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8090 [49]
4 years ago
12

At what temperature does a solid turn into a liquid

Chemistry
2 answers:
Lostsunrise [7]4 years ago
6 0

Answer:

0°C

<h3>Hope this helps </h3><h3>Do mark as brainliest </h3>

Lapatulllka [165]4 years ago
3 0

Answer:

a little over 0 degrease cel

Explanation:

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Which region of the electromagnetic spectrum is used by doctors to view the skeletal structure of the human anatomy? A) X-Rays B
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The order of increasing wavelength (and decreasing energy) of the given radiations is:

Gamma Rays > X-Rays > Visible Light > Radio waves

X-rays due to the short wavelength and higher energies have the ability to penetrate through soft tissues like the skin or get absorbed by hard tissues like the bones. Thus, when the human anatomy is exposed to X-rays, bones appear white whereas the skin/tissues appear gray.

Ans: A)  X-rays are used by doctors to view skeletal structures

6 0
3 years ago
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A 100.0 mL solution containing 0.864 g of maleic acid (MW=116.072 g/mol) is titrated with 0.276 M KOH. Calculate the pH of the s
Lilit [14]

Answer:

pH = 1.32

Explanation:

                 H₂M + KOH ------------------------ HM⁻ + H₂O + K⁺

This problem involves a weak diprotic acid which we can solve by realizing they amount  to buffer solutions.  In the first  deprotonation if all the acid is not consumed we will have an equilibrium of a wak acid and its weak conjugate base. Lets see:

So first calculate the moles reacted and produced:

n H₂M = 0.864 g/mol x 1 mol/ 116.072 g  =  0.074 mol H₂M

54 mL x  1L / 1000 mL x 0. 0.276 moles/L = 0.015 mol KOH

it is clear that the maleic acid will not be completely consumed, hence treat it as an equilibrium problem of a buffer solution.

moles H₂M left = 0.074 - 0.015 = 0.059

moles HM⁻ produced = 0.015

Using the Henderson - Hasselbach equation to solve for pH:

ph = pKₐ + log ( HM⁻/ HA) = 1.92 + log ( 0.015 / 0.059) = 1.325

Notes: In the HH equation we used the moles of the species since the volume is the same and they will cancel out in the quotient.

For polyprotic acids the second or third deprotonation contribution to the pH when there is still unreacted acid ( Maleic in this case) unreacted.

           

3 0
3 years ago
The ph of an aqueous solution at 25.0°c is 10.66. what is the molarity of h+ in this solution? the ph of an aqueous solution at
love history [14]

Answer: The molarity of H^+ in this solution is 2.2\times 10^{-11}M

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

pH=-\log [H^+]

Given : pH = 10.66

Putting in the values:

10.66=-\log[H^+]

[H^+]=10^{-10.66}

[H^+]=2.2\times 10^{-11}

Thus the molarity of H^+ in this solution is 2.2\times 10^{-11}M

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4 years ago
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I hope my answer has come to your help. Thank you for posting your question here in Brainly. We hope to answer more of your questions and inquiries soon. Have a nice day ahead!
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