0.300 M Ba(OH)2 was added to 60.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 24.37 °C to 28.46 °C. If the solution has the same density and specific heat as water, what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes. Find kJ/mol of H20.

  • 4. A solution of 0.200 M NaOH (14.0 mL) is mixed with 42.4 mL of o.170...

    4. A solution of 0.200 M NaOH (14.0 mL) is mixed with 42.4 mL of o.170 M HNO,. Assuming that the final volume is the sum of the initial volumes, calculate: (a) the molarity of the Na* cation (b) the molarity of the NO, anion (c) the pH of the final solution (d) the pOH of the final solution

  • Enthalpy of Neutralization Reaction: A 25.0 mL sample of 0.200 M NaOH is mixed with a...

    Enthalpy of Neutralization Reaction: A 25.0 mL sample of 0.200 M NaOH is mixed with a 25.0 mL sample of 0.200 M HNO3 in a coffee cup calorimeter.  NaOH and HNO3 will undergo Neutralization Reaction according to the following balanced equation: NaOH(aq) +   HNO3(aq) --> NaCl (aq) +  H2O (l)   Both solutions were initially at 35.00°C and Tmax of the resulting solution was recorded as 37.00°C (from the graph). Assume 1) that no heat is lost to the calorimeter or the surroundings, and...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT