Question

Suppose a 500.0 mL solution contains 1.25 millimoles of Co(NO3)2, 125.0 millimoles of NH3, and 100.0...

Suppose a 500.0 mL solution contains 1.25 millimoles of Co(NO3)2, 125.0 millimoles of NH3, and 100.0 millimoles of ethylenediamine. What is the concentration of Co2+(aq) in the 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
consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of...
consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3. Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2^+. K1= 2.1x10^3; K2=8.2x10^3, what is the concentration of Ag(NH3)2^+ at equilibrium?
100.0 mL of a Pb(NO3)2 solution was concentrated to 80.0 mL. To 2.00 mL of the...
100.0 mL of a Pb(NO3)2 solution was concentrated to 80.0 mL. To 2.00 mL of the concentrated solution was added an excess of NaCl(aq), and 3.407 g of a solid was obtained. What was the molarity of the original Pb(NO3)2 solution? The "To 2.00mL of the concentrated...an excess of NaCl" confuses me.
You mix a 125.0 mL sample of a solution that is 0.0100 M in NiCl2 with...
You mix a 125.0 mL sample of a solution that is 0.0100 M in NiCl2 with a 166.0 mL sample of a solution that is 0.253 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? (Formation constant is Kf=2.0×108.)
One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.500 M in...
One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.500 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×108 What is the initial concentration of Ni(NO3)2 in the solution? _____M What is the equilibrium concentration of Ni2+(aq ) in the solution? ______M
A 1.00 L solution contains 2.25×10-4M Cu(NO3)2 and 2.500×10-3M ethylenediamine (en). The Kf for Cu(en)22+ is...
A 1.00 L solution contains 2.25×10-4M Cu(NO3)2 and 2.500×10-3M ethylenediamine (en). The Kf for Cu(en)22+ is 1.00×1020. What is the concentration of Cu2+(aq ) in the solution?
One millimole of Ni(NO3)2 dissolves in 260.0 mL of a solution that is 0.400 M in...
One millimole of Ni(NO3)2 dissolves in 260.0 mL of a solution that is 0.400 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×108. b)What is the equilibrium concentration of Ni2+(aq ) in the solution?
A 1.0 L solution contains 3.00×10-4 M Cu(NO3)2 and 1.63×10-3 M ethylenediamine (en). The Kf for...
A 1.0 L solution contains 3.00×10-4 M Cu(NO3)2 and 1.63×10-3 M ethylenediamine (en). The Kf for Cu(en)22+ is 1.00×1020. What is the concentration of Cu2+(aq ) in the solution?
A 1.00 L solution contains 2.50×10^-4 M Cu(NO3)2 and 2.50×10^-3 M ethylenediamine (en). The Kf for...
A 1.00 L solution contains 2.50×10^-4 M Cu(NO3)2 and 2.50×10^-3 M ethylenediamine (en). The Kf for Cu(en)22+ is 1.00×10^20. What is the concentration of Cu2+(aq ) in the solution?
A buffer solution is prepared by mixing 50.0 mL of 0.300 M NH3(aq) with 50.0 mL...
A buffer solution is prepared by mixing 50.0 mL of 0.300 M NH3(aq) with 50.0 mL of 0.300 M NH4Cl(aq). The pKb of NH3  is 4.74. 7.50 mL of 0.125 M NaOH is added to the 100.0 mL of the original buffer solution prepared in Question 1 (no HCl added). Calculate the new NH3 concentration for the buffer solution. Calculate the new NH4Cl concentration for the buffer solution. Calculate the new pH of the solution.
Co(NO3)2 + 2 NH3 = Co(NH3)2 + 2 NO3 what is the net ionic equation?
Co(NO3)2 + 2 NH3 = Co(NH3)2 + 2 NO3 what is the net ionic equation?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT