# Calculate the molarity (in mol/L) of #"K"^(+)# ions present in an aqueous solution prepared by adding #"23.4 mL"# of #9.32*10^(-1)"M"# aqueous #"K"_2"SO"_3# to #"185 mL"# of water? Report your answer to three significant figures.

The first thing that you need to do here is to figure out how many moles of potassium sulfite are present in the initial sample.

Now, you know that potassium sulfite is soluble in aqueous solution, which implies that it dissociates completely when dissolved in water

Next, calculate the total volume of the resulting solution, i.e. the volume of the diluted solution

This means that the molarity of the potassium cations in the diluted solution will be--don't forget to convert the volume of the solution to liters!

The answer is rounded to three sig figs.

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[Molarity = \frac{moles\ of\ solute}{liters\ of\ solution}] [moles\ of\ solute = Molarity \times liters\ of\ solution] [liters\ of\ solution = \frac{23.4\ mL\ +\ 185\ mL}{1000}] [moles\ of\ solute = (9.32 \times 10^{-1} M) \times \frac{23.4\ mL\ +\ 185\ mL}{1000}] [moles\ of\ solute \approx 0.221\ mol] [Molarity\ of\ K^+ ions \approx \frac{0.221\ mol}{23.4\ mL\ +\ 185\ mL}] [Molarity\ of\ K^+ ions \approx 0.00118\ M]

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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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