Chemistry Question?

Question

1.

a.What is the molarity of a solution of nitric acid if .216 g of barium hydroxide is required to neutralize 20 mL of nitric acid?

b. A lead storage battery needs sulfuric acid to function. The recommended minimum concentration of sulfuric acid for maximum effectivity is about 4.8 M. A 10 mL sample of battery acid requires 66.52 mLof 1.325 M KOH for its complete neutralization. Does the concentration of battery acid satisfy the minimum requirement? (Note: Two H+ ions are produced for every mole of H2SO4.)

Please explain/show all work.

Answer 1

The reaction is Ba(OH)2 + 2HNO3 -> Ba(NO3)2 + 2H2O; therefore one mole of Ba(OH2)2 will neutralize two moles of HNO3. The molecular mass of Ba(OH2) is 171.34 g/mole so 0.216g of Ba(OH)2 is 0.12/171.34 mole or 0.0007mole. That means there were 0.00035moles of HNO3 in the 20mL solution, or 0.0175 moles/liter or 0.0175M.

The battery acid reaction is H2SO4 + 2KOH -> 2H2O + K2SO4. Two moles of KOH are required to neutralize one mole of H2SO4. Your solution of KOH is 1.325M or 1.325 mole/liter. In 66.52 mL (0.06652L) there are 0.06652*1.325=0.088139 moles of KOH. This will neutralize half that, or 0.04407 moles of H2SO4. That was in 10mL of battery acid, so the molarity of that was 0.04407/0.01 = 4.407M, which is less than 4.8

Answer 2

to find the molarity of something the equation is

Moles of solute/Liters of solution equals Molarity

or in lamen's terms
Moles of solute divided by Liters of solution equals Molarity

however im not sure about the neutralization part sorry!