How much calcium hydroxide (#Ca(OH)_2#), in grams, is needed much produce 1.5 L of a 0.25M solution?

Answer 1

27.75 gm

molarity is defined as = moles of solute / litres of solution

to produce 1.5 L of 0.25 M solution , moles of calcium hydroxide needed are = # 0.25*1.5 # = 0.375 mol now amount of calcium hydroxide in grams needed can be calculated by multiplying moles by molar mass : # 0.375*74 # = 27.75 gm

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Answer 2

Naomi Aronson

To calculate the amount of calcium hydroxide (Ca(OH)2) needed to produce a 0.25M solution in 1.5 liters, use the formula:

Amount (in moles) = concentration (in M) × volume (in liters).

Firstly, calculate the moles of Ca(OH)2 required: 0.25 mol/L × 1.5 L = 0.375 moles.

Then, use the molar mass of Ca(OH)2 to convert moles to grams: Ca(OH)2 molar mass = 40.08 g/mol (for calcium) + 2(15.999 g/mol) + 2(1.008 g/mol) = 74.1 g/mol.

Finally, multiply the moles by the molar mass: 0.375 moles × 74.1 g/mol = 27.79 grams.

So, approximately 27.79 grams of calcium hydroxide (Ca(OH)2) is needed to produce 1.5 liters of a 0.25M solution.

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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.