A student mixes 4 reagents together thinking that the solution will neutralize each other . The solutions are mixed together are 50 ml of 0.100 M .hydrochloric acid 100 ml of 0.200 M of nitric acid 500 ml of 0.0100 M calcium hydroxide and 200 ml of 0.100 M of rubidium hydroxide did the acid and bases exactly neutralize each other If not calculate the concentration of excess H+ or OH- ions left solution
What's your problem here Mathew? You calculate mols H^+ and mols OH and see where you stand.
To determine if the acid and bases exactly neutralize each other, we need to compare the number of moles of H+ ions from the acids and the number of moles of OH- ions from the bases.
First, let's calculate the number of moles of H+ ions from the acids:
Number of moles of H+ ions from hydrochloric acid = volume (in liters) x concentration
= 0.050 L x 0.100 mol/L
= 0.005 mol H+
Number of moles of H+ ions from nitric acid = volume (in liters) x concentration
= 0.100 L x 0.200 mol/L
= 0.020 mol H+
Next, let's calculate the number of moles of OH- ions from the bases:
Number of moles of OH- ions from calcium hydroxide = volume (in liters) x concentration
= 0.500 L x 0.0100 mol/L
= 0.005 mol OH-
Number of moles of OH- ions from rubidium hydroxide = volume (in liters) x concentration
= 0.200 L x 0.100 mol/L
= 0.020 mol OH-
Now, let's compare the moles of H+ ions and OH- ions:
Total moles of H+ ions = 0.005 mol + 0.020 mol = 0.025 mol
Total moles of OH- ions = 0.005 mol + 0.020 mol = 0.025 mol
Since the number of moles of H+ ions is equal to the number of moles of OH- ions, we can conclude that the acid and bases exactly neutralize each other. There is no excess H+ or OH- ions left in the solution.