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Luda [366]
3 years ago
5

Describe how a homogeneous mixture differs from a heterogeneous mixture?

Chemistry
1 answer:
yaroslaw [1]3 years ago
8 0

Answer:

A homogeneous mixture has the same uniform appearance and composition throughout.A heterogeneous mixture consists of different substances or phases.It is a mixture where the components of the mixture are not uniform or have localized regions with different properties The three phases or states of matter are gas, liquid, and solid.

Explanation:

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How many moles are present in 4.7 liters of argon gas as STP
algol [13]
Answer:

0.21mol Ar (g)

Explanation:

To convert from litres to moles at STP we must divide the amount of litres by 22.4.

4.7 / 22.4 = 0.21mol Ar (g)
5 0
3 years ago
Read 2 more answers
if 100. mL of 0.800 M Na2SO4 is added to 200. mL of 1.20 M NaCl, what is the concentration of Na+ ions in the final solution? As
Black_prince [1.1K]
Compounds Na₂SO₄ and NaCl are mixed together are we are asked to find the concentration of Na⁺ in the mixture 
Na₂SO₄ ---> 2 Na⁺ + SO₄³⁻

1 mol of Na₂SO₄ gives out 2 mol of Na⁺ ions 

the number of Na₂SO₄ moles added - 0.800 M/1000 * 100 ml
                                                         = 0.08 mol
therefore number of Na⁺ ions from Na₂SO₄ = 0.08 * 2 = 0.16 mol

NaCl ----> Na⁺ + Cl⁻ 
1 mol of NaCl gives 1 mol of Na⁺ ions
number of NaCl moles added = 1.20 M/1000 * 200 ml
                                               = 0.24 mol
number of Na⁺ ions from NaCl = 0.24 mol

total number of Na⁺ ions in the mixture = 0.16 mol + 0.24 mol = 0.4 mol
as stated the volumes are additive, 
therefore total volume  = 100 ml + 200 ml = 300 ml 
the concentration of Na⁺ ions = number of moles / volume 
                                              = 0.4 mol/ 0.3 dm³
concentration of Na⁺ = 1.33 mol/dm³
5 0
3 years ago
Which is not needed for a hurricane to form?
aliya0001 [1]

Answer:

strong cold front

Explanation:

5 0
3 years ago
Read 2 more answers
An aqueous solution containing 16.5 g of an unknown molecular (nonelectrolyte) compound in 106.0 g of water was found to have a
salantis [7]

Answer : The molar mass of unknown compound is 152.38 g/mole

Explanation :

Depression in freezing point = 1.9^oC

Mass of unknown compound = 16.5 g

Mass of water = 106.0 g

Formula used :  

\Delta T_f=i\times K_f\times m\\\\\Delta T_f=i\times K_f\times\frac{\text{Mass of unknown compound}}{\text{Molar mass of unknown compound}\times \text{Mass of water in Kg}}

where,

\Delta T_f = depression in freezing point

i = Van't Hoff factor = 1 (for non-electrolyte)

K_f = freezing point constant for water = 1.86^oC/m

m = molality

Now put all the given values in this formula, we get

1.9^oC=1\times (1.86^oC/m)\times \frac{16.5g\times 1000}{\text{Molar mass of unknown compound}\times 106.0g}

\text{Molar mass of unknown compound}=152.38g/mole

Therefore, the molar mass of unknown compound is 152.38 g/mole

5 0
3 years ago
Read 2 more answers
Write a net ionic equation to show how isoquinoline, c9h7n, behaves as a base in water.
Gekata [30.6K]
There can be three definitions of a base: Arrhenius base, Lewis base or Bronsted-Lowry base. Isoquinoline acts specifically as a Bronsted-Lowry base, which is a proton acceptor. Also, it acts as an Arrhenius base because it produces OH- ions after the reaction. The net ionic equation is:

<span><em>C</em></span><em>₉</em><span><em>H</em></span><em>₇</em><span><em>N (aq) + H</em></span><em>₂</em><span><em>O ---> C</em></span><em>₉</em><span><em>H</em></span><em>₇</em><span><em>NH</em></span><em>⁺</em><span><em> (aq) + OH</em></span><em>⁻</em><span><em> (aq)</em></span>
6 0
3 years ago
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