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disa [49]
3 years ago
11

Five different substances are given to you to be dissolved in water. which substances are most likely to undergo dissolution in

water? check all that apply. view available hint(s) check all that apply. ethanol, ch3ch2oh potassium fluoride, kf octane, c8h18 toluene, c7h8 sodium iodide, nai
Chemistry
2 answers:
almond37 [142]3 years ago
7 0

\boxed{{\text{Ethanol, potassium fluoride and sodium iodide}}} are most likely to undergo dissolution in water.

Further explanation:

Solubility is the property of substance as a result of which it has a tendency to dissolve in other substances. It is measured in terms of the maximum amount of solute that can be dissolved in the given amount of solvent.

“Like dissolves like” is a general rule that is used to predict whether the substance is soluble in the given solvent or not.

Water is composed of one oxygen and two hydrogen atoms. Since O is more electronegative than H, water has some net dipole moment that is directed towards oxygen atom. So water is a polar molecule.

Ethanol \left( {{\text{C}}{{\text{H}}_3}{\text{C}}{{\text{H}}_2}{\text{OH}}} \right) has a -OH group whose oxygen forms hydrogen bonding with the hydrogen atom of the water molecule and therefore ethanol is dissolved in water.

Potassium fluoride is an ionic compound that is composed of {{\text{K}}^ + } and {{\text{F}}^ - } ions. Water is a polar molecule that has {{\text{H}}^ + } and {{\text{F}}^ - } ions in it. So   is surrounded by {\text{O}}{{\text{H}}^ - } and {{\text{F}}^ - } is surrounded by {{\text{H}}^ + } ions and therefore KF is dissolved in water.

Octane \left( {{{\text{C}}_{\text{8}}}{{\text{H}}_{{\text{18}}}}} \right) is a hydrocarbon of eight carbon atoms and is non-polar in nature. So it does not dissolve in water.

Toluene \left( {{{\text{C}}_{\text{7}}}{{\text{H}}_{\text{8}}}} \right) is an aromatic hydrocarbon that is non-polar in nature. So it does not dissolve in water.

Sodium iodide is an ionic compound that is composed of   and   ions. Water is a polar molecule that has {{\text{H}}^ + } and {\text{O}}{{\text{H}}^ - } ions in it. So {\text{N}}{{\text{a}}^ + } is surrounded by {\text{O}}{{\text{H}}^ - } and {{\text{I}}^ - } is surrounded by {{\text{H}}^ + } ions and therefore NaI is dissolved in water.

Therefore ethanol, potassium fluoride and sodium iodide are dissolved in water.

Learn more:

  1. Identification of ionic bonding: brainly.com/question/1603987
  2. What type of bond exists between phosphorus and chlorine? brainly.com/question/81715

Answer details:

Grade: High School

Chapter: Ionic and covalent compounds

Subject: Chemistry

Keywords: ethanol, potassium fluoride, sodium iodide, toluene, octane, water, polar, non-polar, hydrocarbon, dipole moment, NaI, KF, CH3CH2OH, C8H18, C7H8.

AlladinOne [14]3 years ago
5 0
Correct Answer: P<span>otassium Fluoride (KF) and sodium iodide (NaI)

Reason: 
Ionic compounds tends to undergo dissolution in aqueous medium. This results generation of ions. On other hand, covalent compounds donot generate ions in aqueous medium.

In present case, </span>Potassium Fluoride (KF) and sodium iodide (NaI) are ionic compounds. Hence, when dissolved in water, these <span>substances are most likely to undergo dissolution.</span>
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Answer:

Molar mass of the gas = 15.15 g/mol

Explanation:

PV = nRT

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698\;torr = 698\times0.00131579 = 0.9184\;atm

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Now, PV = nRT

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n = \frac{0.9184\times48.7}{0.082057\times384.15}

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8 0
3 years ago
1. Calculate the concentration of hydronium ion of both buffer solutions at their starting pHs. Calculate the moles of hydronium
lilavasa [31]

Answer:

This question is incomplete, here's the complete question:

1. Calculate the concentration of hydronium ion of both buffer solutions at their starting pHs. Calculate the moles of hydronium ion present in 20.0 mL of each buffer.

Buffer A

Mass of sodium acetate used: 0.3730 g

Actual ph of the buffer 5.27

volume of the buffer used in buffer capacity titration 20.0 mL

Concentration of standardized NaOH 0.100M

moles of Naoh needed to change the ph by 1 unit for the buffer 0.00095mol

the buffer capacity 0.0475 M

Buffer B

Mass of sodium acetate used 1.12 g

Actual pH of the buffer 5.34

Volume of the buffer used in buffer capacity titration 20.0 mL

Concentration if standardized NaOH 0.100 M

moles of Naoh needed to change the ph by 1 unit 0.0019 mol

the buffer capacity 0.095 M

2.) A change of pH by 1 unit means a change in hydronium ion concentration by a factor of 10. Calculate the number of moles of NaOH that would theoretically be needed to decrease the moles of hydronium you calculated in #1 by a factor of 10 for each buffer. Are there any differences between your experimental results and the theoretical calculation?

3.) which buffer had a higher buffer capacity? Why?

Explanation:

Formula,

moles = grams/molar mass

molarity = moles/L of solution

1. Buffer A

molarity of NaC2H3O2 = 0.3731 g/82.03 g/mol x 0.02 L = 0.23 M

molarity of HC2H3O2 = 0. 1 M

Initial pH

pH = pKa + log(base/acid)

= 4.74 + log(0.23/0.1)

= 5.10

pH = -log[H3O+]

[H3O+] = 7.91 x 10^-6 M

In 20 ml buffer,

moles of H3O+ = 7.91 x 10^-6 M x 0.02 L

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Buffer B

molarity of NaC2H3O2 = 1.12 g/82.03 g/mol x 0.02 L = 0.68 M

molarity of HC2H3O2 = 0.3 M

Initial pH

pH = pKa + log(base/acid)

= 4.74 + log(0.68/0.3)

= 5.10

pH = -log[H3O+]

[H3O+] = 7.91 x 10^-6 M

In 20 ml buffer,

moles of H3O+ = 7.91 x 10^-6 M x 0.02 L

= 1.58 x 10^-7 mol

2. let x moles of NaOH is added,

Buffer A,

pH = 5.10

[H3O+] = 7.91 x 10^-6 M

new pH = 4.10

new [H3O+] = 7.91 x 10^-5 M

moles of NaOH to be added = (7.91 x 10^-5 - 7.91 x 10^-6) x 0.02 L

= 1.42 x 10^-6 mol

3. Buffer B with greater concentration of NaC2H3O2 and HC2H3O2 has higher buffer capacity as it resists pH change to a wider range due to addition of acid or base to the system as compared to low concentration of Buffer A

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