1. Lemon juice (pH 2.2) = Acidic
2. Salt solution (pH 7) = Neutral
3. Baking soda (pH 9) = Alkaline
4. Bleach (pH 13) = Alkaline
5. Tomato juice (pH 4) = Acidic
6. Gastric juices (pH 1) = Acidic
<h3>Explanation: </h3>
The pH scale measures how acidic or alkaline a substance is. The pH scale ranges from <u>0 to 14.</u>
A pH of 7 is neutral.
Acidic substances have pH less than 7.
Alkaline(Base) substances have a pH greater than 7
Hence, the given samples can be categorized as acidic, basic or neutral based on their pH values.
1. Lemon juice (pH 2.2 < 7) = Acidic
2. Salt solution (pH 7 = 7) = Neutral
3. Baking soda (pH 9 > 7) = Alkaline
4. Bleach (pH 13 >7) = Alkaline
5. Tomato juice (pH 4 < 7) = Acidic
6. Gastric juices (pH 1 < 7) = Acidic
Answer:
1.32 moles.
Explanation:
From the question given above, the following data were obtained:
Density of Al = 2.70 g/cm³
Volume of Al = 13.2 cm³
Number of mole of Al =.?
Next, we shall determine the mass of Al.
This can be obtained as follow:
Density of Al = 2.70 g/cm³
Volume of Al = 13.2 cm³
Mass of Al =?
Density = mass / volume
2.7 = mass of Al / 13.2
Cross multiply
Mass of Al = 2.7 × 13.2
Mass of Al = 35.64 g
Finally, we shall determine the number of mole of Al. This can be obtained as follow:
Mass of Al = 35.64 g
Molar mass of Al = 27 g/mol
Number of mole of Al =?
Mole = mass / molar mass
Number of mole of Al = 35.64 / 27
Number of mole of Al = 1.32 moles
Thus, 1.32 moles of aluminum are present in the block of the metal.
A highly polar molecule that contains a weak bond between a hydrogen atom and another element would be a strong acid.
The water molecules are not completely removed so additional heating is required.
Explanation:
We have the copper (II) sulfate pentehydrate with the chemical formula CuSO₄ · 5H₂O.
molar mass of CuSO₄ · 5H₂O = 159.6 + 5 × 18 = 249.6 g/mole
Knowing this, we devise the following reasoning:
if in 249.6 g of CuSO₄ · 5H₂O there are 90 g of H₂O
then in 8 g of CuSO₄ · 5H₂O there are Y g of H₂O
Y = (8 × 90) / 249.6 = 2.88 g of water
mass of dried CuSO₄ = mass of CuSO₄ · 5H₂O - mass of H₂O
mass of dried CuSO₄ = 8 - 2.88 = 5.12 g
5.12 g is less that the weighted mass of 6.50 g. We deduce from this that the sample needs additional heating in order to remove all the water (H₂O) molecules.
Learn more about:
hydrates
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