chemistry

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.
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)

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  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.

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  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

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  3. CHEMISTRY

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  4. Correct

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  5. Can u paste how the solution was solved

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  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

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  7. The answer for this question

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  8. I want an answer to the question

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  9. I want the answer to my question

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