The concentration of a dextrose solution prepared by diluting 14 ml of a 1.0 M dextrose solution to 25 ml using a 25 ml volumetric flask is 0.56M.
Concentration is defined as the number of moles of a solute present in the specific volume of a solution.
According to the dilution law, the degree of ionization increases on a dilution and it is inversely proportional to the square root of concentration. The degree of dissociation of an acid is directly proportional to the square root of a volume.
M₁V₁=M₂V₂
Where, M₁=1.0M, V₁=14ml, M₂=?, V₂=25ml
Rearrange the formula for M₂
M₂=(M₁V₁/V₂)
Plug all the values in the formula
M₂=(1.0M×14 ml/25 ml)
M₂=14 M/25
M₂=0.56 M
Therefore, the concentration of a dextrose solution after the dilution is 0.56M.
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Answer:
B its B
Explanation:
P406(s) + 202(g) P4010(s)
Answer:
0.928 M
Explanation:
The concentration of acid can be determined by using the volume used and the concentration and volume used of base.
We will use the law of equivalence of moles.
M₁V₁=M₂V₂
M₁ = concentration of base used
V₁ = volume of base used
M₂ = concentration of acid used =? (to be determined)
V₂ = volume of acid used
The initial concentration of KOH used is diluted so let us find the final concentration of KOH after dilution
initial moles = final moles
initial concentration X initial volume = final concentration X final volume
6.2 X 2.1 = 250 X final concentration
final concentration = 0.052 M = M₁
V₁ = 36.9 mL
V₂ = 6.2 mL
Here with each mole of phosphoric acid three moles of KOH are used.
Therefore
3 M₁V₁ = M₂V₂
M₂ = 
Answer:
83.9g of sulfuric acid is the minimum mass you would need
1.73g of hydrogen would be produced
Explanation:
Based on the reaction:
2 Al(s) + 3 H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3 H₂(g)
2 moles of solid aluminium react with 3 moles of sulfuric acid. Also, two moles of Al produce 3 moles of hydrogen gas.
15.4g of Al are:
15.4g Al × (1mol / 26.98g) = 0.571 moles of Al.
Moles of sulfuric acid:
0.571 moles Al × (3 mol H₂SO₄ / 2 mol Al) = 0.8565 moles H₂SO₄
In grams:
0.8565 moles H₂SO₄ × (98g / 1mol) = <em>83.9g of sulfuric acid is the minimum mass you would need</em>
In the same way, moles of hydrogen produced are:
0.571 moles Al × (3 mol H₂ / 2 mol Al) = 0.8565 moles H₂
In grams:
0.8565 moles H₂ × (2.015g / 1mol) = <em>1.73g of hydrogen would be produced</em>
