A is a solution of trioxonitrate(v) acid, HNO3, of unknown concentration. B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25cm3 portions solution B required an average of 24.00cm3 of solution A for neutralization, using 2drops of methyl orange.

Question

a: write a balanced equation for the reaction?
b:Calulate the concentration of solution B in moles per dm3 ?
c: calculate the concentration of solution A in moles per dm3
d: calculate the concentration in g/dm3 of HNO3 in solution A. (H=1, N=14, O=16, Na=23)

Answer 1

I would be much happier if you just called HNO3 as nitric acid and Pb(NO3)2 as lead(II) nitrate.
a.
HNO3 + NaOH ==> NaNO3 + H2O

b.
mols NaOH = 4/molar mass NaOH = ?

c.
M NaOH(soln B) = mols/cm3 = ?
cc(HNO3) x M(HNO3) = cc(NaOH)x M(NaOH. Substitute and solve for M HNO3.

d.
I'll leave this for you.

Answer 2

conc. of solution b is 0.1 molperdm3conc. of solution a inmolperdm3 is 0.01 conc. in gperdm3 of hno3 in solution a is 0.63g/dm3

Answer 3

CHEMISTRY

Answer 4

Correct

Answer 5

Can u paste how the solution was solved

Answer 6

A is a solution of trioxonitrate (iv) acid (nitric acid) of unknown concentration. B is a standard solution containing 4.00g, 25cm3 portion of solution B requires an average of 24.00cm3 of solution A for complete neutralization

Answer 7

The answer for this question

Answer 8

I want an answer to the question

Answer 9

I want the answer to my question