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Vlad [161]
3 years ago
7

Find the mass of 2.16 × 1023 molecules H2S. Answer in units of g.

Chemistry
1 answer:
worty [1.4K]3 years ago
7 0

Answer:

Mass = 12.276 g

Explanation:

Given data:

Number of molecules of H₂S = 2.16 × 10²³

Mass in gram = ?

Solution:

The given problem will solve by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.

The number 6.022 × 10²³ is called Avogadro number.

For example,

18 g of water = 1 mole = 6.022 × 10²³ molecules of water

Number of moles of  H₂S:

2.16 × 10²³ molecules × 1 mole /6.022 × 10²³ molecules

0.36 moles

Mass = number of moles ×  molar mass

Mass = 0.36 mol × 34.1 g/mol

Mass = 12.276 g

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a solution is made by combining 15.0 mlml of 18.5 mm acetic acid with 5.54 gg of sodium acetate and diluting to a total volume o
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pH of the solution is 4.14.

m(CH₃COONa) = 5.54 g.

n(CH₃COONa) = m(CH₃COONa) ÷ M(CH₃COONa).

n(CH₃COONa) = 5.54 g ÷ 82.034 g/mol.

n(CH₃COONa) = 0.067 mol; amount of sodium acetate.

V(CH₃COONa) = 1.5 L

c(CH₃COONa) = n(CH₃COONa) ÷ V(CH₃COONa).

c(CH₃COONa) = 0.067 mol ÷ 1.5 L.

c(CH₃COONa) = 0.045 M; molarity of sodium acetate in solution.

c(CH₃COOH) = 18.5 M; molarity of pure acetic acid.

V(CH₃COOH) = 15.0 mL = 0.015 L; volume of acetic acid

n(CH₃COOH) = 18.5 M x 0.015 L = 0.2775 mol; amount of pure acetic acid

c(CH₃COOH) = 0.2775 mol / 1.5 L = 0.185 M; concentration of acetic acid in solution

Ka(CH₃COOH) = 1.8·10⁻⁵

pKa = -logKa = 4.75

Henderson–Hasselbalch equation: pH = pKa + log(cs/ck).

pH = 4.75 + log(0.045M / 0.185M)

pH = 4.14; potential of hydrogen

More about sodium acetate: brainly.com/question/24671704

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8 0
1 year ago
SIGNIFICANT FIGURES ARE FIGURES WITH
nexus9112 [7]

Answer:

All zeros between other significant digits are significant. The number of significant figures is determined by starting with the leftmost non-zero digit. The leftmost non-zero digit is sometimes called the most significant digit or the most significant figure. For example, in the number 0.004205, the '4' is the most significant figure.

Explanation:

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