Molal concentration gives the number of moles dissolved in 1 kg of solution.
Molal concentration of H₂SO₄ is 2.88 mol/kg
the weight of H₂SO₄ in 1 kg - 2.88 mol x 98 g/mol = 282.2 g
The total weight of solution - 1000 g + 282.2 g = 1282.2 g
density of solution is 1.167 g/ml
We need to find how many moles are dissolved in 1 L.
We know the weight of the solution, using this we can calculate volume of the solution
volume of solution is - 1282.2 g / 1.167 g/mL = 1098.7 mL
The number of H₂SO₄ moles in 1.0987 L = 2.88 mol
Therefore in 1 L = 2.88 mol / 1.0987 L = 2.62 mol
Molarity of H₂SO₄ is 2.62 mol/L = 2.62 M
Answer:
The correct answer is 399.8 ppm
Explanation:
A concentration in parts per million (ppm) is equal to:
Solute: Cd; Mass = 180 mg x (1 g/1000 mg) = 0.18 g
Solvent: Water ; Mass= 450.0 g x (1 kg/1000 g) = 0.45 kg
We have the following total mass of solution:
Mass of solution = Mass of solute + Mass of solvent = 0.18 g + 450 g = 450.18 g = 0.45018 kg
Finally, we divide the <u>mass of solute (in mg)</u> into the <u>mass of solution (in kg)</u> to obtain the ppm (in mg/Kg):
ppm = 180 mg/0.45018 kg = 399.8 mg/Kg = 399.8 ppm
Its 70 and more because its right
Answer:
<h2>If we mix equal amounts of an acid and a base then two chemicals essentially cancel out each other and produce </h2><h2>salt and water. Mixing equal amounts of a strong acid with strong base results in a neutral solution whose pH value remains 7 and this type of reactions are known as neutralization reactions.</h2>
Explanation:
<h2>
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C
I have had this question on a test before!! Hope this helps