0
answers
0
watching
94
views
17 Nov 2019
When the solution reaches equilibrium, the pH is 9.34 Explain why the pH increased above that of the pure water (7.0) Write the equation that would have so be solved to determined the equilibrium pH if the system had not been investigated experimentally. Assume the solution behaves ideally. When the system reaches equilibrium the concentration of the total dissolved Ca (TOT Ca) and total dissolved phosphate (TOTPO_4) are 3.54 Times 10^-5 M and 2.3 Times 10^-5 M, respectively. If an additional 1.0 L of pure water is added to the suspension and the system then re-equilibrates, will the pH increase, decrease or remain the same as before the water was added? Explain briefly.
When the solution reaches equilibrium, the pH is 9.34 Explain why the pH increased above that of the pure water (7.0) Write the equation that would have so be solved to determined the equilibrium pH if the system had not been investigated experimentally. Assume the solution behaves ideally. When the system reaches equilibrium the concentration of the total dissolved Ca (TOT Ca) and total dissolved phosphate (TOTPO_4) are 3.54 Times 10^-5 M and 2.3 Times 10^-5 M, respectively. If an additional 1.0 L of pure water is added to the suspension and the system then re-equilibrates, will the pH increase, decrease or remain the same as before the water was added? Explain briefly.