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#?

Answer 1

#"0.2 M"#

Write the neutralization reaction's balanced chemical equation first.

#"KOH"_text((aq]) + "HNO"_text(3(aq]) -> "KNO"_text(3(aq]) + "H"_2"O"_text((aq])#
Notice that you have #1:1# mole ratios between potassium hydroxide, #"KOH"#, and nitric acid, #"HNO"_3#. This tells you that the reaction will always consume equal numbers of moles of the two reactants.

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

#color(blue)(c = n_"solute"/V_"solution")#

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.

#c = n/V implies n = c * V#
#n_(KOH) = "0.15 M" * 10 * 10^(-3)"L" = "0.0015 moles KOH"#

Naturally, this suggests that you have

#0.0015 color(red)(cancel(color(black)("moles KOH"))) * "1 mole HNO"_3/(1color(red)(cancel(color(black)("mole KOH")))) = "0.0015 moles HNO"_3#

This indicates that the molarity of the nitric acid solution was

#c = n/V#
#c_(HNO_3) = "0.0015 moles"/(7.5 * 10^(-3)"L") = color(green)("0.2 M")#

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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Answer 2

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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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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