# It takes 10 mL of 0.15 M #KOH# solution to neutralize 7.5 mL of #HNO_3# solution. What is the molarity of #HNO_3#?

Write the neutralization reaction's balanced chemical equation first.

The number of moles of solute in liters of solution is now the definition of molarity.

To calculate how many moles of this strong base were used to neutralize the strong acid, all you really need to do in this case is use the molarity and volume of the potassium hydroxide solution.

The number of moles of acid and base will be equal, based on the previously mentioned mole ratio.

Naturally, this suggests that you have

This indicates that the molarity of the nitric acid solution was

The number of sig figs you have for the volume of the potassium hydroxide solution is the answer, rounded to one.

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To find the molarity of HNO3, use the equation (M_1V_1 = M_2V_2). Plug in the given values: (V_1 = 10 , \text{mL}), (M_1 = 0.15 , \text{M}), (V_2 = 7.5 , \text{mL}). Solve for (M_2).

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