Precipitation calculations with Ni²⁺ and Pb²⁺ a. Use the solubility product for Ni(OH)₂ (s) . the pH at which Ni(OH)₂ begins to precipitate from a 0.18 M Ni²⁺ solution. (Ksp Ni(OH)₂ = 5.5x10⁻¹⁶) is 6.8.
When Ni(OH)₂ starts precipitate :
Ksp of Ni(OH)₂ = [ Ni²⁺ ] [ OH²⁻ ]
5.5x10⁻¹⁶ = [ 0.18 ] [ OH²⁻ ]
[ OH²⁻ ] = 5.5x10⁻¹⁶ / 0.18
[ OH⁻ ] = 5.5 × 10⁻⁸ M
pOH = 7.2
therefore , pH = 14 - 7.2
pH = 6.8
Thus, Precipitation calculations with Ni²⁺ and Pb²⁺ a. Use the solubility product for Ni(OH)₂ (s) . the pH at which Ni(OH)₂ begins to precipitate from a 0.18 M Ni²⁺ solution. (Ksp Ni(OH)₂ = 5.5x10⁻¹⁶) is 6.8.
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I believe the answer is C
Answer:
No.
Explanation:
During chemical reaction, atomes cannot be created or destroyed, they can only react together to form <em>E</em><em>l</em><em>e</em><em>m</em><em>e</em><em>n</em><em>t</em><em> </em>or <em>C</em><em>o</em><em>m</em><em>p</em><em>o</em><em>u</em><em>n</em><em>d</em><em> </em>at the <em>P</em><em>r</em><em>o</em><em>d</em><em>u</em><em>c</em><em>t</em><em> </em>side.
<span>The net ionic equation for the reaction of alum (KAl(SO4)2.12H2O.) and KOH is </span>the solid AlOH3 formed.
