10 points if you help me with these Chemistry question!!!!?

Question

how would you solve this (not the answer but how you do the work)

25.0 mL of 0.05 M Ba(OH)2 (that is a subscript) neutralised 40.0 mL of nitric acid. Determine the concentration of the acid

please help me solve this question

Also what is the oxidation state of the nitrogen atom in N2O

Any ideas that one kinda confused me

Answer 1

Ba(OH)2(aq) + 2HNO3(aq) -----> Ba(NO3)2(aq) + 2H2O(l)



Moles of Ba(OH)2:

n = MV = 0.05*25.0 x 10-3 = 1.25 x 10^-3 mol



The stoichometric ratio is= Ba(OH)2 : HNO3= 1 : 2

Find moles HNO3, using that Ba(OH)2 : HNO3 is 1 : 2

So n(HNO3) = 2 times the moles in Ba(OH)2 = 2 *1.25 x 10-3

= 2.5 x 10-3 mol

Calculate concentration of HNO3: M = n ÷ V

n = 2.5 x 10-3moles, V = 40.0 x 10-3L

      

M = 2.5 x 10-^3 ÷ 40.0 x 10^-3

M = 0.0625M or 0.0625 mol L-1   <~~Answer

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Oxygen usually has a charge of -2.

In N2O, we have one Oxygen which carries a charge of -2.

Since the overall molecule is neutral, the Nitrogen must balance that charge, so since we have 2 Nitrogen, each one is in a +1 state.

N2O:

O = -2

N = +1   <~~Answer.

Hope this helps.