When an electron moves from a lower to a higher energy level does the electron gain or lose Quantum of energy

A- south<br> B- north <br> C-west<br> D- east <br> Help ASAP no links or I’m reporting

Agata [3.3K]

Answer:

east

Explanation:

5 0

3 years ago

Determine the pH of a 2.8 ×10−4 M solution<br> of Ca(OH)2.

shepuryov [24]

Answer:

pH = 10.75

Explanation:

To solve this problem, we must find the molarity of [OH⁻]. With the molarity we can find the pOH = -log[OH⁻]

Using the equation:

pH = 14 - pOH

We can find the pH of the solution.

The molarity of Ca(OH)₂ is 2.8x10⁻⁴M, as there are 2 moles of OH⁻ in 1 mole of Ca(OH)₂, the molarity of [OH⁻] is 2*2.8x10⁻⁴M = 5.6x10⁻⁴M

pOH is

pOH = -log 5.6x10⁻⁴M

pOH = 3.25

pH = 14-pOH

3 0

3 years ago

Which instrument is used to measure mass?

lara [203]

A triple beam balance is used to measure mass

5 0

3 years ago

Read 2 more answers

Push your palms again a wall. What happened

kondaur [170]

Answer:

It felt good!!!

Why do you ask??

3 0

3 years ago

What is the most soluble salt of the following set? What is the most soluble salt of the following set?

DiKsa [7]

Answer:

(c) $AgCN\ (K_{sp} =6.0\times 10^{-17})$

Explanation:

The solubility product of a solid is the amount of solid dissociates into its respective ions in the solution. Thus more the value of the Ksp, the more is the salt soluble in the solvent.

So, Given that:-

$Sn(OH)_2\ (K_{sp} =1.6\times 10^{-19})$

$Al(OH)_3\ (K_{sp} =1.9\times 10^{-33})$

$AgCN\ (K_{sp} =6.0\times 10^{-17})$

$Fe(OH)_3\ (K_{sp} =2.6\times 10^{-39})$

The salt having highest value of Ksp is AgCN. So, it is most soluble.

4 0

3 years ago