Question

In: Chemistry

26. A solution of 0.075 M CoBr2 is saturated with H2S ( [H2S] = 0.10 M)....

26.

A solution of 0.075 M CoBr2 is saturated with H2S ( [H2S] = 0.10 M). What is the minimum pH at which CoS ( Ksp = 5.9 x 10 -21) will precipitate?
Ka1 =8.9 x 10 -8 & Ka2 = 1.2 x 10 -13 for H2S and Ksp for CoS = 5.9 x 10 -21

Solutions

Expert Solution

Answer:

Given:-

In satutated solution of CoS the solubility equilibrium exist as

...(A)

The solubility product for eq(A) is

ie.

Hence,

Ie. The precipitate of CoS will form only if [S2-] exceeds the concentration of

Now, The first dissociation of H2S is

Ka1 is

ie. ...(1)

Second Dissociation of H2S is

Ka2 is

ie. ...(2)

from eq(1) and (2) we have,

ie. ...(3)

Now putting the values in eq(3) we get,

ie.

  

Taking square root of both side we get,

Now,

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

26. A solution of 0.075 M CoBr2 is saturated with H2S ( [H2S] = 0.10 M)....
26. A solution of 0.075 M CoBr2 is saturated with H2S ( [H2S] = 0.10 M). What is the minimum pH at which CoS ( Ksp = 5.9 x 10 -21) will precipitate? Ka1 =8.9 x 10 -8 & Ka2 = 1.2 x 10 -13 for H2S Ksp for CoS = 5.9 x 10 -21
A solution containing 0.10 M Zn2+ and 0.10 M Fe2+ is saturated with H2S (i.e. 0.10...
A solution containing 0.10 M Zn2+ and 0.10 M Fe2+ is saturated with H2S (i.e. 0.10 M H2S). (a) What must the H+ concentration be to separate these ions by selectively precipitating ZnS? Note: ZnS has Ksp=1.2x10-23; FeS has Ksp=3.7x10-19. (b) What is the smallest concentration of Zn2+ that can be achieved without precipitating any of the Fe2+ as FeS?
1. 0.075 moles of LiF is added to 1 L of a saturated solution of BaF2....
1. 0.075 moles of LiF is added to 1 L of a saturated solution of BaF2. a) write the ksp reaction and expression for BaF2. explain b) what is the molar solubility of the BaF2 in the solution with the added LiF? explain 2. A saturated solution of silver chloride is in equilibrium with solid silver chloride. These reagents are added to seperate portions of the mixture. What effect (if any) with each of them have on the amount of...
A 500.0 mL buffer solution is 0.10 M in benzoic acid and 0.10 M in sodium...
A 500.0 mL buffer solution is 0.10 M in benzoic acid and 0.10 M in sodium benzoate and has an initial pH of 4.19. What is the pH of the buffer upon addition of 0.020 mol of NaOH?
Which solution has the highest pH? a. 0.10 M NaF(aq) b. 0.10 M NaCl(aq) c.  0.10 M...
Which solution has the highest pH? a. 0.10 M NaF(aq) b. 0.10 M NaCl(aq) c.  0.10 M NaBr(aq) d. 0.10 M NaClO4(aq)
In the solution containing both 0.10 M acetic acid and 0.10 M sodium acetate, the acetic...
In the solution containing both 0.10 M acetic acid and 0.10 M sodium acetate, the acetic acid undergoes ionization. The chemical equation for this ionization reaction is the same as for a solution containing acetic acid alone. The difference is that the initial concentration of acetate ion (before any ionization reaction occurs) for the solution containing acetic acid alone is zero, whereas the initial concentration of acetate ion is 0.10 M in your solution containing both acetic acid and sodium...
1.) Consider a solution that is 0.10 M Acetic Acid (HC2H3O2) and 0.10 M Sodium Acetate (NaC2H3O2).
1.) Consider a solution that is 0.10 M Acetic Acid (HC2H3O2) and 0.10 M Sodium Acetate (NaC2H3O2).HC2H3O2 + H2O <---> C2H3O2- + H3O+a.) What happens if you add HCl (acid)?b.) What happens if you add NaOH (base)?2.) NH3 + H2O <---> NH4+ + OH-If you add HCl, which way will it shift?
calculate the percent ionization of ha in a 0.10 m solution.
A certain weak acid, HA, has a Ka value of 6.7 X 10^-7. Part A Calculate the percent ionization of HA in a 0.10 M solution. Express your answer to two significant figures and include the appropriate units. Part B Calculate the percent ionization of HA in a 0.010 M solution. Express your answer to two significant figures, and include the appropriate units.
An aqueous solution of formic acid, HCOOH, is prepared at 0.075 M. The acid-ionization constant is...
An aqueous solution of formic acid, HCOOH, is prepared at 0.075 M. The acid-ionization constant is Ka = 1.8 x 10-4. Because this is a weak acid, you may presume that the ionic strength is negligible (m = 0). Calculate: a) the pKa of HCOOH b) [H+] c) [HCOO-]   d) [HCOOH] at equilibrium
a 25.0 mL solution if 0.10 M acetic acid is titrated with 0.1 M NaOH solution....
a 25.0 mL solution if 0.10 M acetic acid is titrated with 0.1 M NaOH solution. the pH equivalence is
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT