(a) Write the balanced ionic equation for this reaction (b) What is the concentration of the nitric acid sol.?

Question

A 25.00 ml sample of nitric acid solution requires 22.49 ml of 0.112 mol L-1 potassium Hydroxide Solution for complete neutralisation.

Answer 1

a) H+ + OH- → H2O

b) V1M1 = V2M2

25.00×M1 = 22.49×0.112, so M1 = (22.49×0.112)/25 = 0.1007552 mol L^-1.

Answer 2

HNO3 (aq)+ KOH (aq)>> KNO3 (aq)+ H2O (l)

H+ + NO3- + K+ + OH- >> K+ + NO3- + H2O

net ionic :

H+ (aq) + OH- (aq) >> H2O (l)

Moles KOH = 0.02249 L x 0.112 =  0.00252 ( 3 significant figures)

Moles KOH = moles HNO3

Molarity HNO3 = 0.00252 mol / 0.02500 L =0.101 M