Chemistry, asked by arindammukerji7386, 11 months ago

How many milliliters of 0.250 M KoH will be needed to titrate 12.53 mL of 0.130 M HNO3?

Answers

Answered by ramashishgupta8161
6

You will need 6.516 mL of KOH to reach the equivalence point.

Explanation:

Since KOH has only one OH− ion in its formula, and HNO3 is monoprotic (donates only one hydrogen ion), the titration reaches an equivalence point when

Moles HNO3 = moles KOH

And since moles (of solute) = concentration x volume, we can write

Ma⋅Va=Mb⋅Vb

(the a and b representing the acid and base, respectively)

We know the first three quantities in this equation. We find the fourth (Vb) as follows:

(0.130)⋅(0.01253)=(0.250)Vb

Vb=(0.130)⋅(0.01253)0.250=0.006516L

or 6.516mL

or

Approx. 6−7⋅mL..........

Explanation:

We need (i) a stoichiometric equation........

HNO3(aq)+KOH(aq)→KNO3(aq)+H2O(l)

And then (ii) equivalent quantities of potassium hydroxide and nitric acid:

Moles of nitric acid=12.53⋅mL×10−3L⋅mL−1×0.130⋅mol⋅L−1=1.63×10−3mol.

And thus we need 1.63×10−3mol0.250⋅mol⋅L−1×103⋅mL⋅L−1

6.52⋅mL

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ramashishgupta8161: gm
Answered by tina9961
0

 \huge\mathcal{Answer}

______________ ________________

Since KOH has only one OH- ion in its formula, and HNO3

is monoprotic (donates only one hydrogen ion), the titration reaches an equivalence point when Moles

HNO3= moles KOH

And since moles (of solute) = concentration x volume, we can write

Ma⋅Va=Mb⋅VL(the a and brepresenting the acid and base, respectively)

We know the first three quantities in this equation. We find the fourth (Vb) as follows:

(0.130)⋅(0.01253)=(0.250)VbVb=(0.1300.250=0.006516L or 6.516mL

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