Question

calculate the concentration of a cyanide ions in a solution that is 0.70 M in HCN...

calculate the concentration of a cyanide ions in a solution that is 0.70 M in HCN and 0.10 M in HI? (Ka = 4.9*10^-10)

Homework Answers

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
Calculate the p H of a 0.10 M solution of NaCN. HCN has Ka = 4.9...
Calculate the p H of a 0.10 M solution of NaCN. HCN has Ka = 4.9 x 10-10
Calculate the PH of an aqueous solution at 298 K that is 0.095 M in (HCN)....
Calculate the PH of an aqueous solution at 298 K that is 0.095 M in (HCN). (Ka for HCN = 4.9 x 10^-10)
sodium cyanide is the salt of the weak acid HCN. Calculate the concentration of H30+, oh-,HCN,...
sodium cyanide is the salt of the weak acid HCN. Calculate the concentration of H30+, oh-,HCN, and Na+ in a solution prepared by dissolving 10.8 g of NaCN in enough water to amke 5.00E2 ml of solution at 25C
sodium cyanide is the salt of the weak acid HCN. Calculate the concentration of H3), OH,...
sodium cyanide is the salt of the weak acid HCN. Calculate the concentration of H3), OH, HCN, and NA in a solution prepared by dissolving 10.8 g of NaCN in enough water to make 5.00x10^2 ml of solution at 25 degrees celsius
sodium cyanide is the salt of the weak acid HCN. Calculate the concentration of H3), OH,...
sodium cyanide is the salt of the weak acid HCN. Calculate the concentration of H3), OH, HCN, and NA in a solution prepared by dissolving 10.8 g of NaCN in enough water to make 5.00x10^2 ml of solution at 25 degrees celsius
Calculate the concentrations of the species (HCN, H+, CN-and OH-)and pH in 0.65M HCN solution (Ka=...
Calculate the concentrations of the species (HCN, H+, CN-and OH-)and pH in 0.65M HCN solution (Ka= 4.9 x 10-10)
Find the pH of 0.180 M NaCN solution. For HCN, Ka=4.9⋅10^−10
Find the pH of 0.180 M NaCN solution. For HCN, Ka=4.9⋅10^−10
Calculate the concentration of H3O(aq) ions present at equilibrium in a solution that is prepared by...
Calculate the concentration of H3O(aq) ions present at equilibrium in a solution that is prepared by mixing 100 mL of .35 M HCN and 200 mL of .15 M NaCN. Kc= 6.2E-10 HCN(aq) + H2O <---> H3O(aq) + CN(aq) (this is an equation from a previous question used for this question also) Please so all work! Thanks!
1). Calculate the pH and the concentration [Na+] =of all species in 3.5×10−2 molar sodium cyanide...
1). Calculate the pH and the concentration [Na+] =of all species in 3.5×10−2 molar sodium cyanide solution. [Na+] = ___ M H+] = ___M pH = ___M [OH−] =___M [CN−] = ___M [HCN]= ___M
Calculate the pH of a 0.1 M NaCN solution. Ka of HCN = 6.2 x10 -10....
Calculate the pH of a 0.1 M NaCN solution. Ka of HCN = 6.2 x10 -10. Please explain and/or show work.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT