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Serjik [45]
3 years ago
9

Some nickel sulfate solution was carefully placed in the bottom of a beaker of water. The beaker was then covered and left for s

everal days.
a. Describe what you would see after:
(i) a few hours
(ii) several days.
b. Explain your answer using your ideas of the kinctic theory of particles.
c. What is the name of the physical process that takes place in this experiment?​
Chemistry
1 answer:
Furkat [3]3 years ago
7 0
When’s this due I think I can find out
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What is the concentration, in mass percent (m/m), of a solution prepared from 50.0 g nacl and 150.0 g of water?
Nataly [62]
Mass of solute ( m1 ) = 50.0 g

mass of solvent ( m2 ) = 150.0 g

Therefore:

m/m = ( m1 / m1 + m2 )

m/m = ( 50.0 / 50.0 + 150.0 )

m/m = ( 50.0 / 200 )

m/m = 0.25
8 0
3 years ago
Read 2 more answers
- a) write the formula unit of calcium fluoride.
8090 [49]

Answer:

hope this image is helpful for you

5 0
3 years ago
Hard water often contains dissolved Ca2+ and Mg2+ ions. One way to soften water is to add phosphates. The phosphate ion forms in
katrin2010 [14]

Answer:

22.4269 grams of sodium phosphate must be added to 1.4 L of this solution to completely eliminate the hard water ions

Explanation:

We will first write the balanced equation for this scenario

3 CaCl2 + 2 Na3PO4 ----> 6 NaCl + Ca3 (PO4)2

3 Mg(NO3)2 + 2 Na3PO4 -----> 6 NaNO3 + Mg3 (PO4)2

The ratio here for both calcium chloride and magnesium nitrate is 3:2

The number of moles of each compound is equal to

0.054 * 1.4 = 0.0756\\0.093* 1.4 = 0.1302

Using the mole ratio of 3:2, convert each to moles of sodium phosphate.

0.0756 mole of CaCl2 is equal to 0.05\\ Na3PO4

0.1302 mole of CaCl2 is equal to 0.0868 Na3PO4

Converting moles of sodium phosphate to grams of sodium phosphate we get

(0.05 +0.0868) * 163.94 g/mol

22.4269 grams of sodium phosphate must be added to 1.4 L of this solution to completely eliminate the hard water ions

8 0
3 years ago
How can you tell what is what and how that what affects what
VLD [36.1K]

Answer:

Hi, this is a super vague question, so its pretty confusing to answer.  Could you please be a bit more specific?

If you are referring to chemistry, then how you tell "what is what" is by the molecular makeup of an element (Periodic table), and "how that..affects what", chemical reactions can occur between elements

8 0
3 years ago
Read 2 more answers
Calculate the amount of heat required to raise the temperature of a 32g sample of water from 8°C to 22°C.
qwelly [4]

Answer:

The amount of heat required to raise the temperature of a 32g sample of water from 8°C to 22°C is 1,874.432 J

Explanation:

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

Sensible heat is the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).

Between heat and temperature there is a direct proportional relationship. The constant of proportionality depends on the substance that constitutes the body and its mass, and is the product of the specific heat and the mass of the body. So, the equation that allows to calculate heat exchanges is:

Q = c * m * ΔT

where Q is the heat exchanged by a body of mass m, constituted by a substance of specific heat c and where ΔT is the variation in temperature.

In this case:

  • c= 4.184 \frac{J}{g*C}
  • m= 32 g
  • ΔT= Tfinal - Tinitial= 22°C - 8°C= 14°C

Replacing:

Q= 32 g* 4.184 \frac{J}{g*C} *14 °C

Solving:

Q= 1,874.432 J

<u><em>The amount of heat required to raise the temperature of a 32g sample of water from 8°C to 22°C is 1,874.432 J</em></u>

7 0
2 years ago
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