A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nintric acid,500. mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Is the resulting solution neutral? If not, calculate the concentration of excess H+ or OH- ions left in solution.

Calculate mols H^+ from the acids and mols OH^- from the bases. Total H^+ and total OH^- and you'll know which is the larger. Subtract one from the other to see which is in excess and by how much.

Thank you so much! this is a lot easier than the way I was originally trying to solve it

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To determine whether the resulting solution is neutral or not, we need to calculate the concentration of H+ and OH- ions left in the solution.

First, let's calculate the moles of each reagent using the formula:

moles = concentration (M) × volume (L)

For hydrochloric acid:
moles of HCl = 0.100 M × 0.0500 L = 0.005 moles HCl

For nitric acid:
moles of HNO3 = 0.200 M × 0.100 L = 0.020 moles HNO3

For calcium hydroxide:
moles of Ca(OH)2 = 0.0100 M × 0.500 L = 0.005 moles Ca(OH)2

For rubidium hydroxide:
moles of RbOH = 0.100 M × 0.200 L = 0.020 moles RbOH

Now, let's look at the neutralization reactions that occur:

HCl + NaOH → H2O + Cl-
HNO3 + NaOH → H2O + NO3-
Ca(OH)2 → Ca2+ + 2OH-
RbOH → Rb+ + OH-

From these reactions, we can see that H+ ions from HCl and HNO3 will react with OH- ions from Ca(OH)2 and RbOH to form water (H2O). Therefore, the excess of either H+ or OH- ions will determine if the resulting solution is neutral or not.

Since the moles of H+ ions from HCl and HNO3 are equal to the moles of OH- ions from Ca(OH)2 and RbOH, the resulting solution will be neutral.

In other words, there are no excess H+ or OH- ions left in the solution, and the resulting solution is neutral.