Answer:
The resulting solution is basic.
Explanation:
The reaction that takes place is:
First we calculate the added moles of HNO₃ and KOH:
As there are more KOH moles than HNO₃, the resulting solution is basic.
The resulting solution is basic.
• It is known that KOH is a base and HNO3 is an acid, so when they mix they undergo a neutralization reaction.
• The reaction between there will be,
HNO3 + KOH ⇔ KNO3 + H2O
Based on the given information,
• The volume of HNO3 is 12.5 ml and the molarity is 0.280 M, and the volume of KOH is 5 ml and the molarity is 0.920 M.
Now 1 mole of HNO3 completely reacts with 1 mole of KOH,
The millimoles of HNO3 is,
[tex]= Molarity * Volume (in ml)\\= 0.280 * 12.5\\= 3.5 mmol[/tex]
The millimoles of KOH is,
[tex]= Molarity * Volume (in ml)\\= 0.920 * 5.0\\= 4.6 mmol[/tex]
Now it can be seen that 3.5 millimoles of HNO3 completely reacts with 3.5 millimoles of KOH. Now we are left with 4.6-3.5 = 1.1 mmol of KOH.
Thus, KOH is in excess amount present in the solution, and as it is basic in nature, therefore, the resultant solution would be basic in nature.
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