If the following solutions are mixed, is the resulting solution acidic, basic, or neutral?
1)65.0 mL of 0.0500 M HClO4 and 40.0 mL of 0.0750 M NaOH
2)125.0 mL of 0.100 M HNO3 and 80.0 mL of 0.0750 M Ca (OH) 2
1)
Mol of HClO4 added = M(HClO4)*V(HClO4)
= 0.0500 M * 65.0 mL
= 3.25 mmol
Mol of NaOH added = M(NaOH)*V(NaOH)
= 0.0750 M * 40.0 mL
= 3.00 mmol
Mol of H+ is more than mol of OH-.
So, the solution would be acidic
Answer: Acidic
2)
Mol of HNO3 added = M(HNO3)*V(HNO3)
= 0.100 M * 125.0 mL
= 12.5 mmol
Mol of Ca(OH)2 added = M(Ca(OH)2)*V(Ca(OH)2)
= 0.0750 M * 80.0 mL
= 6.0 mmol
1 mol of Ca(OH)2 has 2 mol of OH-
So,
Mol of OH- = 2*6.0 mmol = 12 mmol
Mol of H+ is more than mol of OH-.
So, the solution would be acidic
Answer: Acidic
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