CHEMISTRY HIGH SCHOOL

What is the molarity of a 10 L solution containing 5.0 moles of solute?

Answers

Answer 1

Answer:

Explanation:

Number of moles consisting in a liter of solution is known as molarity.

Mathematically, Molarity = \frac{\text{no. of moles}}{\text{Volume in one liter}}[/tex]

It is given that volume is 10 liter and there is 5.0 moles of solute. Hence, we will calculate the molarity as follows.

Molarity = $\frac{\text{no. of moles}}{\text{Volume in one liter}}$

= $(5.0 mol)/(10 liter)$

= 0.5 mol/L

Thus, we can conclude that molarity of the given solution is 0.5 mol/L.

Answer 2

Answer: Molarity = Moles of solute/ L(liters) of solution

So let's plug in the information.

5.0 moles/10L = 0.5 M

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Which molecules shown on the graph above are likely candidates for evaporation? 1. molecules under the left end of the curve
2. molecules under the apex of the curve
3. molecules under the right end of the curve
4. all molecules under curve "T2"

Answers

Answer : The correct option is, (3) molecules under the right end of the curve

Explanation :

Evaporation : It is type of process in which the phase changes from liquid state to gaseous state below the boiling temperature of the liquid.

As we know that the higher the temperature of the liquid $(T_2)$ , the more will be the molecule escaping into the gaseous phase than the lower temperature $(T_1)$ .

So, the molecules under the right end of the curve are likely candidates for evaporation.

Hence, the correct option is, (3)

Answer: molecules under the right end of the curve

Explanation: smart

Which statement correctly compares an atom of an alkali metal with an atom of the alkaline earth metal next to it on the periodic table?

Answers

The atom of alkaline earth metal has one more proton and one more electron than the alkali metal that is next to it to the left on the periodic table. Then the atomic number of the alkali metal is one unit less than the atomic number of the alkaline earth metal next to it.

If the Kb of a weak base is 4.6 × 10-6, what is the pH of a 0.32 M solution of this base?

Answers

Assuming that the given base is a weak monoprotic base, the pH of the solution can be calculated as follows:

Write the balanced reaction and ice chart:

BOH --> OH- + B+

i 0.32 0 0
c -x x x
e 0.32-x x x

Kb = x^2/ (0.32-x)
x = 1.21x10^-3 = [OH-]
pOH = -log[OH-] = -log[1.21x10^-3] = 2.917
pH = 14 - pOH = 14 - 2.917 = 11.08

What is true about Carbon-14 and Carbon-12?a. The mass of the Carbon-14 sample is less than the Carbon-12 sample, but the reactivity of both samples was the same.
b. The mass of the Carbon-14 sample is greater than the Carbon-12 sample, but the reactivity of both samples was the same .
c. The reactivity of the Carbon-14 sample is less than the Carbon-12 sample, but the mass of both samples was the same.
d. The reactivity of the Carbon-14 sample is greater than the Carbon-12 sample, but the mass of both samples was the same.

Answers

Answer:

Explanation:

Correct: b. The mass of the Carbon-14 sample is greater than the Carbon-12 sample, but the reactivity of both samples was the same .

- C-14 has two additional neutrons, so is heavier than C-12. The chemical properties will be the same, however.

How is skepticism important to the progress of science in this scenario?

Answers

being a sceptic is important because it keeps you searching for answers

Calculate the number of moles 3.15 g of HNO3 19.3 g of NaCl 21.25 g of NaNO3

Answers

The number of moles:
3.15g of $HNO_(3)$
1 mole of $HNO_(3)$ - 63g.
x moles of $HNO_(3)$ - 3.15g
$x=(1\ mole*3.15g)/(63g)=(3.15)/(63)=0.05\ mole$

The number of moles:
19.3 g of NaCl
1 mole of NaCl- 58.44g.
x moles of NaCl- 19.3g.
$x=(1\ mole*19.3g)/(58.44g)=(19.3)/(58.44)=0.33\ mole$

The number of moles:
21.25 g of $NaNO_(3)$
1 mole of $NaNO_(3)$ - 85g.
x moles of $NaNO_(3)$ - 21.25g.
$x=(1\ mole*21.25g)/(85g)=(21.25)/(85)=0.25\ mole$

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