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Marina CMI [18]
3 years ago
10

What mass of solute must be used to prepare 500ml of 0.100M aqueous sodium borate Na2B4O7 from solid hydrated sodium borate Na2B

4O7.10H2O?
please show all working.

30 points on offer!!!!!
Chemistry
1 answer:
motikmotik3 years ago
4 0

0.000132 g of hydrated sodium borate (Na₂B₄O₇ · 10 H₂O)

Explanation:

First we need to find the number of moles of sodium borate (Na₂B₄O₇) in the solution:

molar concentration = number of moles / volume (L)

number of moles = molar concentration × volume (L)

number of moles of Na₂B₄O₇ = 0.1 × 0.5 = 0.05 moles

We know now that we need 0.05 moles of hydrated sodium borate (Na₂B₄O₇ · 10 H₂O) to make the solution.

Now to find the mass of hydrated sodium borate we use the following formula:

number of moles = mass / molar weight

mass =  number of moles × molar weight

mass of hydrated sodium borate = 0.05 / 381 = 0.000132 g

Learn more about:

molar concentration

brainly.com/question/14106518

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People take antacids, such as milk of magnesia, to reduce the discomfort of acid stomach or heartburn. The recommended dose of m
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Explanation:

Hello,

In this case, since the chemical reaction is:

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We can see that hydrochloric acid and magnesium hydroxide are in a 2:1 mole ratio, which means that the neutralization point, we can write:

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In such a way, the moles of magnesium hydroxide (molar mass 58.3 g/mol) in 500 mg are:

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Then, since the concentration and the volume define the moles, we can write:

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Always subtract the smaller number from the greater one. 
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