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vlabodo [156]
3 years ago
14

In atomic mass units, what is the average atomic mass of the atoms that make up boron (B)?

Chemistry
1 answer:
Annette [7]3 years ago
5 0
Atomic mass is the decimal number that is on the periodic table...

Boron's atomic mass is 10.81
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C. inorganic does not contain carbon
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Most of the high-level radiation associated with nuclear energy is
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Consider the nuclear equation below. Superscript 235 subscript 92 upper U right arrow superscript 4 subscript 2 upper H e. What
Leto [7]

Answer: The nuclide symbol of X is ^{231}_{90}\textrm{Th}

Explanation:

The given nuclear reaction is a type of alpha decay process. In this process, the nucleus decays by releasing an alpha particle. The mass number of the nucleus is reduced by 4 units and atomic number is also decreased by 2 units. The particle released is a helium nucleus.

The general equation representing alpha decay process is:

_{Z}^{A}\textrm{X}\rightarrow _{Z-2}^{A-4}\textrm{Y}+_2^4\textrm{He}

For the given equation :

^{235}_{92}\textrm{U}\rightarrow ^{A}_{Z}\textrm{X}+^4_2\textrm{He}

As the atomic number and mass number must be equal on both sides of the nuclear equation:

^{235}_{92}\textrm{U}\rightarrow ^{231}_{90}\textrm{Th}+^4_2\textrm{He}

Thus the nuclide symbol of X is ^{231}_{90}\textrm{Th}

5 0
3 years ago
What is the difference between a strong acid and a weak acid?
Jobisdone [24]

Answer:

The 3rd choice

Explanation:

A strong acid ionises COMPLETELY in water to produce high concentration of hydrogen ions

A weak acid ionises PARTIALLY in water to produce low concentration of hydrogen ions

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A chemist dissolves 797. mg of pure barium hydroxide in enough water to make up 60. mL of solution. Calculate the pH of the solu
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Answer:

13.20

Explanation:

Step 1: Calculate the moles of Ba(OH)₂

The molar mass of Ba(OH)₂ is 171.34 g/mol.

0.797 g × 1 mol/171.34 g = 4.65 × 10⁻³ mol

Step 2: Calculate the molar concentration of Ba(OH)₂

Molarity is equal to the moles of solute divided by the liters of solution.

[Ba(OH)₂] = 4.65 × 10⁻³ mol/60 × 10⁻³ L = 0.078 M

Step 3: Calculate [OH⁻]

Ba(OH)₂ is a strong base according to the following equation.

Ba(OH)₂ ⇒ Ba²⁺ + 2 OH⁻

The concentration of OH⁻ is 2/1 × 0.078 M = 0.16 M

Step 4: Calculate the pOH

pOH = -log OH⁻ = -log 0.16 = 0.80

Step 5: Calculate the pH

We will use the following expression.

pH + pOH = 14

pH = 14 - 0.80 = 13.20

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