<h3>
Answer:</h3>
2.624 g
<h3>
Explanation:</h3>
The equation for the reaction is given as;
- CuSO₄(aq) + 2NaOH(aq) → Cu(OH)₂(s) + Na₂SO₄(aq)
- Volume of CuSO₄ as 46.0 mL;
- Molarity of CuSO₄ as 0.584 M
We are required to calculate the mass of Cu(OH)₂ precipitated
- We are going to use the following steps;
<h3>Step 1: Calculate the number of moles of CuSO₄ used</h3>
Molarity = Number of moles ÷ Volume
To get the number of moles;
Moles = Molarity × volume
= 0.584 M × 0.046 L
= 0.0269 moles
<h3>
Step 2: Calculate the number of moles of Cu(OH)₂ produced </h3>
- From the equation 1 mole of CuSO₄ reacts to give out 1 mole of Cu(OH)₂
- Therefore; Mole ratio of CuSO₄ to Cu(OH)₂ is 1 : 1.
Thus, Moles of CuSO₄ = Moles of Cu(OH)₂
Hence, moles of Cu(OH)₂ = 0.0269 moles
<h3>
Step 3: Calculate the mass of Cu(OH)₂</h3>
To get mass we multiply the number of moles with the molar mass.
Mass = Moles × Molar mass
Molar mass of Cu(OH)₂ is 97.561 g/mol
Therefore;
Mass of Cu(OH)₂ = 0.0269 moles × 97.561 g/mol
= 2.624 g
Thus, the mass of Cu(OH)₂ that will precipitate is 2.624 g
Answer:
B) 0.59 M NaCl.
Explanation:
- It is known that the no. of millimoles of NaCl before dilution = the no. of millimoles of NaCl after dilution.
∵ (MV) before dilution = (MV) after dilution.
<em>∴ M after dilution = (MV) before dilution / V after dilution </em>= (3.2 M)(25.0 mL)/(135.0 mL) = <em>0.5926 M ≅ 0.59 M.</em>
The identity of a metal that has a mass of 27.0g and a volume of 10.0cm is Aluminium. That is option B.
<h3>What is molar mass?</h3>
Molar mass is defined as the mass in grams of one mole of an element. This is measured in grams/mole of that substance.
The metal that is 27.0 g and a volume of 10.0 cm3 is aluminium because aluminium is 27 times heavier than 1/12th of the mass of carbon-12 atom.
Therefore, the identity of a metal that has a mass of 27.0g and a volume of 10.0cm is Aluminium.
Learn more about molar mass here:
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