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Andrews [41]
2 years ago
8

How many milliliters of a stock solution of 12.1 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3

Chemistry
1 answer:
AnnZ [28]2 years ago
7 0

Answer:

(5.00M)(X) = (0.120L)(0.470M)

 

X = (0.120)(0.470)/(5.00)

0.01128

Explanation:

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Calculate the molarity of 48.0 mL of 6.00 M H2SO4 diluted to 0.250 L
const2013 [10]

Answer:

The answer is 1.15m.

Since molality is defined as moles of solute divided by kg of solvent, we need to calculated the moles of H2SO4 and the mass of the solvent, which I presume is water.

We can find the number of H2SO4 moles by using its molarity

C=nV→nH2SO4=C⋅VH2SO4=6.00molesL⋅48.0⋅10−3L=0.288

Since water has a density of 1.00kgL, the mass of solvent is

m=ρ⋅Vwater=1.00kgL⋅0.250L=0.250 kg

Therefore, molality is

m=nmass.solvent=0.288moles0.250kg=1.15m

4 0
3 years ago
Read 2 more answers
You have a gas at a volume of 9.71 L at a pressure of 209 torr and at 10.1 °C. What
Usimov [2.4K]

Answer:

219.95 °C

Explanation:

Given data:

Volume of gas = 9.71 L

Initial pressure = 209 torr (209/760 = 0.275 atm)

Initial temperature = 10.1 °C (10.1 +273 = 283.1 K)

Final temperature = ?

Final pressure = 364 torr (364/760 =0.479 atm)

Solution:

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

0.275 atm / 283.1 K = 0.479 atm/T₂

T₂ = 0.479 atm × 283.1 K/ 0.275 atm

T₂ = 135.6 atm. K /0.275 atm

T₂ = 493.1 K

Kelvin to °C:

493.1 K - 273.15 = 219.95 °C

8 0
3 years ago
This chart shows descriptions of the atoms for four different substances.
Whitepunk [10]
I think it’s Object 3
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3 years ago
Who were good friends in one day a stranger came<br><br>​
insens350 [35]

Answer:

???

Explanation:

5 0
3 years ago
In a combustion reaction, one of the reactants is always _______________.
QveST [7]
In a combustion reaction, one of the reactants is always oxygen.
4 0
3 years ago
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