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Calculate the relative atomic mass of zinc sulphate

Last updated date: 17th Apr 2024
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Hint: Zinc Sulphate is an inorganic compound. It's a nutritional supplement that's used to cure zinc deficiency and avoid it in people who are at high risk. Abdominal pain, vomiting, headaches, and exhaustion are also possible side effects of excessive supplementation. It was formerly referred to as "white vitriol." Zinc sulphate and its hydrates are colourless solids.

Complete answer:
The ratio of the total mass of atoms of a chemical element in a given sample to the atomic mass constant is referred to as relative atomic mass (symbol: Ar) or atomic weight. \[\dfrac{1}{{12}}\] the mass of a carbon-12 atom is known as the atomic mass constant (symbol: mu). The resulting value is dimensionless since all quantities in the ratio are masses; hence, the value is said to be relative.
The relative atomic mass of a given element in a single sample is the weighted arithmetic mean of the masses of the individual atoms (including their isotopes) in the sample. Since the sample's origin (and thus its radiation background or diffusion history) may have created unusual variations of isotopic abundances, this amount can differ significantly between samples. A sample of elemental carbon obtained from volcanic methane, for example, would have a different relative atomic mass than one collected from plant or animal tissues due to a different combination of stable carbon-12 and carbon-13 isotopes.
Add the number of protons to the number of neutrons to get the relative mass of every particle. The relative atomic mass of hydrogen is one, and the relative atomic mass of carbon-12 is twelve. Since different isotopes of the same element have different numbers of neutrons, you must account for one of them.
Given substance ZnSO₄
Atomic mass of Zinc = 65
Atomic mass of Sulphur = 32
Atomic mass of Oxygen = 16
Atomic mass of 4 x Oxygen = 4 x 16 = 64
Atomic mass of ZnSO₄ = 65 + 32 + 64 = 161 amu

The total mass of an element's atoms, measured in atomic mass units, is its atomic mass (amu, also known as daltons, D). The atomic mass of an element is a weighted average of all its isotopes, where the mass of each isotope is multiplied by the abundance of that isotope.
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