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mestny [16]
2 years ago
11

Can someone do these? Brainliest included

Chemistry
1 answer:
mixas84 [53]2 years ago
7 0

Answer:

Explanation:

6.         p⁺      e⁻

Ca²⁺    20     18

F⁻          9      10

O²⁻        8      10

Na⁺       11      10

7. Physical properties of matter are properties that can be measured or observed without matter changing to an entirely different substance. These include odor, boiling point, melting point, density, electrical conductivity and heat conductivity.

Separation of mixture:

Chromatography involves solvent separation on a solid medium.

Distillation takes advantage of differences in boiling points.

Evaporation removes a liquid from a solution to leave a solid material.

Filtration separates solids of different sizes.

Funnel partitioning with solvents. Solvent dissolves one component but not the other.

8.Bulk Elements => Carbon, Hydrogen, Oxygen, Nitrogen, Sulfur & Phosphouous

Microminerals are those minerals needed in less than 100 mg quantities. Trace minerals or trace elements are usually needed in microgram quantities. Microminerals include iron, zinc, copper, iodine, fluoride, chromium, cobalt, selenium, manganese, and molybdenum.

Diatomic Molecules => H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂

9. Electron Configurations

    Na: 1s²2s²2p⁶3s¹ => valence = 3s¹

    N:   1s²2s²2p³ => valence = 2s²2p³

    Al:  1s²2s²2p⁶3s²3p¹ => valence = 3s²3p¹

Valence is the highest principle quantum number (or, principle energy level  ~ ring) in the electron configurations.

10.moles of glucose = 450g/180.16 g/mol =2.50 moles

   C₂H₆O₂ = 2(12) + 6(1) + 2(16) = 24 + 6 + 32 = 62 g/mole

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4 0
3 years ago
What is the pH of a solution that is 0.40 M NaBrO and 0.50 M HBrO (hypobromous acid) (Ka for HBrO = 2.3 x 10^-9)
Pie

Answer

pH=8.5414

Procedure

The Henderson–Hasselbalch equation relates the pH of a chemical solution of a weak acid to the numerical value of the acid dissociation constant, Kₐ. In this equation, [HA] and [A⁻] refer to the equilibrium concentrations of the conjugate acid-base pair used to create the buffer solution.

pH = pKa + log₁₀ ([A⁻] / [HA])

Where

pH = acidity of a buffer solution

pKa = negative logarithm of Ka

Ka =acid disassociation constant

[HA]= concentration of an acid

[A⁻]= concentration of conjugate base

First, calculate the pKa

pKa=-log₁₀(Ka)= 8.6383

Then use the equation to get the pH (in this case the acid is HBrO)

pH=8.6383+\log_{10}(\frac{0.40\text{ M}}{0.50\text{ M}})=8.5414

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