# Chemistry

The S^2- ion is a relatively strong base with an equilibrium constant of 7.7x10^-1.
What is the Ka value for HS- ?

I got the equation HS^- <-> H^+ + S^-2. Am I able to find [S^-2] with the Keq?

1. 👍 0
2. 👎 0
3. 👁 130
1. I think Ka = Kw/Kb. I'm not sure what you mean by S%2= ion has eq const of 0.77. Is that Kb?

1. 👍 0
2. 👎 0
posted by DrBob222
2. S^-2 ion has equilibrium constant of 7.7x10^-1

So it's just (1.00x10^-14)/(0.77)=1.3x10^14 = Ka HS^- ?

1. 👍 0
2. 👎 0
posted by sh
3. If the equilibrium constant is the same as Kb, yes. But I'm not sure that it is. I've never seen an ION shown as an equilibrium constant.

1. 👍 0
2. 👎 0
posted by DrBob222

1. 👍 0
2. 👎 0
posted by sh

## Similar Questions

1. ### chemistry

Hi there, ok, my question stated "Use information from acid/base table and the value of Kw t ocalulate the base ionization constant, Kb, of the following bases: a)hypochlorite ion b) nitrite ion c) benzoate ion I looked at my

asked by Jay on April 8, 2008
2. ### AP Chemistry

Rank these compounds in order of increasing hyroxide ion concentration: weak base, weak acid, strong base, strong acid.

asked by Angie on January 11, 2010
3. ### math , steve or damon pls

for questions 15 and 16, multiply. write in scientific notation (9x10^4)(8x10^6) 7.2x10^25 1.7x10^11 7.2x10^11 1.7x10^25 (1.7x10^-4)(5x10^-5) 8.5x10^-9 8.5x10^20 6.7x10^-9 6.7x10^20 for 15 I'm thinking it is c and 16 could be A

asked by jacob :) on May 8, 2016
4. ### Chemistry

I am predicting acid-base equilibria using the Brondsted-Lowry predictions. I am asked to do "solid aluminum sulfate added to water". So I know there is an Al^2+ ion and a SO4^-2 ion, but does water dissociate into H30^+ and OH^-?

asked by Stuck on May 7, 2010
5. ### Chemistry

What is the equilibrium constant for the reaction of ammonium ion with formate ion? I know that the ionization constant for ammonium ion is Ka=5.6e-10 and for formate Kb=5.6e-11. a) 1.0 X 10-13 b) 5.6 X 10-11 c) 3.1 X 10-6 d) 1.8

asked by Mohamed on April 3, 2012
6. ### CHEMISTRY

Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid

asked by Alexander on November 9, 2011
7. ### Chemistry

Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid

asked by Alex on November 9, 2011
8. ### chemistry

Which of the following is true of the solubility product constant? A. It is the product of the initial concentrations of the ions in a solution. B. It is an equilibrium constant. C. It is an equilibrium position. D. Its value

asked by emma on September 10, 2016
9. ### chemistry help

Which of the following is true of the solubility product constant? A. It is the product of the initial concentrations of the ions in a solution. B. It is an equilibrium constant. C. It is an equilibrium position. D. Its value

asked by emma on September 10, 2016
10. ### Chemistry(Thank you for your help)

What is the equilibrium constant for the reaction of ammonium ion with formate ion? I know that the ionization constant for ammonium ion is Ka=5.6e-10 and for formate Kb=5.6e-11. I am not sure what to do next. Should I divide ka

asked by Hannah on April 2, 2012

More Similar Questions