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shutvik [7]
3 years ago
13

= 25 X 5 = (use the correct number of sig figs)

Chemistry
1 answer:
Anton [14]3 years ago
5 0

Answer:

1.25 *10^2

Explanation:

25*5 = 125

= 1.25 *10^2

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A water treatment tablet contains 20.0 mg of tetraglycine hydroperiodide, 40.0% of which is available as soluble iodine. If two
Galina-37 [17]

Answer:

16\ \text{ppm}

Explanation:

Mass of one tablet = 20 mg

Mass of two tablets = 2\times 20=40\ \text{mg}

Percent that is soluble in water = 40%

Mass of tablet that is soluble in water = 0.4\times 40=16\ \text{mg}

So, mass of solute is 16\ \text{mg}

Density of water = 1 kg/L

Volume of water = 1 L

So, mass of 1 L of water is 1\times 1=1\ \text{kg}=1000\ \text{g}

PPM is given by

\dfrac{\text{Mass of solute}}{\text{Mass of solvent}}\times 10^6=\dfrac{16\times 10^{-3}}{1000}\times 10^6\\ =16\ \text{ppm}

Hence, the concentration of iodine in the treated water 16\ \text{ppm}.

8 0
2 years ago
What's the answer to this question?
Lena [83]
The answer is B- 124 degrees
4 0
2 years ago
Read 2 more answers
How does one calculate the mass of the sample?
antoniya [11.8K]

Answer:

HUH I NEED A PIC of the question

Explanation:

4 0
2 years ago
A sample of iron with a mass of 200g releases 9840 cal when it freezes at it’s freezing point. What is the molar heat of fusion
antoniya [11.8K]

Answer:-

2747.7 Cal mol -1

Explanation:-

Molar heat of Fusion is defined as the amount of heat necessary to melt (or freeze) 1 mole of a substance at its melting point.

Atomic mass of Iron = 55.845 g mol-1

Mass of Iron = 200 g

Number of moles of Iron = 200 g / (55.845 g mol-)

= 3.581 moles

Heat released = 9840 Cal

Molar heat of Fusion = Heat released / Number of moles

= 9840 Cal / 3.581 moles

= 2747.7 Cal mol -1

8 0
2 years ago
Read 2 more answers
Answer with explanation
creativ13 [48]
The answer should be:

KOH (aq) + HCl (aq) --> KCl (aq) + H20 (l).

KOH is a base, because OH can accept a H+.
HCl is an acid because it can donate a H+.

In general, bases are : OH-, and acids are : H+.


8 0
2 years ago
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