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sleet_krkn [62]
2 years ago
7

In this experiment you used an excess of the BaCl2 solution. How would your results be affected if you did not use an excess of

the BaCl2 solution? Would this error cause your calculation of the mass percent of sulfate in the unknown to be too high or too low? Explain.
Chemistry
1 answer:
Igoryamba2 years ago
3 0

if we did not use an excess of the BaCl2 solution it would decrease the mass percentage of sulfate in the unknown sample.

The net precipitation equation would be.

Ba2+(aq) + SO42-(aq)  → BaSO4(s)

If BaCl2 (Ba2+) is not taken in excess then the precipitation would not be completed as some of the sulfate ions would still be remaining in the solution. This would decrease the mass percentage of sulfate in the unknown sample.

If some tiny pieces of filter paper still remained mixed with the precipitate(BaSO4) then the mass of sulfate would increase and it gives a high mass percentage of the sulfate.

mass percentage of sulfate = (mass of sulfate/mass of sample)*100

Learn more about precipitation here brainly.com/question/14675507

#SPJ4

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A container of oxygen has a volume of 30.0 mL and a pressure of 72.5 psi. If the pressure of the oxygen gas is reduced to 28 psi
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Answer:

THE NEW VOLUME OF THE OXYGEN GAS AT 28 PSI FROM 72.5 PSI IS 0.078 L.

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This question follows Boyle's equation of gas laws and mathematically it is written as:

P1 V1 = P2 V2

Re-arranging by making P2 the subject of the formula, we have:

V2 = P1 V1 / P2

V2 = 72,5 * 0.03 / 28

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<u>Hence, 4. is the answer.</u>

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