Which ion, K^+ or Cl^-, influences the solubility of KHT? Briefly explain. Suppo

Question

Which ion, K^+ or Cl^-, influences the solubility of KHT? Briefly explain. Suppose this experiment were performed using NaBr-KBr solutions instead of the NaCl-KCl solutions. Would you expect different results? Briefly explain. Would the results be different if NaCl-LiCl solutions were used in this experiment, instead of the NaCl-KCl solutions? Briefly explain. If KHT did not dissociate when dissolved in aqueous solution, what effect would added KCl solution have on KHT solubility? Briefly explain. The solubility of KHT in water increases with increasing temperature. What effect would an increase in temperature have on the experimentally determined K_sp of KHT? Briefly explain.

Explanation / Answer

b)

K+ or Cl-:

Only K+ influences, since it will shift:

KHT <-> K+ + HT-

which is the common ioni in equilibrium

Q2

a)

Not really, since Br- and Cl- are not par of th eequilibrium

b)

Yes, since there is Li vs. K presence, therefore equilibirum will shift

Q3

if KHT wont dissociate, KCl solution will lower solubility, and favour solid production

Q4

Typically, Increasing T increases solubility

so Ksp will increase

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