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3 years ago

Which radioisotope is naturally occurring?

Chemistry

1 answer:

Lena [83]3 years ago

5 0

Answer:

I think the answer is 13H

Explanation:

The best known example of a naturally-occurring radioisotope is uranium. All but 0.7 per cent of naturally-occurring uranium is uranium-238; the rest is the less stable, or more radioactive, uranium-235, which has three fewer neutrons in its nucleus.

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Consider the perbromate anion. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central a

Yanka [14]

Answer:

See explanation

Explanation:

The central atom in the perbromate ion is bromine. The chemical symbol of bromine is Br. There are no lone pairs around the central bromine atom. The ion is tetrahedral in shape hence we expect a bond angle of 109°. 27 which is the ideal tetrahedral bond angle. The actual bond angle of the prebromate ion is 109.5°. The perbromate ion is BrO4^-

The observed bond angle is very close to the ideal value because of the absence of lone pairs of electrons from the central atom in the ion.

8 0

3 years ago

Sodium sulfate is slowly added to a solution containing 0.0500 M Ca 2 + ( aq ) and 0.0390 M Ag + ( aq ) . What will be the conce

levacccp [35]

The given question is incomplete. The complete question is as follows.

Sodium sulfate is slowly added to a solution containing 0.0500 M $Ca^{2+}(aq)$ and 0.0390 M $Ag^{+}(aq)$ . What will be the concentration of $Ca^{2+}$ (aq) when $Ag_{2}SO_{4}(s)$ begins to precipitate? What percentage of the $Ca^{2+}(aq)$ can be separated from the Ag(aq) by selective precipitation?

Explanation:

The given reaction is as follows.

$Ag_{2}SO_{4} \rightleftharpoons 2Ag^{+} + SO^{2-}_{4}$

$[Ag^{+}]$ = 0.0390 M

When $Ag_{2}SO_{4}$ precipitates then expression for $K_{sp}$ will be as follows.

$K_{sp} = [Ag^{+}]^{2}[SO^{2-}_{4}]$

$1.20 \times 10^{-5} = (0.0390)^{2} \times [SO^{2-}_{4}]$

$[SO^{2-}_{4}]$ = 0.00788 M

Now, equation for dissociation of calcium sulfate is as follows.

$CaSO_{4} \rightleftharpoons Ca^{2+} + SO^{2-}_{4}$

$K_{sp} = [Ca^{2+}][SO^{2-}_{4}]$

$4.93 \times 10^{-5} = [Ca^{2+}] \times 0.00788$

$[Ca^{2+}]$ = 0.00625 M

Now, we will calculate the percentage of $Ca^{2+}$ remaining in the solution as follows.

$\frac{0.00625}{0.05} \times 100$

= 12.5%

And, the percentage of $Ca^{2+}$ that can be separated is as follows.

100 - 12.5

= 87.5%

Thus, we can conclude that 87.5% will be the concentration of $Ca^{2+}(aq)$ when $Ag_{2}SO_{4}(s)$ begins to precipitate.

4 0

3 years ago

Lysol Power Toilet Bowl Cleaner contains 9.5% hydrochloric acid. Explain why this would be necessary to clean toilet bowls that

Romashka [77]

Answer:

The acid will absolutely remove the hard water deposits that are trapping the stains. The longer it soaks, the less you have to scrub. It works for hard water stains, limescale, and rust!

Explanation:

hope this helped you out.

8 0

3 years ago

Can some one please help

Scilla [17]

Answer:

Chadwick-he discovered the neutron. He discovered this by demonstrating a neutral particle with a mass the same as a proton through a reaction between gramma Ray's and a wax sample.

Rutherford-he discovered the concept of radioactive half-life, the radioactive element radon, and named alpha and beta radiation.

j.j.Thompson discovered that atoms where made up of smaller components. This had major effects for the field of physics.

8 0

3 years ago

Read 2 more answers

Ok so the answer for this question, A student measured the mass of salt that can dissolve in 100 mL of water at five different t

Dmitriy789 [7]

Answer:

penguin

Explanation:

8 0

2 years ago