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3 years ago

A 650.0 g hard-water sample contains 101 mg Ca.what is this concentration in parts per million

Chemistry

1 answer:

ki77a [65]3 years ago

8 0

Answer:

= 155 ppm

Explanation:

PPM also refers to parts per million, it represents a low concentration of a solution. It represents 0.001 gram or a milligram in a 1000 mL, equivalent to 1 mg per liter

Given that;

101 mg of Ca in 650.0 g of water

1 ppm = 1 mg/L

650 g = 650 mL = 0.65 L

Therefore;

= 101 mg/ 0.65 L

= 155.38 mg/L

= 155 ppm

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Answer:

588.2 mL

Explanation:

FeSO₄(aq) + 2KOH(aq) → Fe(OH)₂(s) + K₂SO₄(aq)

First we calculate how many Fe⁺² moles reacted, using the given concentration and volume of FeSO₄ solution (the number of FeSO₄ moles is equal to the number of Fe⁺² moles):

moles = molarity * volume

187 mL * 0.692 M = 129.404 mmol Fe⁺²

Then we convert Fe⁺² moles to KOH moles, using the stoichiometric ratios:

129.404 mmol Fe⁺² * $\frac{2mmolKOH}{1mmolFeSO_4}$ = 258.808 mmol KOH

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258.808 mmol KOH / 0.440 M = 588.2 mL

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3 years ago

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Answer:

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8.10

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Explanation:

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2 years ago

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