Respuesta :
Answer:
273 mL.
Explanation:
From the question given above, the following data were obtained:
Molarity of HBr = 0.220 M
Mole of HBr = 0.060 mole
Volume =?
Molarity is simply defined as the mole of solute per unit litre of the solution. Mathematically, it is expressed as:
Molarity = mole /Volume
With the above formula, we can obtain the volume required as illustrated below:
Molarity of HBr = 0.220 M
Mole of HBr = 0.060 mole
Volume =?
Molarity = mole /Volume
0.220 = 0.060 / Volume
Cross multiply
0.220 × Volume = 0.060
Divide both side by 0.220
Volume = 0.060 / 0.220
Volume = 0.273 L
Finally, we shall convert 0.273 L to millilitres (mL). This can be obtained as follow:
1 L = 1000 mL
Therefore,
0.273 L = 0.273 L × 1000 mL / 1 L
0.273 L = 273 mL
Thus, 0.273 L is equivalent to 273 mL.
From the calculations made above, 273 mL of HBr is required.
The volume of 0.220 M HBr solution (in mL) required to obtain 0.060 moles of HBr is 272.7mL
From the question,
We are to determine the volume of 0.220M HBr solution that is required to obtain 0.060 moles of HBr.
To determine this, we will use the formula connecting number of moles, concentration and volume
From the formula,
Number of moles = Concentration × Volume
Then,
[tex]Volume = \frac{Number \ of \ moles}{Concentration}[/tex]
From the question,
Concentration of the HBr solution = 0.220 M
Required number of moles of HBr = 0.060 moles
∴ [tex]Volume \ of \ HBr \ required = \frac{0.060}{0.220}[/tex]
Volume of HBr required = 0.272727 L
Now, we will convert this to milliliter (mL)
(NOTE: 1L = 1000 mL)
∴ 0.272727 L = 0.272727 × 1000 mL
= 272.727 mL
≅ 272.7 mL
Hence, the volume of 0.220 M HBr solution (in mL) required to obtain 0.060 moles of HBr is 272.7mL
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